Are you excitedly awaiting the 2023 NPSC Preliminary Exam? Obtaining the NPSC Preliminary Admit Card 2023 is the initial step towards achieving your ideal career with the Nagaland Public Service Commission. In this article, we will provide you with all the pertinent details regarding the NPSC Preliminary Admit Card, including the direct download link from the official website, @npsc.nagaland.gov.in.
NPSC Preliminary Admit Card 2023 and Hall Ticket for Preliminary Exam Direct Link at npsc.nagaland.gov.in
The NPSC Preliminary Admit Card 2023 is a crucial document that every applicant must possess in order to sit for the NPSC Preliminary Exam. It serves as your admission ticket to the examination room and contains vital information such as your name, portrait, exam location, and timings. Without the NPSC Preliminary Exam Admit Card, you will not be permitted to take the examination.
To obtain the NPSC Preliminary Admit Card 2023, you must visit the organization’s official website, @npsc.nagaland.gov.in. It is the only authorized location to procure a hall ticket. You will need your authentication credentials to access your admit card, so be sure to keep them handy.
NPSC Preliminary Admit Card 2023: A Ticket to Your Dreams
The NPSC Preliminary Admit Card 2023 is a ticket to your dreams of securing a government job in Nagaland. This essential document ensures that you are eligible to participate in the NPSC Prelims Exam, which is a crucial stage in the selection process. Without the admit card, you will not be allowed to enter the examination hall or take the test. Therefore, it is imperative to download and carry your NPSC Preliminary Admit Card 2023 on the day of the exam.
Here is a detailed guide on how to obtain your NPSC Prelims Exam Admit Card:
- The official NPSC website is npsc.nagaland.gov.in.
- On the homepage, locate the “Download Admit Card” section.
- Click the link to continue.
- Include your registration number and password in your login credentials.
- Verify the particulars and submit the data.
- Your NPSC Preliminary Call Letter 2023 will appear on the screen.
- Examine the details listed on the admit card with care.
- Download and save the admission ticket.
- Make a copy of the admission ticket for future reference.
- Your NPSC Preliminary Admit Card 2023 will be displayed on the screen.
- Carefully review all the details mentioned on the admit card, including your name, photograph, examination date, time, and venue.
Verify that you’ve double-checked all the information on your NPSC Preliminary Admit Card 2023. If you discover any discrepancies or errors, contact the NPSC promptly so that they can be rectified.
Frequently Asked Questions (FAQs)
Q1. When can I acquire the NPSC Preliminary Admit Card for the 2023 exam?
It is anticipated that the NPSC Preliminary Admit Card 2023 will be available for download approximately two weeks prior to the exam date. Visit the NPSC’s official website, @npsc.nagaland.gov.in, for the most recent updates and announcements regarding the issue of the admit card.
Q2. Can I obtain the NPSC Preliminary Exam Admit Card offline?
No, the only way to obtain the NPSC Preliminary Admit Card 2023 is online. To obtain your hall ticket, you must visit the official website of NPSC, @npsc.nagaland.gov.in. The commission does not offer offline distribution of admissions tickets.
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August 3, 2023Hsslive.net SCERT Kerala Class 12th Mathematics syllabus for the year 2023. It mentions that the syllabus gives a clear picture of the number of units and chapters covered, and the time allotted for each month to ensure a balanced course of study. Having a copy of the syllabus allows students to create their action plan accordingly.
To prepare for the class 12th Kerala Board examination, it is recommended to have in-depth knowledge of the Kerala Board Syllabus 12th Standard Textbooks. The syllabus is designed to help students shine in the HSE plus 2 exam.Table of ContentsKerala Plus one Higher Secondary Class 12th Math’s Syllabus PDF The Maths textbooks for Class 12 are divided into two parts:SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 1SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 2
Kerala Plus one Higher Secondary Class 12th Math’s Syllabus PDF Based on
Kerala StateClasses
Plus one or Class 11thSubject
MathsState Board
Kerala Board (DHSE)Format
PDF & WebBook uses
SCERT & NCERT
The Maths textbooks for Class 12 are divided into two parts:SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 1
SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 2The website only mentions that the SCERT Kerala Class 12 Maths textbooks are updated and thoroughly revised according to the latest exam pattern and Kerala State syllabus.
SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 1Chapter Number
Chapter Name
Topics1
Relations and Functions
Introduction, Types of Relations, Types of Functions, Composition of Functions and Invertible Function, Binary Operations2
Inverse Trigonometric Functions
Introduction, Basic Concepts, Properties of Inverse Trigonometric Functions3
Matrices
Introduction, Matrix, Types of Matrices, Operations on Matrices, Transpose of a Matrix, Symmetric and Skew Symmetric Matrices, Elementary Operation (Transformation) of a Matrix, Invertible Matrices4
Determinants
Introduction, Determinant, Properties of Determinants, Area of a Triangle, Minors and Cofactors, Adjoint and Inverse of a Matrix, Applications of Determinants and Matrices5
Continuity and Differentiability
Introduction, Continuity, Differentiability, Exponential and Logarithmic Functions, Logarithmic Differentiation, Derivatives of Functions in Parametric Forms, Second Order Derivative, Mean Value Theorem6
Application of Derivatives
Introduction, Rate of Change of Quantities, Increasing and Decreasing Functions, Tangents and Normals, Approximations, Maxima and MinimaAppendix 1
Proofs in Mathematics
Introduction, What is a Proof?Appendix 2
Mathematical Modelling
Introduction, Why Mathematical Modelling?, Principles of Mathematical Modelling
SCERT Kerala State Syllabus 12th Standard Maths Textbooks Part 2Chapter Number
Chapter
Topics7
Integrals
– Introduction, Integration as an Inverse Process of Differentiation, Methods of Integration, Integrals of Some Particular Functions, Integration by Partial Fractions, Integration by Parts, Definite Integral, Fundamental Theorem of Calculus, Evaluation of Definite Integrals by Substitution, Some Properties of Definite Integrals8
Application of Integrals
– Introduction, Area under Simple Curves9
Differential Equations
– Introduction, Basic Concepts, General and Particular Solutions of a Differential Equation, Methods of Solving First Order, First Degree Differential Equations10
Vector Algebra
– Introduction, Some Basic Concepts, Types of Vectors, Addition of Vectors, Multiplication of a Vector by a Scalar, Product of Two Vectors11
Three Dimensional Geometry
– Introduction, Direction Cosines and Direction Ratios of a Line, Equation of a Line in Space, Angle between Two Lines, Shortest Distance between Two Lines12
Linear Programming
– Introduction, Linear Programming Problem and its Mathematical Formulation13
Probability
– Introduction, Conditional Probability, Multiplication Theorem on Probability, Independent Events, Bayes’ Theorem
Official syllabus from your State Council of Educational Research and Training (SCERT) or educational institution for the most accurate and up-to-date information. [...]Read more...
August 3, 2023Higher Secondary Plus One Chemistry Notes for Kerala Board Syllabus. It’s a fascinating subject that helps us understand the world around us at a molecular level. Hsslive.net provided Plus One Chemistry notes for students in their higher secondary years in two languages English Medium & Malayalam Medium. Topics that are usually covered in the first year of chemistry at the higher secondary level. Student also Download Notes In Pdf in both English & Malayalam. Notes are well researched trusted buy qualified teacher’s and Made by Sudha Tiwari, Praveen K.L, Krishnappa.Table of ContentsKerala Plus one Higher Secondary Chemistry PDF Notes Class 11thFAQs
Kerala Plus one Higher Secondary Chemistry PDF Notes Class 11thBased on
Kerala StateClasses
Plus one or Class 11thSubject
ChemistryState Board
Kerala Board (DHSE)Format
PDF & WebBook uses
SCERT & NCERTThese study notes have been meticulously crafted to align perfectly with the NCERT syllabus, making them exceptionally valuable for both Kerala Syllabus and CBSE students with knowledge cultivated over two decades of teaching experience. Our aim is to equip you with the best possible resources so that you can excel and flourish in your academic pursuits. Let the joy of learning take over as you unlock the boundless potential of Chemistry. Best wishes for an enriching learning experience with Hsslive.net.Chapter
Topics in Details1. Some Basic Concepts of Chemistry
Importance of Chemistry, Nature of Matter, Properties of Matter and their Measurements, Uncertainty in Measurement, Laws of Chemical Combinations, Dalton’s Atomic Theory, Atomic and Molecular Masses, Mole Concept and Molar Masses, Percentage Composition, Empirical and Molecular Formula, Stoichiometry2. Structure of Atom
Discovery of Electron, Proton and Neutron, Atomic Number, Isotopes and Isobars, Thomson’s Model and its Limitations, Rutherford’s Model and its Limitations, Bohr’s Model and its Limitations, Concept of Shells and Subshells, Dual Nature of Matter and Light, de Broglie’s Relationship, Heisenberg Uncertainty Principle, Concept of Orbitals, Quantum Numbers, Shapes of s, p and d Orbitals, Rules for Filling Electrons in Orbitals – Aufbau Principle, Pauli’s Exclusion Principle and Hund’s Rule, Electronic Configuration of Atoms, Stability of Half-filled and Completely filled Orbitals3. Classification of Elements and Periodicity in Properties
Modern Periodic Law and the present form of the Periodic Table, Periodic Trends in Properties of Elements – Atomic Radii, Ionic Radii, Inert Gas Radii, Ionization Enthalpy, Electron Gain Enthalpy, Electronegativity, Valency4. Chemical Bonding and Molecular Structure
Kossel-Lewis Approach to Chemical Bonding, Ionic Bond, Covalent Bond, Bond Parameters, Limitations of Octet Rule, Lewis Structures, Formal Charge, Resonance, VSEPR Theory, Concept of Hybridization involving s, p and d orbitals and shapes of some simple molecules, Molecular Orbital Theory of Homonuclear Diatomic Molecules5. States of Matter: Gases and Liquids
Three States of Matter, Intermolecular Interactions, Types of Bonding, Melting and Boiling Points, Role of Gas Laws in elucidating the concept of the molecule, Boyle’s Law, Charles Law, Gay Lussac’s Law, Avogadro’s Law, Ideal Behaviour, Empirical derivation of Gas Equation, Avogadro’s Number, Ideal Gas Equation, Kinetic Energy and Molecular Speeds, Real Gases, Deviation from Ideal Behaviour, Liquefaction of Gases, Liquid State6. Thermodynamics
Concepts of System and types of Systems, Surroundings, Work, Heat, Energy, Extensive and Intensive Properties, State Functions, First Law of Thermodynamics – Internal Energy and Enthalpy, Heat Capacity and Specific Heat, Measurement of ΔU and ΔH, Hess’s Law of Constant Heat Summation, Enthalpy of Bond Dissociation, Combustion, Formation, Atomization, Sublimation, Phase Transition, Ionization, Solution and Dilution7. Equilibrium
Equilibrium in Physical and Chemical Processes, Dynamic Nature of Equilibrium, Law of Mass Action, Equilibrium Constant, Factors Affecting Equilibria, Le Chatelier’s Principle, Ionic Equilibrium – Ionization of Acids and Bases, Strong and Weak Electrolytes, Degree of Ionization, Ionization of Polybasic Acids, Acid Strength, Concept of pH, Hydrolysis of Salts, Buffer Solution, Solubility Product, Common Ion Effect8. Redox Reactions
Concept of Oxidation and Reduction, Redox Reactions, Oxidation Number, Balancing Redox Reactions, Applications of Redox Reactions9. Hydrogen
Position of Hydrogen in Periodic Table, Occurrence, Isotopes, Preparation, Properties and Uses of Hydrogen, Hydrides – Ionic, Covalent and Interstitial, Water, Hydrogen Peroxide, Heavy Water, Hydrogen as a Fuel10. s-Block Elements (Alkali and Alkaline Earth Metals)
Group 1 and Group 2 Elements, General Introduction, Electronic Configuration, Occurrence, Anomalous Properties of the First Element of each Group, Diagonal Relationship, Trends in the Variation of Properties, Trends in Chemical Reactivity with Oxygen, Water, Hydrogen and Halogens, Uses11. Some p-Block Elements
General Introduction to p-Block Elements, Group 13 Elements: Boron – Electronic Configuration, Occurrence, Isolation, Physical and Chemical Properties, Some Important Compounds, Uses, Group 14 Elements: Carbon – Electronic Configuration, Occurrence, Physical and Chemical Properties, Uses, Some Important Compounds, Allotropes of Carbon12. Organic Chemistry – Some Basic Principles and Techniques
General Introduction, Methods of Purification, Qualitative and Quantitative Analysis, Classification and IUPAC Nomenclature of Organic Compounds, Electronic Displacements in a Covalent Bond, Homolytic and Heterolytic Fission of a Covalent Bond, Carbocations, Carbanions, Free Radicals, Electrophiles and Nucleophiles, Types of Organic Reactions13. Hydrocarbons
Classification of Hydrocarbons, Alkanes – Nomenclature, Isomerism, Conformational Isomerism, Physical Properties, Chemical Reactions, Alkenes – Nomenclature, Structure of Double Bond, Geometrical Isomerism, Physical Properties, Chemical Reactions, Alkynes – Nomenclature, Structure of Triple Bond, Physical Properties, Chemical Reactions, Aromatic Hydrocarbons – Nomenclature, Benzene – Resonance, Aromaticity, Chemical Properties, Directive Influence of Functional Group in Monosubstituted Benzene, Carcinogenicity and Toxicity14. Environmental Chemistry
Environmental Pollution, Atmospheric Pollution, Water Pollution, Soil Pollution, Marine Pollution, Noise Pollution, Thermal Pollution, Nuclear Hazards, Solid Waste Management, Role of the Individual in Prevention of Pollution, Sustainable Development
FAQs
What are the Higher Secondary Plus One Chemistry Notes?
Higher Secondary Plus One/Plus Two Chemistry Notes are comprehensive study materials that cover the entire chemistry syllabus for higher secondary students. They provide detailed explanations of core concepts, solved examples, and practice questions to help students prepare for their exams.
How can I effectively use the Higher Secondary Plus One Chemistry Notes for exam preparation?
Start by reading through the notes to understand the concepts. Then, solve the examples and practice questions to reinforce your understanding. Regular revision is key to retaining the information.
Are the Higher Secondary Plus One/Plus Two Chemistry Notes sufficient for exam preparation?
While the notes provide a comprehensive overview of the syllabus, it’s recommended to refer to standard textbooks for a more in-depth understanding. The notes should be used as a supplement to your regular study materials.
What topics are covered in the Higher Secondary Plus One/Plus Two Chemistry Notes?
The notes cover all the topics in the higher secondary chemistry syllabus, including atomic structure, chemical bonding, stoichiometry, states of matter, thermodynamics, electrochemistry, chemical kinetics, and organic chemistry. [...]Read more...
August 3, 2023Hsslive.net provided Plus One Chemistry notes for students in their higher secondary years in two languages English Medium & Malayalam Medium. Topics- “Law of Chemical Combination” that are usually covered in the first year of chemistry at the higher secondary levelTable of ContentsLaws of Chemical CombinationsLaw of Conservation of Mass:Law of Definite Proportions:Law of Multiple Proportions:Law of Reciprocal Proportions:
Laws of Chemical Combinations
The rules for how different elements can be put together to make compounds are called the laws of chemistry combinations. They are based on what experts who have studied the nature and behavior’s of matter have seen and done. These rules help us understand the composition and properties of compounds, as well as the stoichiometry and conservation of mass in chemical reactions. In this chapter, we will learn about four rules. These are:
Law of Conservation of Mass:
This law says that during a chemical reaction, matter can neither be made nor removed. In other words, in a chemical process, the total mass of the reactants is the same as the total mass of the products. In 1789, Antoine Lavoisier came up with this law and did a number of experiments to show it. He showed, for example, that when mercury oxide is burned, it breaks down into mercury and oxygen, and the amount of mercury and oxygen is the same as the amount of mercury oxide. !Mercury oxide decomposition)
We can do a simple experiment with a closed system, like a sealed flask or a balloon, to test this rule. We can burn a known amount of a fuel, like a strip of magnesium, in air or oxygen. Then, we can measure the mass of the result, like magnesium oxide, and compare it to the mass of the reactant at the beginning. As shown below, we will find that there is no change in mass. !Magnesium burning)
Law of Definite Proportions:
This law says that a given compound always has the same parts in the same fixed mass ratio, no matter where it came from or how it was made. For example, water always has 1 part hydrogen to 8 parts oxygen by mass. In 1799, Joseph Proust came up with this law and did several experiments to show it. For instance, he showed that the amount of copper, carbon, and oxygen in copper carbonate is always 5:2:3 by mass. !Copper carbonate)
To test this rule, we can do a simple experiment in which we use a known amount of a compound, like sodium chloride, and use electricity to separate its parts. Then we can measure how much sodium and chlorine were made and compare them to how much sodium chloride there was to start with. As shown below, we will find that they are in a set ratio. !Sodium chloride electrolysis)
Law of Multiple Proportions:
This law says that when two elements combine to make more than one compound, the masses of one element that combine with a set mass of the other element are in a simple ratio of whole numbers. Carbon and oxygen, for example, can join to make two different compounds: carbon monoxide (CO) and carbon dioxide (CO2). In each of these molecules, 12 g of carbon combines with either 16 g or 32 g of oxygen. 16:32, or 1:2, is the ratio of the amounts of oxygen that combine with a given amount of carbon. John Dalton came up with this law in 1803. He used it to back up his atomic theory. !Carbon and oxygen compounds)
To test this rule, we can do a simple experiment in which we mix a known amount of one element, like nitrogen gas, with different amounts of another element, like hydrogen gas. Then, we can compare the amounts of ammonia (NH3) and hydrazine (N2H4) that were made to the amounts of nitrogen and hydrogen that were used at the beginning. As shown below, we will find that they are in a simple ratio. !Nitrogen and hydrogen compounds)
Law of Reciprocal Proportions:
This law says that when two elements combine separately with a third element, the ratio of the masses in which they do so is either the same as or a simple multiple of the ratio in which they combine with each other. For example, hydrogen and oxygen can each join with nitrogen to make ammonia (NH3) and nitric oxide (NO), respectively. In these molecules, 14 grammes of nitrogen are mixed with 3 grammes of hydrogen and 8 grammes of oxygen. When hydrogen and oxygen combine with a set amount of nitrogen, the ratio of their masses is 3:8. This is the same number of hydrogen atoms and oxygen atoms that come together to make water. In 1792, Jeremias Richter came up with this rule. He used it to study how salts are made. !Hydrogen and oxygen compounds)
To test this rule, we can do a simple experiment with a known mass of one element, like carbon, and different masses of another element, like chlorine, that react with it separately. Then, we can compare the amounts of carbon tetrachloride (CCl4) and carbon monochloride (CCl) that were made to the amounts of carbon and chlorine that were used in the beginning. We will find that they are in a simple multiple of the ratio of how much carbon and chlorine are needed to make carbon dichloride (CCl2), as shown below. !Carbon and chlorine compounds)
In this chapter, we’ve learned the four rules of chemical combinations. They help us understand the parts and properties of compounds, as well as the stoichiometry and conservation of mass in chemical processes. I hope these notes were fun and that you learned something new. [...]Read more...
August 3, 2023Higher Secondary Plus One Chemistry Notes for Kerala Board Syllabus. It’s a fascinating subject that helps us understand the world around us at a molecular level. Hsslive.net provided Plus One Chemistry notes for students. Topics- “Some Basic Concepts of Chemistry” that are usually covered in the first year of chemistry at the higher secondary level. valuable for both Kerala Syllabus and CBSE students with knowledge cultivated over two decades of teaching experience.Table of ContentsSome Basic Concepts of ChemistryThe International System of Units (SI)Atomic Mass, Molecular Mass, Formula Mass, and Molar MassLaws of Chemical CombinationThe Mole ConceptConcentration of Solutions
Some Basic Concepts of Chemistry
Chemistry is the study of matter and the changes it can undergo. Matter is anything that has mass and occupies space. Matter can be classified into different types based on its physical state (solid, liquid, or gas), composition (element, compound, or mixture), and properties (physical or chemical).
Some basic concepts of chemistry that we will learn in this chapter are:The International System of Units (SI) and the rules for using them.
The concepts of atomic mass, molecular mass, formula mass, and molar mass.
The laws of chemical combination and their applications.
The mole concept and its relation to mass, volume, and number of particles.
The methods of expressing concentration of solutions.
The calculations involving stoichiometry and limiting reagents.The International System of Units (SI)
The International System of Units (SI) is a standard system of measurement that is widely used in science and engineering. It consists of seven base units and several derived units. The base units are:Metre (m) for length
Kilogram (kg) for mass
Second (s) for time
Ampere (A) for electric current
Kelvin (K) for temperature
Mole (mol) for amount of substance
Candela (cd) for luminous intensityThe derived units are obtained by combining the base units with appropriate prefixes and exponents. For example, the unit of force is newton (N), which is defined as kg m s-2.
Some rules for using the SI units are:Use a decimal point as the separator for fractional parts of a number.
Use a space to separate the digits into groups of three, starting from the decimal point.
Do not use commas or spaces within a number.
Use a space to separate the number and the unit symbol.
Do not use a period after the unit symbol unless it ends a sentence.
Use capital letters for unit symbols derived from proper names, such as N for newton or K for kelvin.
Use lowercase letters for unit symbols derived from common names, such as m for metre or s for second.
Do not use plural forms or hyphens for unit symbols, such as ms for milliseconds or kg-m for kilogram-metre.Atomic Mass, Molecular Mass, Formula Mass, and Molar Mass
The atomic mass of an any element is the average mass of its atoms relative to one-twelfth of the mass of a carbon-12 atom. It is called in atomic mass units (u), where 1 u = 1.66 x 10-27 kg. The atomic masses of different elements can be found in the periodic table.
The molecular mass of a any compound is the sum of the atomic masses of all the atoms in one molecule of the compound. It is also called in atomic mass units (u). For example, the molecular mass of water (H2O) is 2 x 1.008 u + 16.00 u = 18.016 u.
The formula mass of an ionic compounds is the sum of the atomic masses of all the ions present in one formula unit of the compound. It is also expressed in atomic mass units (u). For example, the formula mass of sodium chloride (NaCl) is 22.99 u + 35.45 u = 58.44 u.
The molar mass of a any substance is the mass of one mole of that substance. It is expressed in grams per mole (g mol-1). One mole of a substance contains 6.022 x 1023 particles (atoms, molecules, or ions) of that substance. This number is called Avogadro’s constant (NA). The molar mass of a substance is equal to its atomic mass, molecular mass, or formula mass in grams. For example, the molar mass of water is 18.016 g mol-1 and the molar mass of sodium chloride is 58.44 g mol-1.
Laws of Chemical Combination
There are four laws that govern the combination of different elements to form compounds. They are:Law of Conservation Of Mass: This law states that matter can neither be created nor destroyed in a chemical reactionyouca, n also say that total mass of the reactants is equal to the total mass of the final products in a chemical reaction.
Law of Definite Proportions: This law states that a given compound always contains the same elements in the same fixed ratio by mass, regardless of its source or method of preparation. For example, water always contains hydrogen and oxygen in the ratio 1:8 by mass.
Law of Multiple Proportions: This law states that when two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in a simple ratio of whole numbers. For example, carbon and oxygen can combine to form two compounds: carbon monoxide (CO) and carbon dioxide (CO2). In these compounds, 12 g of carbon combine with 16 g and 32 g of oxygen, respectively. The ratio of the masses of oxygen that combine with a fixed mass of carbon is 16:32 or 1:2.
Law of Reciprocal Proportions: This law states that when two elements combine separately with a third element, the ratio of the masses in which they do so is either the same or a simple multiple of the ratio in which they combine with each other. For example, hydrogen and oxygen can combine separately with nitrogen to form ammonia (NH3) and nitric oxide (NO), respectively. In these compounds, 14 g of nitrogen combine with 3 g and 8 g of hydrogen and oxygen, respectively. The ratio of the masses of hydrogen and oxygen that combined with a fixed mass of nitrogen is 3:8. This is the same as the ratio in which hydrogen and oxygen combine with each other to form water.The Mole Concept
The mole concept is a convenient way of expressing the amount of a substance in terms of its particles. One mole of a substance is defined as the amount that contains as many particles as there are atoms in 12 g of carbon-12. This number is equal to Avogadro’s constant (NA), which is 6.022 x 1023. The mole concept can be used to relate the mass, volume, and number of particles of a substance.Mass-Mole Relationship: The mass-mole relationship is based on the molar mass of a any substance, which is the mass of one mole of that substance. The molar mass can be calculated by multiplying the atomic mass, molecular mass, or formula mass by NA. The mass-mole relationship can be expressed as:
Mass (g) = Number of moles (mol) x Molar mass (g mol-1)
For example, to calculate the mass of 2 moles of water, we use the formula:
Mass (g) = 2 mol x 18.016 g mol-1 = 36.032 g
Volume-Mole Relationship: The volume-mole relationship is based on the molar volume of a gas, which is the volume occupied by one mole of any gas at standard temperature and pressure (STP). STP is defined as 0°C (273 K) and 1 atm (101.3 kPa). The molar volume of any gas at STP is 22.4 L mol-1. The volume-mole relationship can be expressed as:
Volume (L) = Number of moles (mol) x Molar volume (L mol-1)
For example, to calculate the volume occupied by 0.5 moles of oxygen gas at STP, we use the formula:
Volume (L) = 0.5 mol x 22.4 L mol-1 = 11.2 L
Particle-Mole Relationship: The particle-mole relationship is based on Avogadro’s constant (NA), which is the number of particles in one mole of a substance. The particles can be atoms, molecules, or ions, depending on the nature of the substance. The particle-mole relationship can be expressed as:
Number of particles = Number of moles (mol) x Avogadro’s constant (NA)
For example, to calculate the number of molecules in 3 moles of carbon dioxide, we use the formula:
Number of molecules = 3 mol x 6.022 x 1023 = 1.807 x 1024Concentration of Solutions
A solution is a homogeneous mixture of two or more substances. The substance that dissolves in another substance is called the solute, and the substance that does the dissolved is called the solvent. The concentration of a solution is a measure of how much solute is present in a given amount of solvent or solution. There are different ways of expressing concentration, such as:Mass Percent: Mass % is defined as the mass of solute per 100 g of solution. It can be calculated by this formula:
Mass percent (%) = Mass of solute (g) / Mass of solution (g) x 100
For example, to calculate the mass percent of sodium chloride in a solution containing 5 g [...]Read more...
August 3, 2023Hsslive.net provided Plus One Chemistry notes for students in their higher secondary years in two languages English Medium & Malayalam Medium. Topics- “Importance of Chemistry” that are usually covered in the first year of chemistry at the higher secondary level. valuable for both Kerala Syllabus and CBSE students with knowledge cultivated over two decades of teaching experience.
Importance of Chemistry
1. Matter and Its Classification
Matter, the substance that occupies space and possesses mass, is classified into three states: solid, liquid, and gas. For example:Ice (solid) – H2O in a solid state
Water (liquid) – H2O in a liquid state
Water vapor (gas) – H2O in a gaseous state2. Laws of Chemical Combinations
Chemical reactions follow well-defined laws, which include:
a) Law of Conservation of Mass: The total mass of substances in a chemical reaction remains constant, indicating that atoms are neither created nor destroyed during the process.
Example: When hydrogen (H2) reacts with oxygen (O2) to form water (H2O), the total mass of reactants (H2 + O2) is equal to the total mass of products (H2O).
b) Law of Definite Proportions: Elements combine in fixed mass ratios to form compounds, leading to their unique identities.
Example: Water (H2O) always has a fixed mass ratio of hydrogen and oxygen, regardless of its source.
c) Law of Multiple Proportions: When two elements form more than one compound, the ratios of masses of one element to a fixed mass of the other element are in small whole numbers.
Example: Carbon and oxygen can form two compounds: carbon monoxide (CO) and carbon dioxide (CO2). The mass ratio of oxygen to carbon in CO2 is twice that of CO.
3. Atomic and Molecular Mass
Understanding the atomic and molecular masses is vital in quantifying substances’ amount in chemical reactions. The atomic mass unit (amu) is used to express these masses relative to the carbon-12 isotope.
Example: The atomic mass of carbon is 12.011 amu, while the molecular mass of water (H2O) is (2×1.008 amu) + 16.00 amu = 18.016 amu.
4. Mole Concept
The mole concept bridges the macroscopic and microscopic worlds by connecting mass, number of particles, and Avogadro’s number (6.022 x 10^23). It enables easy conversions between mass, moles, and particles.
Example: One mole of any substance contains Avogadro’s number of particles, which is approximately 6.022 x 10^23. Therefore, one mole of atoms of an element has a mass equal to its atomic mass in grams.
Numerical Example: Calculate the number of moles in 60 grams of carbon dioxide (CO2).
Solution: Molar mass of CO2 = (12.01 g/mol + 2×16.00 g/mol) = 44.01 g/mol Number of moles = Mass of CO2 / Molar mass of CO2 Number of moles = 60 g / 44.01 g/mol ≈ 1.36 moles [...]Read more...
August 3, 2023Welcome to the captivating world of Chemistry, where we unravel the mysteries of matter – the building blocks of the universe. In this chapter, “Some Basic Concepts of Chemistry – Nature of Matter,” we embark on a journey of exploration to understand the fundamental nature and characteristics of matter.
1. Atomic Structure: The Foundation of Matter
At the heart of matter lies the concept of atomic structure. Imagine atoms as tiny, dynamic universes with their subatomic planets. The nucleus, composed of protons and neutrons, anchors the electrons in their orbits. This delicate balance between positive and negative charges governs the behavior of matter at the atomic level.
2. Elements and Compounds: The Diversity of Matter
In the realm of Chemistry, matter manifests itself as elements and compounds. Elements are like the unique personalities of the periodic table, with each possessing its distinct identity. On the other hand, compounds are a marriage of different elements, combining their characteristics to create novel substances.
For instance, oxygen (O2) is an element, a life-sustaining gas crucial for respiration. However, when two hydrogen atoms join forces with an oxygen atom, they create the remarkable compound, water (H2O), essential for life as we know it.
3. States of Matter: The Ever-Changing Dance
Matter is a performer of a beautiful dance, transitioning effortlessly between three states – solid, liquid, and gas. In the solid state, particles are locked in an elegant arrangement, creating distinct shapes and structures. When warmed by energy, matter gracefully transforms into the fluid state of liquids, where particles move with a newfound freedom. Finally, with a surge of energy, matter takes to the stage as a vibrant gas, where particles move unchained and unrestrained.
4. Physical and Chemical Properties: Unraveling the Essence
Every substance exhibits its unique personality through physical and chemical properties. Physical properties, like a distinctive fingerprint, can be observed without changing the substance’s composition. These characteristics include color, odor, density, and melting/boiling points.
As an analogy, consider a rose – its color, fragrance, and shape are all physical properties that distinguish it from other flowers.
Conversely, chemical properties are more like the hidden talents of a performer. They reveal themselves during a chemical reaction when substances interact to form new compounds. These properties define the substance’s reactivity and ability to undergo transformations.
Conclusion: Unleashing the Marvels of Matter
As we conclude our journey into the “Nature of Matter,” I encourage you to cherish the beauty of Chemistry’s foundational concepts. Embrace the wonders of atomic structure, elements, compounds, and states of matter, for they hold the keys to unraveling the secrets of our universe. [...]Read more...
August 3, 2023So will IIT JEE is tough and it is not easy to score well if you are not following the discipline the time table the structure of course your Physical health and of course your mental health but I want to remind each one of you giving this examination that no matter who you are no matter where you from if you follow the tips that is being told you in this article you will definitely make it and make it big.Table of ContentsWhat is IIT JEE? What its importance? What things an average student should keep in mind while preparing for IIT JEE exam, so that his preparation can be good and mistakes are less?Start Preparing at the right time:-Understand the Syllabus well:-Keep in mind the marks and Weightage:-Select the High Study Material:-Have a Proper Time Management:-
What is IIT JEE? What its importance?
IIT JEE Indian Institute of Technology is the dream destination of those students who wants to advance in engineering and technology education because of such a world class educational platform which comes provider of quality education and best engineering education and IIT Delhi work on high positions in India and abroad. If you are doing this, then every student with an interest in technology wants to reach IIT, then it should not be surprising because everyone wants to make a secure and precious career.
But what happens by wanting, friends get it only to those who are deserving. And the question is, who is deserving, the one who performs the best at the right time with the right sprite while keeping the right attitude, although you know that every year you understand that lakhs of students. They become a part of this, but they get the victory, if they have A to Z knowledge about it and the name of this exam is IIT JEE National level engineering exam, which has two stages, one is JEE Mains and the other is JEE Advanced.
Well, you must know all this about it, yet we are telling you once more, JEE Main is such an exam in which the selected students are eligible for JEE Advanced and those who get selected in JEE Advanced, that race. are the winners of the IITs because after winning this highly tough race, they get admission in IIT, every year IIT conducts JEE to select the best student for 4 years B Tech, B Pharma 5 years B Architecture, Integrated MSc and MTech course.
Well, you must have known about what is IIT JEE and its importance, but today again a main reason has been done to tell it to remind you that the competition is very high in this exam, it is very tough, the ignition will not work at all without strategy selection. Chances cannot be made and even if there is no motivation, things will not work, so remember that both your effort and intention should be firm, if you share that your intentions are strong, then in today’s article we will tell you that one How the average student cracks IIT JEE?
Let us know,
What things an average student should keep in mind while preparing for IIT JEE exam, so that his preparation can be good and mistakes are less?
Start Preparing at the right time:-
Suppose your aim is to clear IIT JEE in the first attempt itself but you have to start preparing for it well in advance and if you are doing consistent practice for a long time then you will not face any further problem as your syllabus is also completed. You will get sufficient time to solve your problem sort out and your notes will be well maintained then tell whether it will be easy for you to crack the exam or not. So for this you start preparing for JEE from class 11th itself and if you start preparation before that then it will be easy for you to follow the time management discipline and routine which is the basic requirement to clear this exam.
Understand the Syllabus well:-
First of all, understand the syllabus well, consider that you do not want to waste much time while preparing, but you cannot do anything without checking the syllabus without understanding it properly, then it will not be the right way for your preparation because preparing for the exam. Before starting, you should know what is coming in the exam, what type of questions will be asked, so understand your syllabus well, keep a copy of it on the study table with you and after that think of getting ready because many times students skip this major step in a hurry but you will not make such mistake at all.
Keep in mind the marks and Weightage:-
While studying the syllabus, you have to understand well that how much is the chapter vice weightage because for each chapter the marks release is different and it doesn’t matter how much knowledge you have but this thing is more important for the exam. It is that how well you are covering the syllabus, so focus more on the unit with height weight age and then on the low weight age chapter.
Like in JEE Mains,
Physics Optics has 10% weightage, Electronic Devices has 14% weightage while Gravitation has 2% weightage.
Similarly, Maths has 15% weightage for Coordinate Geometry and 3% weightage for Mathematical Reasoning.
In chemistry, organic compound containing oxygen has 6% weight and surface chemistry has 1% weightage.
Over all you have to walk high to low but it does not mean that you should study only high weightage because you have to cover the entire syllabus.
Select the High Study Material:-
Best preparation for the exam does not mean that you have to read a lot of books. The best study method of the exam is that you should choose the right book and the right study material for your exam, in this NCERT books will prepare your base and subject and topic. According to you, you can refer the reference book so that the chances of getting confused do not increase.
Where we tell you the names of the subject wise reference books such as:-
Best books for physics are HC Verma’s Concepts of Physics Volume One and Volume Two, Halliday Resnick and Walker Fundamentals of Physics, DC Pandey Understanding Physics, and etc.
Best books for maths are R.D Sharma, Exemplar, etc.
Best books for chemistry are O.P Aggarwal IIT chemistry, Dr RK Gupta textbook of physical chemistry, etc.
Have a Proper Time Management:-
Managing the time properly for the preparation of the exam. Time plays a very important role, if you have made your proper time table for the preparation of the exam, then it is very good for you and in that time table you have to see that you give particular time to your particular subject. Give equal time to the subject, not that you are studying your favourite subject mostly. Give some time to your weak subjects also. [...]Read more...
August 3, 2023How to prepare for the exam a week before the exam As soon as the exam comes, a sensation spreads among the children, they get scared, now the exam time is going on and the students are very worried about the exam preparation, so I thought why not the preparation of the exam. Share some tips for people whom you follow and then your stress will be less than that.
I have seen this that many times we are not able to score well even after preparing the exam well, whatever the region may be, whether we have made mistake in writing or have not given good content, due to which it is difficult for the teacher to understand. This is why you people do not get good marks, due to which we feel very sad and there is a lack of confidence in our region.
Times give all but the way of studying is different, studying is an art and the art of giving exams there is a lot of difference between the two, studying is good but how well you have attended the paper, the teacher will give a number on it.Table of ContentsBest Method prepare for the exam an weekWays to succeed in the exam an week before the examWe should read all our subjects well, if we do not understand anything while studying, then we should underline it so that we can go to our teacher the next day and understand all the subjects should be studied equally.Key Point should Remember before preparing Exam
Best Method prepare for the exam an week
I am telling in some points, which you follow and guarantee your result in hundred percent that at least 10% of your result will improve, first of all we have to decide for the exam, how many times are exams in a year, we have to give our time. We have to make a table and accordingly we will have to do our studies and also make a time table in which all our subjects are equal to us because all the subjects are equal for us, if we fall short in any subject, our marks will be less and then our percentage will also be there.
We have to make such a way in which all our subjects are equal to us because all the subjects are equal to us, if we fall short in any subject, our marks will be less in it and then our percentage will also be less, that’s why we have to take all the subjects equal.
Ways to succeed in the exam an week before the examWe should take our regular self-test, how we do our self-test, there are two methods for this, the first method is make small notes of whatever you study, the second method is whatever you have studied, the subject related to which you are small. Make small questions and then answer them later and then check them, you can also check those answers yourself or you can get your friend checked or your teacher can get it checked 2 of Self Confident There are advantages, one is that your confidence increases, the other is your mistakes Let’s make corrections on it so that the mistake does not happen again in future.
We should not depend only on the studies before the exam, most of the children start studying a week before the exam but they should not do this, to get good marks in the exam, we should study all the subjects in equal quantity from the beginning. According to me, in the subject in which the work has been done, please come and revise it again at home and I tell you the test, I take the math’s test, if the teacher has made 5 questions, then you should come home and practice it immediately. And whatever the problem may be, from the very beginning, if the child pays attention to studies, then go to the next day and ask his teacher, then he will not have to work hard at the time of examination, what will happen that he will be relaxed at exam time and can give his paper easily without of tension
It is very important to have a calm mind for a good exam Mistakes will also be less and when mistakes are less, then we will be able to write the exam well, it means to say that it is very important to have a calm mind for a good paper.
We need to revise our subject only a few weeks before the exam. Most of the children want to study only at the time of examination but they should not do so because by doing this they put a lot of pressure on the subject. We should only revise our subject, we should read the short note made by us so that we can pass with good marks in the examination.
How to get good marks in your exam what to doWe should read all our subjects well, if we do not understand anything while studying, then we should underline it so that we can go to our teacher the next day and understand all the subjects should be studied equally.Must take weekly or monthly practice test
At the end of every lesson, a test must be given whether it is written or oral.
If any important thing is seen while studying the subject, it should be highlighted or noted down so that they can revise it at the time of examination.Key Point should Remember before preparing Exam
We can also get good marks in the exam with the art of writing, it is not necessary that we write a lot, write as much as is asked, use beautiful writing, give your answer in points like SST is a subject. In that we will give our answer in points then there will be more batter, you can present your answer from picture also writing is an art and with this art also you can get good marks in exam creativity and by writing answer in points you will be good in exam You can get the number creativity and by writing the answer in point you can get good marks in the exam
In order to get good marks in the examination, we have to take special care of speed, even after answering the questions many times in the examination, we miss the paper, due to which our paper is not able to be done in the examination, we have to take special care of writing for this. We have to keep our writing speed fast, the questions that come first, we have to do the questions which come a little less, we should do it later, for this you have to do the revision which you do before the exam, only then you will have the practice of writing.
Routine can also bring good marks in the examination A good routine can make a good impression in our examination, if you want to be successful in life, it is very important to have a routine, if you are a student, then your study time is your time for sports. Time to talk to friends and you have to give time to your family too [...]Read more...
August 3, 2023As a professional educator working for the esteemed education website, “Hsslive” it is my privilege to provide students with the best resources to help them excel academically. Our commitment to excellence is reflected in our comprehensive collection of previous year question papers, which are an indispensable tool for students preparing for their exams.
For Class 10th students, we offer previous year question papers of Kerala education board in subjects such as Mathematics and Science. These question papers provide students with an opportunity to familiarize themselves with the exam pattern and marking scheme, helping them to approach their exams with greater confidence.Table of ContentsPrevious year question papers Class 10th to Class 12thMaximize Your Exam Success with “hsslive’s” User-Friendly Study Tools and Materials
Previous year question papers Class 10th to Class 12thClass 10th Maths Previous year question papers
Class 10th Physics Previous year question papers
Class 10th Standard Chemistry Previous year question papers
Kerala Class 10th Standard Biology Kerala Previous year question papers
Kerala Class 10th Biology Previous year question papers
10th Standard Social Studies Previous year question papers
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10th Standard Other Subjects Previous year question papers in MalayalamSimilarly, for Class 11th students, we offer previous year question papers of Kerala Plus One for all subjects, including Mathematics, Physics, Chemistry, and more. Our question papers are designed to provide students with a clear understanding of the exam format and the types of questions that are likely to be asked. They are an excellent resource for students who want to practice and improve their exam-taking skills.Plus One Maths Previous Question papers
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Plus One Computer Science Question papersFor Class 12th students, we offer Plus Two previous year question papers and model test papers. These papers are designed to help students prepare for their final exams by providing them with a comprehensive overview of the syllabus and an opportunity to practice answering different types of questions. Our model test papers are especially useful, as they are designed to simulate the actual exam environment, helping students to develop a feel for the exam and to identify areas where they need to improve.Plus Two Maths Previous Question papers
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Plus Two English, Hindi, and Malayalam Previous Question papersMaximize Your Exam Success with “hsslive’s” User-Friendly Study Tools and Materials
At “hsslive,” we understand the importance of providing students with the best possible resources to help them succeed. Our previous year question papers are carefully selected and curated by our team of expert teachers, who have years of experience teaching in their respective fields. They understand the nuances and complexities of the syllabus and have used their knowledge to develop question papers that are insightful, engaging, and informative.
In addition to our previous year question papers, we also offer a range of other resources and tools to help students prepare for their exams. These include study materials, video lectures, and more. All of our resources are designed to be user-friendly and accessible, making it easy for students to learn and study at their own pace.
In conclusion, if you are a student preparing for your exams in Class 10th to Class 12th, “hsslive” is your one-stop destination for all your academic needs. Our collection of previous year question papers is an invaluable resource for students who want to practice and improve their exam-taking skills. With the help of our expertly crafted question papers and other resources, you can approach your exams with greater confidence and achieve your academic goals. [...]Read more...