Grade 11
  1. Basic concepts of chemistry  1.1. Importance of Chemistry  1.2. Nature and scope of chemistry  1.3. laws of chemical combination  1.3.1. Law of conservation of mass  1.3.2. Law of definite proportions  1.3.3. Law of multiple proportions  1.3.4. Law of gaseous volume  1.3.5. Avogadro's Law  1.4. Dalton's atomic theory  1.5. Mole concept and molar mass  1.6. Percent composition  1.7. Empirical and molecular formula  1.8. Stoichiometry and Stoichiometric Calculations  1.9. Limiting reagent concept
  2. Structure of the atom  2.1. Discovery of the electron, proton, and neutron  2.2. Atomic Model  2.2.1. Thomson's model  2.2.2. Rutherford's model  2.2.3. Bohr's model  2.3. Quantum mechanical model of the atom  2.4. Dual nature of matter and radiation  2.5. Heisenberg's uncertainty principle  2.6. Quantum numbers  2.7. Atomic orbitals and their shapes  2.8. Electronic configuration of elements  2.9. Aufbau principle  2.10. Pauli's exclusion principle  2.11. Hund's maximum multiplicity rule  2.12. de Broglie's hypothesis  2.13. Photoelectric effect
  3. Classification of elements and periodicity in properties  3.1. Historical development of the periodic table  3.2. Modern Periodic Law and Periodic Table  3.3. Periodic trends in properties  3.3.1. Atomic and Ionic Radius  3.3.2. Ionization enthalpy  3.3.3. Electron gain enthalpy  3.3.4. Electronegativity  3.3.5. Valency  3.3.6. Metallic and Non-Metallic Properties  3.3.7. Oxidation states  3.4. Unusual Properties of the First Elements
  4. Chemical Bonding and Molecular Structure  4.1. Kossel–Lewis approach to chemical bonding  4.2. Ionic or electrovalent bond  4.3. Covalent bond and its features  4.4. Bond parameters  4.5. VSEPR Theory  4.6. Valence bond theory  4.7. Hybridization and its types  4.8. Molecular orbital theory  4.8.1. Bond order and stability  4.9. Hydrogen bonding
  5. States of matter  5.1. Intermolecular forces  5.2. Gas Laws  5.2.1. Boyle's law  5.2.2. Charles's Law  5.2.3. Avogadro's Law  5.2.4. Dalton's law of partial pressure  5.2.5. Graham's law of spread  5.3. Ideal Gas Equation and Applications  5.4. Real gases and deviations from ideal behaviour  5.5. Kinetic molecular theory of gases  5.6. Liquefaction of gases  5.7. Properties of Liquids  5.8. Surface tension and viscosity
  6. Thermodynamics  6.1. System and environment  6.2. Types of systems in thermodynamics  6.3. Types of procedures  6.4. First law of thermodynamics  6.5. Internal energy and enthalpy  6.6. Heat capacity and specific heat  6.7. Hess's law of constant heat summation  6.8. Bond dissociation enthalpy  6.9. Enthalpy of formation and combustion  6.10. Enthalpy of solution and neutralization  6.11. Spontaneity and the second law of thermodynamics  6.12. Gibbs free energy and its applications
  7. Balance  7.1. The concept of balance  7.2. Equilibrium constant and its applications  7.3. Le Chatelier's principle  7.4. Ionic equilibrium in solutions  7.5. Acid and Base Theory  7.5.1. Arrhenius concept  7.5.2. Bronsted-Lowry concept  7.5.3. Lewis concept  7.6. pH Scale and pOH  7.7. Common ion effect  7.8. Hydrolysis of salts  7.9. Buffer solutions and their mechanism of action  7.10. Solubility equilibrium of sparingly soluble salts
  8. Redox reactions  8.1. Oxidation and reduction concepts  8.2. Oxidation number and its applications  8.3. Redox reactions in terms of electron transfer  8.4. Balancing redox reactions (oxidation number and ion-electron methods)  8.5. Types of redox reactions  8.6. Electrochemical Cells and Redox Reactions
  9. Hydrogen  9.1. Position of Hydrogen in the Periodic Table  9.2. Isotopes of hydrogen  9.3. Preparation of Hydrogen  9.4. Properties of Hydrogen  9.5. Hydrides and their classification  9.6. Water and heavy water  9.7. Hydrogen peroxide and its properties  9.8. Uses of Hydrogen and Its Compounds
  10. S-block elements (alkali and alkaline earth metals)  10.1. Group 1 Elements - Properties and Trends  10.2. Group 2 Elements - Properties and Trends  10.3. Unusual properties of lithium and beryllium  10.4. Important compounds of sodium and their uses  10.5. Important Compounds of Magnesium and Calcium
  11. Some p-block elements  11.1. General Introduction to p-Block Elements  11.2. Group 13 Elements  11.2.1. Boron and its compounds  11.3. Group 14 Elements  11.3.1. Carbon and its allotropes  11.3.2. Important Compounds of Carbon and Silicon
  12. Organic Chemistry - Some Basic Principles and Techniques  12.1. Classification and Nomenclature of Organic Compounds  12.2. Structural representation of organic compounds  12.3. Classification of organic reactions  12.4. Electronic Effects in Organic Chemistry  12.4.1. Inductive effect  12.4.2. Resonance effect  12.4.3. Hyperconjugation  12.5. Reaction mechanism and intermediate species  12.6. Purification and qualitative analysis of organic compounds
  13. Hydrocarbons  13.1. Hydrocarbons  13.1.1. Preparation and Properties of Alkenes  13.2. alkene  13.2.1. Preparation and Properties of Alkenes  13.2.2. Electrophilic addition reactions  13.3. Alkynes  13.3.1. Preparation and Properties of Alkynes  13.4. Aromatic hydrocarbons  13.4.1. Structure and properties of benzene  13.4.2. Electrophilic substitution reactions of benzene
  14. Environmental Chemistry  14.1. Environmental Pollution  14.2. Atmospheric pollution and the greenhouse effect  14.3. Water pollution and treatment methods  14.4. Soil pollution and its effects  14.5. Industrial waste and its treatment  14.6. Strategies for pollution control

Grade 11 → Basic concepts of chemistry → laws of chemical combination ↓


Law of gaseous volume


The law of gaseous volumes, also known as Gay-Lussac's law of combining volumes, is a principle in chemistry that describes how gases react together in simple volume ratios. The law was proposed by Joseph Louis Gay-Lussac in 1808. It is one of the fundamental laws of chemical combinations and plays an important role in understanding the behavior and reactions of gases.

Understanding the law

The essence of the law of gaseous volumes may be summarized as follows: When gases react together at constant temperature and pressure, the volumes of the reacting gases and the volumes of the products (if gaseous) are in simple whole number ratio.

To understand this in more detail, consider the following points:

  • This law applies only to gases and not to solids or liquids.
  • This law is true under constant temperature and pressure conditions.
  • Volume ratios are always simple whole numbers, representing a proportional relationship in the gaseous state.

Visual example

Let's illustrate this concept with a simple reaction between hydrogen and oxygen to form water vapor:

2H 2 (g) + O 2 (g) → 2H 2 O(g)

In this response:

  • Two volumes of hydrogen gas react with one volume of oxygen gas.
  • As a result, two quantities of water vapor are obtained.
2H 2 (g) O 2 (g) 2H 2 O(g)

From this illustration you can see that the volumes of gases involved in the reaction are in the ratio of 2:1:2, which is a simple whole number ratio.

Other examples

Let us consider more chemical reactions to understand the application of the law of gaseous volumes:

Example 1: Reaction of hydrogen and chlorine

H 2 (g) + Cl 2 (g) → 2HCl(g)

In this response:

  • One quantity of hydrogen reacts with one quantity of chlorine.
  • This produces two quantities of hydrogen chloride gas.
H 2 (g) CL 2 (g) 2HCl(g)

Again, the volumes of the gases are in a simple ratio of 1:1:2.

Example 2: Reaction of nitrogen and hydrogen

N 2 (g) + 3H 2 (g) → 2NH 3 (g)

In this response:

  • One quantity of nitrogen reacts with three quantities of hydrogen.
  • This produces two quantities of ammonia.
N2 (g) 3H 2 (g) 2NH3 (g)

Here the simple ratio is 1:3:2.

Real-world implications

The laws of gaseous volumes have important implications in both theoretical and applied chemistry. Understanding these volume relationships is important for tasks such as gas stoichiometry, designing chemical processes involving gases, and performing accurate and efficient chemical synthesis.

In addition, it helps chemists estimate the amount of gaseous products formed during reactions, which is essential in industries such as pharmaceuticals, petroleum refining, and food processing where gas reactions are prevalent.

Mathematical representation

This law can be expressed mathematically. If a reaction involving gaseous reactants and products can be represented as follows:

aA(g) + bB(g) → cC(g) + dD(g)

Then, the volume relation according to the law will be:

V A : V B : V C : V D = a : b : c : d

where V A, V B, V C and V D represent the volumes of gases A, B, C and D respectively.

Considerations and limitations

Although the law of gaseous volumes is a powerful tool in chemistry, it has some caveats and limitations to keep in mind:

  • This law applies only to gases, not to liquids or solids.
  • It is important that the reactions occur at constant temperature and pressure, usually at standard conditions (0°C and 1 atm).
  • This law assumes ideal gas behaviour, which means that it may not accurately describe volume under conditions of high pressure or low temperature, where gases deviate from ideal behaviour.

Conclusion

The law of gaseous volumes is essential to understanding reactions involving gases. By exploring visual examples and mathematical representations, it reveals the simplicity and predictability of gaseous reactions. Mastering this law provides insight not only into theoretical chemistry but also into practical applications in various industries.


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Law of multiple proportions
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Law of gaseous volume

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