What are some examples of Gay Lussac’s Law?

Gay-Lussac's Law, also known as the Law of Combining Volumes, describes the relationship between the volumes of gases involved in a chemical reaction when the gases are at constant temperature and pressure. It states that the ratio of the volumes of the reactant gases and the ratio of the volumes of the products, when measured at the same conditions of temperature and pressure, can be expressed as small whole numbers.

Here are a few examples of Gay-Lussac's Law:

Hydrogen and Oxygen Combustion:

When hydrogen (H2) and oxygen (O2) react to form water (H2O), they do so in a 2:1 volume ratio. This means that 2 volumes of hydrogen gas combine with 1 volume of oxygen gas to produce 2 volumes of water vapor, all at the same temperature and pressure.
Ammonia Synthesis:

In the synthesis of ammonia (NH3) from nitrogen gas (N2) and hydrogen gas (H2), the volumes also follow a simple ratio. 1 volume of nitrogen gas combines with 3 volumes of hydrogen gas to produce 2 volumes of ammonia gas.
Chlorine and Hydrogen Reaction:

The reaction between chlorine gas (Cl2) and hydrogen gas (H2) to form hydrogen chloride gas (HCl) follows a 1:1 volume ratio. 1 volume of chlorine gas combines with 1 volume of hydrogen gas to produce 2 volumes of hydrogen chloride gas.
Carbon Monoxide and Oxygen Combustion:

When carbon monoxide (CO) burns in oxygen (O2) to produce carbon dioxide (CO2), it does so in a 2:1 volume ratio. 2 volumes of carbon monoxide combine with 1 volume of oxygen gas to produce 2 volumes of carbon dioxide gas.
These examples illustrate how the Law of Combining Volumes, as formulated by Gay-Lussac, helps to describe the stoichiometry of chemical reactions involving gases when measured under constant temperature and pressure conditions. It provides insight into the simple whole-number ratios in which gases combine to form new compounds.