Examples of Law of Multiple Proportion

Examples of the Law of Multiple Proportion are:

Carbon and Oxygen

When Carbon combines with oxygen it forms two compounds, namely carbon monoxide (CO) and carbon dioxide (CO₂). In the formation of carbon dioxide and carbon monoxide, the ratio of carbon that combine with a fix mass of oxygen are in a ratio 1 : 2. The general equation for the same is given below:

Carbon + Oxygen → carbon dioxide

12g 16g 18g

Carbon + Oxygen → carbon monoxide

24g 16g 40g

Here, the masses of carbon (i.e., 12 g and 24 g), which combine with a fixed mass of oxygen (16g) are in a simple ratio, i.e., 12:24 or 1:2.

Hydrogen and Oxygen

When hydrogen combines with oxygen it forms two compounds, namely water (H₂O) and Hydrogen peroxide(H₂O₂). In the formation of these compounds, the ratio of oxygen that combine with a fix mass of hydrogen are in a ratio 1 : 2. The general equation for the same is given below:

Hydrogen + Oxygen → Water

2g 16g 18g

Hydrogen + Oxygen → Hydrogen peroxide

2g 32g 34g

Here, the ratio of masses of oxygen (i.e., 16 g and 32 g) that combine with a fixed mass of hydrogen (2g) are in a simple ratio, i.e., 16:32 or 1:2.

Law of Multiple Proportions is a fundamental principle in chemistry that describes the relationship between the masses of elements that combine to form different compounds. This law was proposed by John Dalton in 1803.

This article will give you a detailed description of Law of Multiple Proportion, its example, limitations, and importance.