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
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.
Table of Content
- What is Law of Multiple Proportion?
- Examples of Law of Multiple Proportion
- Significance of Law of Multiple Proportion
- Limitations of Law of Multiple Proportion