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.

What is Law of Multiple Proportion?

Law of Multiple Proportions provides a relationship between the masses of elements when they combine to form two or more compounds. This Law was given by John Dalton in the early 19th century as part of his atomic theory.

According to Law of Multiple Proportions, if 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 the ratio of small whole numbers.

In simple term, if two elements A and B form multiple compounds, then the ratio of the masses of B that combine with a fixed mass of A will be in a ratio of small whole numbers.

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.

Significance of Law of Multiple Proportion

Importance of Law of Multiple Proportion are:

• This law supports the atomic theory proposed by John Dalton.

• This law helps to predict the composition of compounds based on the masses of the constituent elements.

• The law allows scientists to predict the existence of additional compounds between two elements.

• The law helped in determining relative atomic masses of elements in the early days of chemistry.

Limitations of Law of Multiple Proportion

The Limitations of Law of Multiple Proportion are:

• The law is primarily applicable to simple compounds only. It can not describe the composition of more complex compounds containing three or more elements.

• The law states that elements combine in simple whole-number ratios, but it does not account for the existence of isotopes.

• This law is not applicable to non-stoichiometric compounds.

• The law of multiple proportions does not provide insights into the spatial arrangement or molecular structure of those compounds.

Read More,

• Laws of Chemical Combination
• Law of Conservation of Mass
• Law of Definite Proportions

FAQs on Law of Multiple Proportion

Who wrote the law of multiple proportions?

The law was formulated by the English chemist John Dalton in 1803.

What is the law of constant proportion?

Law of constant proportion states that the elements in a chemical compound are always combined in fixed, definite proportions by mass.

What is the law of multiple proportions of water and hydrogen peroxide?

The Law of Multiple Proportions applied to water (H₂O) and hydrogen peroxide (H₂O₂) states that the masses of oxygen that combine with a fixed mass of hydrogen to form these compounds are in simple whole number ratios i.e. 1:2.

What is the law of multiple proportions?

The Law of Multiple Proportions states that when two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers.