Question

Explain the law of chemical combination with example​

Answer 1

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Here is the answer to your question:

There are three important laws of chemical combination. These are:

1. Law of conservation of mass (or matter),

2. Law of constant proportions, and

3. Law of multiple proportions.

The laws of chemical combination are the experimental laws which have been formulated by scientists after performing a large number of experiments involving various types of chemical reactions. These experimental laws ultimately led to the idea of 'atoms' being the 'smallest unit' of matter. In fact, the laws of chemical combination played a significant role in the development of Dalton's atomic theory of matter.

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Answer 2

Explanation:

The laws of chemical combination describe the basic principles obeyed by interacting atoms and molecules, interactions that can include many different combinations that happen in many different ways. This amazing diversity of interactions allows for an astounding variety of chemical reactions and compounds. Spontaneous chemical reactions happen constantly, shaping the world around us, while humans engineer specific reactions to our benefit and attempt to curb reactions that hurt us. Though chemical reactions can be as complex as they are numerous, they are all fundamentally governed by these same guiding laws of chemical combination, which lay the groundwork for analysis of chemical reactions. They give a mathematical formulation and allow predictability given initial conditions.

They are the launch pad from which we jump off to creating all sorts of wild compounds and phenomena. And while chemistry is still difficult and intricate, with the laws of chemical combination on our side, we can begin to make some headway.

law of multiple proportions:

According to this law, if 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 the ratio of small whole numbers.

Example

Hydrogen + Oxygen → Water

2g 16g 18g

Hydrogen + Oxygen → Hydrogen Peroxide

2g 32g 34g

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

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