You will learn about "Balancing Chemical Equations" in this video. The law of conservation of mass states that mass can neither be created nor destroyed in a chemical reaction. This means that the number of atoms in each element should remain the same before and after a reaction.
Let us understand this with the help of an example. Hydrogen combines with nitrogen to give ammonia. Here, 2 is the subscript, which tells us the number of hydrogen and nitrogen atoms. Now, we need to balance the number of atoms on both the sides. There are 2 hydrogen atoms in the reactant and 3 in the product. Also, there are 2 nitrogen atoms in the reactant and only 1 in the product. We need to multiply hydrogen atoms by 3 and ammonia by 2. Now, there are 3 * 2, i.e. 6 hydrogen atoms in the reactant and 2 * 3, i.e. 6 hydrogen atoms in the product. Similarly, there are 2 nitrogen atoms in the reactant and 2 * 1, i.e. 2 nitrogen atoms in the product. Hence, this chemical equation is now perfectly balanced.
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