Question

Given 1 mole of ${{N}_{2}}$ reacts with $Ca$ to form $C{{a}_{3}}{{N}_{2}}$. How many moles of $C{{a}_{3}}{{N}_{2}}$ are produced?

Answer 1

Hint: Write the balanced chemical equation where calcium and nitrogen reacts to form calcium nitride. By taking care of stoichiometry of the reaction, conclude the number of moles of calcium nitride produced.

Complete step by step solution:
The chapters of chemistry which tell us about some of the basic reactions of the chemical compounds and also the concept of balancing a chemical equation are familiar to us.
We shall see these concepts in detail so that we will be able to conclude the correct answer.
- Balancing of a chemical equation means that the number of moles of each reactant should be equal to that of the number of moles of product.
- The equation is written as, the reactants on left hand side and the product on the right hand side which is separated by the arrow pointing from the reactant to the product side.
- Now in the above reaction where 1 moles of nitrogen reacting with calcium and the product formed as the calcium nitride will be as shown below,
${{N}_{2}}+Ca\to C{{a}_{3}}{{N}_{2}}$
Now, this equation is not balanced. To balance this, let us make the number of moles of calcium as 3 so that the equation is balanced. Thus, the reaction can be written as,
\[{{N}_{2}}(g)+3Ca(s)\to C{{a}_{3}}{{N}_{2}}(s)\]
Since the reaction is now balanced, we can conclude that 1 mole of ${{N}_{2}}$ reacts with 3 moles of calcium to give one mole calcium nitride.
Thus, we can say that 1 mole of nitrogen produces 1 mole of calcium nitride.

Note:
Note that balancing of a chemical equation may not necessarily be a whole number but can also have the fraction values and this does not change the total equilibrium or the stoichiometry of the reaction.