# What volume at STP would be required to react with 0.100 mol of hydrogen to produce ammonia?

## Question:

What volume at STP would be required to react with 0.100 mol of hydrogen to produce ammonia?

## Stoichiometry:

Stoichiometry in chemistry gives a quantitative relationship between the reactants and the products in a chemical reaction. In a well balanced chemical reaction, the coefficients represent the mole ratio. Thus, given the moles of one of the reactants or the products, we can determine the moles of the other reactants or the products using the mole ratio.

The reaction between nitrogen gas and hydrogen gas to produce ammonia is represented by the reaction equation:

• {eq}\rm H_2(g) + N_2(g)\rightarrow NH_3(g) {/eq}

Balancing the reaction equation, we have:

• {eq}\rm 3H_2(g) + N_2(g)\rightarrow 2NH_3(g) {/eq}

From the balanced reaction equation, 3 moles of hydrogen gas react with 1 mole of nitrogen gas to produce 2 moles of ammonia gas. Thus, the mole ratio between hydrogen gas and nitrogen gas is {eq}3:1 {/eq}. Given that the moles of hydrogen gas in the reaction is {eq}\rm 0.100mols {/eq}, the moles of nitrogen gas required in the reaction is:

• {eq}\rm \dfrac{1}{3}\times 0.100mols = 0.0333mols {/eq}.

At standard temperature and pressure (STP), one mole of a gas occupies 22.4L. Therefore, 0.0333mols of nitrogen gas will occupy:

• {eq}V = 0.0333\times 22.4 = 0.747L {/eq}

Therefore, at STP, {eq}\boxed{0.747\, \rm liters} {/eq} of nitrogen gas will be required to react with 0.100 moles of hydrogen to produce ammonia.