Question

N2 + 3H2 → 2NH3 How many grams of hydrogen are necessary to react completely with 853.42g of nitrogen in the above reaction?

Answer 1

Answer: 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.

Explanation:

The balanced chemical reaction is :

$N_2+3H_2\rightarrow 2NH_3$

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$  

$\text{Number of moles of nitrogen}=\frac{853.42g}{28g/mol}=30.479moles$

According to stoichiometry:

1 mole of $N_2$ react with = 3 moles of $H_2$

30.479 moles of $N_2$ will react with=$\frac{3}{1}\times 30.479=91.437moles$ of $H_2$

 Mass of $H_2$ =$moles\times {\text {Molar mass}}=91.437mol\times 2g/mol=182.87g$

Thus 182.87 grams of hydrogen are necessary to react completely with 853.42g of nitrogen.