What volume of ammonia gas, NH3, in liters is produced at stp by the complete reaction of 100 g of nitrogen N2, with excess hydrogen? N2 + 3H2 ---> 2NH3

Oct 9, 2016

Molar mass of ${N}_{2} \to 28 \text{ g/mol}$

So 100 g ${N}_{2} = \frac{100 g}{28 \frac{g}{\text{mol}}} = \frac{100}{28} m o l = \frac{25}{7} m o l$

The equation of the reaction is

${N}_{2} + 3 {H}_{2} \to 2 N {H}_{3}$

The stochiometry of this equation reveals that 1 mol ${N}_{2}$ produces 2 moles $N {H}_{3}$having volume $2 \times 22.4 L$ at STP ( when reacted with excess ${H}_{2}$)

So 100g or.$\frac{25}{7} \text{ mol } {N}_{2}$ produces $\frac{25}{7} m o l \times 2 \times 22.4 \frac{L}{\text{mol}} N {H}_{3}$
$= 160 \text{ L } N {H}_{3}$