Question

For the Haber process,N2+3H2 yields 2NH3, what volume of Nitrogen is consumed at STP if you collect 44.8 L of ammonia in excess hydrogen (N=14 AMU, H=1 AMU)
a. 14.9 L
b. 29.9 L
c. 44.8L
d. 22.4 L

Answer 1

Answer: d. 22.4 L

Explanation:

$N_2+3H_2\rightarrow 2NH_3$

According to Avogadro's law , 1 mole of every gas occupies 22.4 L of volume at STP.

moles of ammonia=$\frac{\text {given volume}}{\text {Standard Volume}}=\frac{44.8}{22.4}=2moles$

Given: Hydrogen is the excess reagent and nitrogen is the limiting reagent as it limits the formation of product.

From the given balanced equation:

2 moles of ammonia is produced by 1 mole of nitrogen.

Thus 2 moles of ammonia is produced by 22.4 L of nitrogen at STP as 1 mole of nitrogen occupies 22.4 L at STP.