Question

Molecular nitrogen can be converted into NO by the following reaction sequence, $N_2+3H_2\to 2N{H}_3$
$4N{H}_3+5O_2\to 4NO+6H_{2}O$
Calculate the mass of NO formed from 100 g of $N_2$ with excess of $H_2$ and $O_2$?

• A. 100 gm
• B. 150.60 gm
• C. 214.28 gm
• D. 256.32 gm

Answer 1

The correct option is C 214.28 gm

$\begin{array}{ccccc}{N}_2& +& 3H_2& \to & 2N{H}_3\\ mole=\frac{100}{28}& & & & \frac{100}{28}\times 2\end{array}$
$4N{H}_3+5O_2\to 4NO+6H_{2}O$
4 moles $N{H}_3$ gives 4 moles of NO
$\frac{200}{28}$ moles $N{H}_3$ gives 4 moles of $\frac{200}{28}$ moles of NO
Moles of NO formed from 100 g $N_2=\frac{200}{28}$
mass of NO formed $=\frac{200}{28}\times 30$ gm = 214.28 gm