Question

$N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right)$

For the given reaction, under certain condition of temperature and partial pressure of the reactants, the rate of formation of $N{H}_3$ is ${10}^{-3}kgh{r}^{-1}$. The rate of conversion of $H_2$ under the same condition is:

• A. $1.5\times {10}^{-3}kgh{r}^{-1}$
• B. $1.76\times {10}^{-4}kgh{r}^{-1}$
• C. $2\times {10}^{-3}kgh{r}^{-1}$
• D. $3\times {10}^{-3}kgh{r}^{-1}$

Answer 1

The correct option is B $1.76\times {10}^{-4}kgh{r}^{-1}$

$N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right)$

$-\frac{1}{3}\frac{d}{dt}\left[H_2\right]=\frac{1}{2}\frac{d}{dt}\left[N{H}_3\right]$

$-\frac{d}{dt}\left[H_2\right]=\frac{3}{2}\frac{d}{dt}\left[N{H}_3\right]$

The rate of formation of ammonia is ${10}^{-3}$ kg/hr. The rate of conversion of hydrogen under same condition is

$-\frac{d}{dt}\left[H_2\right]=\frac{3\times 2}{2\times 17}\times {10}^{-3}$ kg/hr $=1.76\times {10}^{-4}kgh{r}^{-1}$

Hence, the correct option is $A$