Question

For the reaction, $N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right)$, under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $N{H}_3$ is 0.001 kg $h^{-1}$. The rate of conversion of hydrogen under the same condition is in $kg{h}^{-1}$ is:

• A. $1.165$ x ${10}^{-4}kgh{r}^{-1}$
• B. $1.295$ x ${10}^{-4}kgh{r}^{-1}$
• C. $1.765$ x ${10}^{-4}kgh{r}^{-1}$
• D. $Noneofthese$

Answer 1

Answer: (C)

$1.765$ x ${10}^{-4}kgh{r}^{-1}$

$3H_2\equiv 2N{H}_3^{\cdot }$

$\frac{d\left[H_2\right]}{dt}=\frac{3}{2}\frac{d\left[N{H}_3\right]}{dt}\times \frac{Totalwtof{H}_{2}inkg}{TotalwtofN{H}_{3}inkg}$

= 0.001 kg $h{r}^{-1}\times \frac{3\times 2\times {10}^{-3}}{2\times 17\times {10}^{-3}}$

= $1.765$ x ${10}^{-4}kgh{r}^{-1}$