Question

For the reaction $N_{2}(g) + 3H_{2}(g) \rightarrow 2NH_{3}(g)$ under certain conditions of temperature and partial pressure of the reactants, the rate of formation of $NH_{3}$ is $0.001kgh^{- 1}$. The rate of conversion of $H_{2}$ under the same conditions is.

• A. $1.82 \times 10^{- 4}kg/hr$
• B. $0.0015kg/hr$
• C. $1.52 \times 10^{4}kg/hr$
• D. $1.82 \times 10^{- 14}kg/hr$

Answer 1

Answer: (B)

$0.0015kg/hr$

Answer 2

$\frac{- dN_{2}}{dt} = \frac{- 1}{3}\frac{dH_{2}}{dt} = \frac{1}{2}\frac{dNH_{3}}{dt}$

$\frac{dH_{2}}{dt} = \frac{3}{2} \times 0.001 = 0.0015kghr^{- 1}.$