For the reaction N_{2(g)} + 3H_{2(g)} to 2NH_ | vedclass

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(B) The rate of reaction is given by the expression: $	ext{Rate} = -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{d

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$0.0015 \ kg \ h^{-1}$

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(B) The rate of reaction is given by the expression: $	ext{Rate} = -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Given that the rate of formation of $NH_3$ is $\frac{d[NH_3]}{dt} = 0.001 \ kg \ h^{-1}$.From the stoichiometric relationship: $-\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$.Therefore,the rate of disappearance (conversion) of $H_2$ is: $-\frac{d[H_2]}{dt} = \frac{3}{2} 	imes \frac{d[NH_3]}{dt} = 1.5 	imes 0.001 \ kg \ h^{-1} = 0.0015 \ kg \ h^{-1}$.

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ h^{-1}$. The rate of conversion of $H_2$ under the same conditions is:

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