Which one of the following equations is corre | vedclass

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Question

(D) For the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of reaction is expressed as: $Rate = -\frac{d[N_2]}{dt} = -\frac{1}{3}

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$3 \frac{d[NH_3]}{dt} = -2 \frac{d[H_2]}{dt}$

Vedclass · Answer

(D) For the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of reaction is expressed as: $Rate = -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$ Equating the terms for $NH_3$ and $H_2$: $-\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$ Multiplying both sides by $6$: $-2 \frac{d[H_2]}{dt} = 3 \frac{d[NH_3]}{dt}$ Rearranging gives $3 \frac{d[NH_3]}{dt} = -2 \frac{d[H_2]}{dt}$.

Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?

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