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 given by the expression: Rate $= -\frac{d[N_2]}{dt} = -

Vedclass · Accepted Answer

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

Vedclass · Answer

(D) For the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$,the rate of reaction is given by the expression: 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 $6$,we get: $-2 \frac{d[H_2]}{dt} = 3 \frac{d[NH_3]}{dt}$. 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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