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(B) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d

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$\frac{d[N_2]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt}$

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(B) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$ For the given reaction $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$,the rate expression is: Rate $= -\frac{1}{2} \frac{d[NO]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2O]}{dt}$ Comparing the terms for $N_2$ and $H_2O$: $\frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2O]}{dt}$ This implies $\frac{d[H_2O]}{dt} = 2 \frac{d[N_2]}{dt}$. Comparing the terms for $N_2$ and $H_2$: $\frac{d[N_2]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt}$. Thus,option $B$ is the correct relationship.

Nitric oxide reacts with $H_2$ according to the reaction:
$2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$
Identify the correct relationship for the rate of consumption of reactants and the rate of formation of products.

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Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$Identify the correct relationship for the rate of consumption of reactants and the rate of formation of products.