Nitric oxide reacts with H_2 according to the | vedclass

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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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$-\frac{d[NO]}{dt} = \frac{d[H_2O]}{dt}$

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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 $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2O_{(g)}$,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 $NO$ and $H_2O$: $-\frac{1}{2} \frac{d[NO]}{dt} = \frac{1}{2} \frac{d[H_2O]}{dt}$. Multiplying both sides by $2$,we get: $-\frac{d[NO]}{dt} = \frac{d[H_2O]}{dt}$.

Nitric oxide reacts with $H_2$ according to the reaction,$2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_2O_{(g)}$. Identify the correct relationship among the following.

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