Identify the correct expression for the rate | vedclass

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

Vedclass · Accepted Answer

$-\frac{1}{2} \frac{d[N_2 O_5]}{dt}$

Vedclass · Answer

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: $r = -\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$ For the reaction $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$,the rate expression is: $r = -\frac{1}{2} \frac{d[N_2 O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$ Comparing this with the given options,option $A$ is the correct expression for the rate of reaction.

Identify the correct expression for the rate of the following reaction: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$

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