Consider the plots for the types of reaction | vedclass

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(A) For plot $(i)$,the rate $-\frac{d[A]}{dt}$ is directly proportional to $[A]$. This represents a $1^{st}$ order reaction,where $rate = k[A]$.For pl

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$1, 0, 2$

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(A) For plot $(i)$,the rate $-\frac{d[A]}{dt}$ is directly proportional to $[A]$. This represents a $1^{st}$ order reaction,where $rate = k[A]$.For plot $(ii)$,the concentration $[A]$ decreases linearly with time $t$. This represents a zero order reaction,where $[A]_t = -kt + [A]_0$.For plot $(iii)$,the graph of $\frac{1}{[A]}$ versus $t$ is a straight line with a positive slope. This represents a $2^{nd}$ order reaction,where $\frac{1}{[A]_t} = kt + \frac{1}{[A]_0}$.Thus,the reaction orders are $1, 0, 2$ respectively.

Consider the plots for the types of reaction $nA \to B + C$. These plots respectively correspond to the reaction orders:

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For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate equation can be expressed in two ways $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$ and $+\frac{d[NO_2]}{dt} = k'[N_2O_5]$. $k$ and $k'$ are related as:

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