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(A) The rate of reaction is defined as the rate of disappearance of reactant divided by its stoichiometric coefficient.For reaction $(a)$: $2N_2O_5 \r

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$k = 2k'$

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(A) The rate of reaction is defined as the rate of disappearance of reactant divided by its stoichiometric coefficient.For reaction $(a)$: $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$Rate $= -\frac{1}{2} \frac{d[N_2O_5]}{dt} = k_{rate}[N_2O_5]$Given $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$,so Rate $= \frac{k}{2} [N_2O_5]$.For reaction $(b)$: $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$Rate $= -\frac{d[N_2O_5]}{dt} = k'_{rate}[N_2O_5]$Given $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$,so Rate $= k' [N_2O_5]$.Since the rate of the reaction is the same regardless of how the stoichiometry is written,we equate the rates:$\frac{k}{2} [N_2O_5] = k' [N_2O_5]$$k = 2k'$

Initial $[A_2]$	Initial $[B_2]$	$R.O.R. (r) \ M s^{-1}$
$0.2$	$0.2$	$0.04$
$0.1$	$0.4$	$0.04$
$0.2$	$0.4$	$0.08$

For the first order decomposition reaction of $N_2O_5$,it is found that -
$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$
Which of the following is true?

Similar Questions

Which of the following is an example of a second-order reaction?

$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$

Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$

$0.2$ $0.2$ $0.04$

$0.1$ $0.4$ $0.04$

$0.2$ $0.4$ $0.08$

Order of reaction with respect to $A_2$ and $B_2$ are respectively:

For the reaction $XA + YB \rightarrow mp + nq$,the rate is given by $\text{Rate} = K[A]^c[B]^d$. What is the overall order of the reaction?

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.

For a reaction between $A$ and $B$,the order with respect to $A$ is $2$ and the order with respect to $B$ is $3$. If the concentrations of both $A$ and $B$ are doubled,the rate will increase by a factor of:

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For the first order decomposition reaction of $N_2O_5$,it is found that -$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$Which of the following is true?