The rate law of the reaction $A + 2B \to \text{Product}$ is given by $\frac{d[B]}{dt} = k[B^2]$. If $A$ is taken in excess,the order of the reaction will be

For the reaction,$2N_2O_5 \to 4NO_2 + O_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol \ L^{-1}$ will be:

The alkaline hydrolysis of an ester is a .......

For the reaction:
$2NO_{2(g)} + O_{3(g)} \to N_2O_{5(g)} + O_{2(g)}$
The rate law is $R = K[NO_2]^1 [O_3]^1$.
Which of these possible reaction mechanisms is consistent with the rate law?
Mechanism $I$:
$NO_{2(g)} + O_{3(g)} \to NO_{3(g)} + O_{2(g)}$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_{5(g)}$ (fast)
Mechanism $II$:
$O_{3(g)} \rightleftharpoons O_{2(g)} + [O]$ (fast)
$NO_{2(g)} + [O] \to NO_3$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_5$ (fast)

The acidic hydrolysis of an ester is a .......

The reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?