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 rate constant is the same for $3$ reactions of order $I, II$,and $III$,respectively,with the unit of concentration being in moles per litre. If the concentration of the reactant is unity,the rates of reaction $R_1, R_2, R_3$ will be:

The rate of reaction,$A + B + C \longrightarrow P$ is given by
$r = K[A]^{1/2} [B]^{1/2} [C]^{1/4}$
The order of reaction is

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?

For the reaction system $2NO_{(g)} + O_{2(g)} \to 2NO_{2(g)}$,the volume is suddenly reduced to half its initial value by increasing the pressure. If the reaction is of first order with respect to $O_2$ and second order with respect to $NO$,the rate of reaction will:

When the temperature increases from $300 \, K$ to $310 \, K$,the rate of reaction increases by $2.3$ times. If the rate constant at $300 \, K$ is $x$,then the rate constant at $310 \, K$ will be equal to .......