For a chemical reaction,if the temperature is increased from $25\,^{\circ}C$ to $55\,^{\circ}C$,the rate of reaction will change by a factor of (Assume $\mu = 3$).

At room temperature,the reaction between $NO$ and $O_2$ to form $NO_2$ is fast,whereas the reaction between $CO$ and $O_2$ is slow because:

For a first order reaction,the rate of reaction is $2.4 \times 10^{-3} \ mol \ L^{-1} \ s^{-1}$ at $27 \ ^\circ C$. The activation energy of the reaction is $24.942 \ kJ \ mol^{-1}$. The rate of reaction at $327 \ ^\circ C$ is ....... $mol \ L^{-1} \ s^{-1}$ [Take $e^5 = 150$,$e^{0.005} = 1$,$e^4 = 55$].

For the process $R \rightarrow P$, the energy of the reactant is $50 \ kJ$ and the energy of the transition state is $170 \ kJ$. Determine the activation energy $(E_a)$ for the forward reaction in $kJ$.

The first order rate constant for the decomposition of ethyl iodide by the reaction $C_{2}H_{5}I_{(g)} \rightarrow C_{2}H_{4(g)} + HI_{(g)}$ at $600 \ K$ is $1.60 \times 10^{-5} \ s^{-1}$. Its energy of activation is $209 \ kJ/mol$. Calculate the rate constant of the reaction at $700 \ K$.

In collision theory of chemical reaction,$Z_{AB}$ represents