If $R = k[NO]^2[O_2]$,the rate constant can be increased by:

The slope of the Arrhenius plot $(\ln k \, vs \, \frac{1}{T})$ of a first-order reaction is $-5 \times 10^{3} \, K$. The value of $E_{a}$ of the reaction is: (in $kJ \, mol^{-1}$)
$[\text{Given } R = 8.314 \, J \, K^{-1} \, mol^{-1}]$

Which of the following graphs of $\log \, K \rightarrow 1/T$ can be used to calculate the activation energy?

$A$ catalyst increases the rate of a chemical reaction by

Which of the following options is incorrect?

Which of the following statements is correct regarding the Arrhenius equation and reaction kinetics?