The Arrhenius equation can be represented as:

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

The energy of activation is

$A_{(g)} + B_{(g)} \rightleftharpoons C_{(g)} + D_{(g)}$
The curves $M$ and $N$ represent the variation of energy with reaction coordinate for the reaction in absence and presence of catalyst.
Which value represents the activation energy $(E_a)$ for the backward reaction in the presence of catalyst?

In a multistep reaction such as $A + B$ $\longrightarrow Q$ $\longrightarrow C$,the potential energy diagram is shown below. What is $E_{a}$ for the reaction $Q \longrightarrow C$?

For the reaction of $H_2$ with $I_2$,the rate constant is $2.5 \times 10^{-4} \ dm^3 \ mol^{-1} \ s^{-1}$ at $327 \ ^oC$ and $1.0 \ dm^3 \ mol^{-1} \ s^{-1}$ at $527 \ ^oC$. The activation energy for the reaction,in $kJ \ mol^{-1}$ is: $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$