The activation energy for the reaction $2HI_{(g)} \to H_{2_{(g)}} + I_{2_{(g)}}$ is $200 \ kJ \ mol^{-1}$ at $600 \ K$. Calculate the fraction of molecules of reactant having energy equal to or greater than activation energy.

For the following reactions:
$A \xrightarrow{700 \ K}$ Product
$A \xrightarrow[\text{catalyst}]{500 \ K}$ Product
it was found that $E_{a}$ is decreased by $30 \ kJ/mol$ in the presence of a catalyst. If the rate remains unchanged,the activation energy for the catalysed reaction is (Assume pre-exponential factor is same):

The rate law for the reaction $2NO + Cl_2 \rightarrow 2NOCl$ is given by $\text{rate} = k[NO]^2[Cl_2]$. Under what conditions will the value of the rate constant $k$ increase?

If the activation energy of a reaction is $80.9 \, kJ \, mol^{-1}$,the fraction of molecules at $700 \, K$,having enough energy to react to form products is $e^{-x}$. The value of $x$ is ....... . (Rounded off to the nearest integer) $[$Use $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$

The activation energy of a chemical reaction can be determined by:

Which plot of $\ln k$ vs $\frac{1}{T}$ is consistent with the Arrhenius equation?