$60 \%$ of a first order reaction was completed in 60 min , then $50 \%$ of the same reaction can be completed in: $[\log 4=0.60, \log 5=0.69]$

Identify the correct values to be plotted in the graph, the slope of which can be used to determine the activation energy of a reaction.

When the initial concentration of a zero order reaction is doubled, the half-life of the reaction is:

When the temperature of a reaction $\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$ is increased from 300 K to 310 K the rate constant increases by $12 \%$. What is the Activation energy of the reaction?