Chemistry - Chemical Kinetics Question with Solution | TestHub

The increase in the reaction rate constant is given by the Arrhenius equation: $\ln \left(\frac{k_2}{k_1}\right)=\frac{E_a}{R}\left(\frac{\Delta T}{T_1{T}_2}\right)$. To find the maximum increase, we compare the ratio $\frac{E_a\cdot \Delta T}{T_1{T}_2}$ for each experiment:

Exp 1: $\frac{40\times 10}{200\times 210}=0.0095$

Exp 2: $\frac{90\times 20}{300\times 320}=0.0188$ (Maximum value)

Exp 3: $\frac{80\times 10}{300\times 310}=0.0086$

Exp 4: $\frac{100\times 10}{300\times 310}=0.0108$

Thus, Experiment 2 shows the maximum increase in rate, making (A) the correct option.