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Which of the following statements is not correct?

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Larger the activation energy, lesser the value of rate constant of a reaction

Larger the temperature, larger the value of rate constant of a reaction

Larger the activation energy, larger the effect of a given temperature increase on the rate constant

At the lower temperature, increase in temperature causes lesser change in the value of rate constant than at higher temperature

answer is D.

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Detailed Solution

We have $\ln (\frac{k_{T_{2}}}{k_{T_{1}}}) = - \frac{E_{a}}{R} (\frac{1}{T_{2}} - \frac{1}{T_{1}}) = \frac{E_{a}}{R} \frac{T_{2} - T_{1}}{T_{2} T_{1}} = \frac{E_{a}}{R} \frac{Δ T}{(T_{1} + Δ T) T_{1}}$

Since the lower temperature occurs in the denomination, the value $k_{T_{2}} / k_{T_{1}}$ will be larger on increasing the temperature by $Δ T$ .

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