Which of the following statements is not correct? 

Options

A. Larger the activation energy, lesser the value of rate constant of a reaction .
B. Larger the temperature, larger the value of rate constant of a reaction
C. Larger the activation energy, larger the effect of a given temperature increase on the rate constant
D. At the lower temperature, increase in temperature causes lesser change in the value of rate constant than at higher temperature

Explanation

We have `ln((k_(T_(2)))/(K_(T_(1)))) = -(E_(a))/(R)((1)/(T_(2)-T_(1)))=(E_(a))/(R)(T_(2) -T_(1))/(T_(2)T_(1)) = (E_(a))/(R)(Delta T)/((T_(1) + Delta T)T_(1))`