A) is independent of temperature
B) increases with temperature
C) gets doubled for every 10 degree rise in temperature
D) decreases with temperature
Correct Answer: D
Solution :
According to Arrhenius equation, the relationship between the activation energy and temperature is \[k=A{{e}^{-{{E}_{a}}/RT}}\] \[\log \,k=\frac{-{{E}_{a}}}{2.303\,RT}+\log A\] \[\therefore \]Activation energy decreases with rise in temperature, thereby increasing the rate of the reaction.
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