question_answer

In terms of Arrhenius equation, \[k=A{{e}^{-{{E}_{a}}RT}}\]the  temperature  dependence  of rate constant (k) of a chemical reaction is written. Then, the activation energy \[({{E}_{a}})\] of the reaction can be calculated by plotting.

A) \[\text{log k vs}\frac{\text{1}}{\text{logT}}\]     

B) \[\log \text{k vs }\frac{1}{T}\]

C) \[\text{k vsT}\]                

D) \[\text{k vs }\frac{1}{\log T}\]

Correct Answer: B

Solution :

According to Arrhenius equation, \[k=A{{e}^{-{{E}_{a}}/RT}}\] \[\text{In k = In A-}\frac{{{\text{E}}_{\text{a}}}}{\text{RT}}\]or \[\log k=\log A-\frac{E}{2.303RT}\] Hence, E is calculated with the help of slope.