question_answer

The temperature dependence of rate constant \[(k)\] of a chemical reaction is written in terms of Arrhenius equation\[,\]\[k=A{{e}^{-{{E}^{*}}/RT}}\]. Activation energy \[({{E}^{*}})\] of the reaction can be calculated by ploting

A) \[\log k\,\,vs\frac{1}{T}\]                            

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

C) \[k\,\,vs\,\,T\]                 

D)  \[k\,\,vs\,\,\frac{1}{\log T}\]

Correct Answer: A

Solution :

Arrhenius equation,\[k=A{{e}^{-E/RT}}\]                 \[\ln k=\ln A-\frac{E}{RT}\] or            \[\log k=\log A-\frac{E}{2.303RT}\] Hence, \[E\] is calculated with the help of slope of following graph