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: [AIPMT 2003]

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 :

[a] Arrhenius equation \[k=A{{e}^{-E/RT}}\]

\[\ln \,k=\ln \,A-\frac{E}{RT}\]

or         \[\log \,k=\log \,A-\frac{E}{2.303\,RT}\]

Hence, E is calculated with the help of slope of following