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