A) \[k=A\cdot {{e}^{-{{E}_{a}}/RT}}\]
B) \[\log \,k=\log \,A-\frac{{{E}_{a}}}{2.303\,RT}\]
C) \[\log \,\frac{{{k}_{2}}}{{{k}_{1}}}=\frac{{{E}_{a}}}{2.303R}\left( \frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{1}}\cdot {{T}_{2}}} \right)\]
D) All of the above
Correct Answer: D
Solution :
Arrhenius equation gives relation between activation energy \[({{E}_{a}})\] and rate constant of reaction\[\left( K \right)\]. It can be represented in all the given forms.
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