Question

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

• A. log k vs $\frac{1}{T}$
• B. log k vs $\frac{1}{logT}$
• C. k vs T
• D. k vs $\frac{1}{logT}$

Answer 1

Answer: (A)

Arrhenius equation $k=A{e}^{-E^{\ast }/RT}ln$ $k=lnA-\frac{E^{\ast }}{RT}$

(E* = energy of activation) or $logk=logA-\frac{E^{\ast }}{2.303RT}$

Compare this equation with the straight line equation,

i.e. $y=mx+c$

where ${}^{\prime }{m}^{\prime }$ is slope and $c^{\prime }$ is intercept Hence, $E$ is calculated with the help of following slope.