The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, `k=Ae^(-E_(a)//RT))` Activation energy `(E_(a))` of the reaction can be calculate by plotting

Options

A. `log k vs (1)/(log T)`
B. `k vs T`
C. `k vs (1)/(log T)`
D. `log k vs (1)/(T)`

Answer

D

Explanation

`k=Ae^(-E^(**)//RT)`
`log_(e)k=log_(e)=(-E^(**))/(RT)`
Thus, a plot of log k vs 1/T will be a straight line with slop `-E^(**)//R`. Knowing the value of gas constants, activation enery `E^(**)` can be calculated.