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^(-Ea // RT)`
or `log k= log A-(E_(a))/(2.303 RT)`
Comparing the above equation with
y=mx + c
`y=log k, x=(1)/(T)`
Thus a plot of log k vs `1 // T` should be a straight line, with slope equal to `-E_(a) // 2.303 RT` and intercept equal to log A

`:. "Slope"=(-E_(a))/(2.303 R)`
or `E_(a)=-2.303 R xx "Slope"`