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

Answer

A

Explanation

Arrhenius equation `k=Ae^(-E//RT)`
` "In" K=I n A-(E^("*"))/(RT)` (E* = energy of actication
`or log K= log A ("E*")/(2.303RT)`
compare this equation with the straight line equation .,
i.e., `y=mx+c`
where 'm' is slope and 'C' intercept
Hence E' can be calculated with the help of following slope