The temperature dependence of a reaction is represented by the Arrhenius euqation
In `k = (E_(a))/(RT) + In A`
Which among the following is wrong conclusion about the given plot?

Options

A. Intercept of the line `= In A`
B. Slope `= -(E_(a))/(RT)`
C. Reaction with high activation energy is more temperature sesitive than thatof low activation energy `(E_(a))`
D. Slope `= -(E_(a))/(R )`

Answer

B

Explanation

`In k = ln A-(E)/(RT)`
In `k = -(E_(a))/(R ) xx (1)/(T) + In A`
`y = mx + C`
(a) `C = In A` correct
(b) is wrong
`m = slope = -(E_(a))/(R )`