Question

The temperature dependence of a reaction is represented by the Arrhenius equation :
ln $ k =- \frac{E_{a}}{RT}+ ln A$
Which among the following is wrong conclusion about the given plot?

• A. Intercept of the line = ln A
• B. Slope $= - \frac{E_{a}}{RT}$
• C. Reaction with high activation energy is more temperature sensitive than that of low activation energy (E_a).
• D. Slope $= - \frac{E_{a}}{R}$

Answer 1

Answer: (B)

The Arrhenius equation is $\text{lnk}=-\frac{E_{ a }}{R T}+\ln A$
It is equation of straight line of type $Y = mX + C$
$Y =\text{lnk}$
$X =\frac{1}{ RT}$
Slope $= m =-\frac{ E _{ a }}{ R }$
$Y$-intercept $=C=\ln A$
Reaction with high activation energy is more temperature sensitive than that of low activation energy (Ea). When $E _{a}$ is high, $\frac{ E _{a}}{R}$ is high and slope is more negative.