Question

The temperature dependence of a reaction is represented by the Arrhenius equation :
ln $k=-\frac{E_a}{RT}+lnA$
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 $\text{lnk}=-\frac{E_a}{RT}+\ln A$
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.