Question

The temperature dependence of a reaction is represented by the Arrhenius equation: $lnk=-\frac{E_a}{RT}+lnA$
Which of 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 $\left(E_a\right)$.
• D. $Slope=-\frac{E_a}{R}$

Answer 1

Answer: (B)

$Slope=-\frac{E_a}{RT}$

The Arrhenius equation is $lnk=-\frac{E_a}{RT}+lnA$
It is equation of straight line of type $Y=mX+C$
$Y=lnk$
$X=\frac{1}{RT}$
Slope $=m=-\frac{E_a}{R}$
Y-intercept $=C=lnA$
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.