Answer:
The activation energy is 7.11 × 10⁴ J/mol.
Explanation:
Let's consider the Arrhenius equation.
[tex]lnk=lnA-\frac{Ea}{R} .\frac{1}{T}[/tex]
where,
k is the rate constant
A is a collision factor
Ea is the activation energy
R is the ideal gas constant
T is the absolute temperature
The plot of ln k vs 1/T is a straight line with lnA as intercept and -Ea/R as slope. Then,
[tex]\frac{-Ea}{R} =-8.55 \times 10^{3} K^{-1} \\Ea= 8.55 \times 10^{3} K^{-1} \times 8.314 \frac{J}{K.mol} =7.11 \times 10^{4} J/mol[/tex]
