Question

The decomposition of a hydrocarbon follows the equation $k=(4.5\times {10}^{11}{s}^{-1})e^{-28000/K/T}$. What will be the value of activation energy?

• A. $669kJmo{l}^{-1}$
• B. $232.79kJmo{l}^{-1}$
• C. $4.5\times {10}^{11}kJmo{l}^{-1}$
• D. $28000kJmo{l}^{-1}$

Answer 1

The correct option is B $232.79kJmo{l}^{-1}$

Arrhenius equation, $k=A{e}^{-E_a/RT}$

Given equation is

$k=(4.5\times {10}^{11}{s}^{-1})e^{-28000K/T}$

Comparing both the equations, we get

$-\frac{E_a}{RT}=-\frac{28000K}{T}$

$E_a=28000K\times R=28000K\times 8.314J{K}^{-1}mo{l}^{-1}$

$=232.79kJmo{l}^{-1}$.