Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, $T$ (K).
$\ln k = 14.34 - \dfrac{1.25 \times 10^{4}}{T}$
The energy of activation in kcal mol $^{-1}$ for the reaction is :
(Given : $k$ in s $^{-1}$ , $R = 1.987$ cal mol $^{-1}$ K $^{-1}$ )

Question

Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature,

T

(K).

\ln k = 14.34 - \dfrac{1.25 \times 10^{4}}{T}

The energy of activation in kcal mol

^{-1}

for the reaction is :
(Given :

k

in s

^{-1}

,

R = 1.987

cal mol

^{-1}

K

^{-1}

)

Quantrex Academy · Accepted Answer

Correct answer: A. 24.84

The Arrhenius equation is given by: k = A - (E_a)/(RT) The given equation is: k = 14.34 - 1.25 × 10^ 4 T Comparing the two equations: (E_a)/(R) = 1.25 × 10^ 4 E_a = 1.25 × 10^ 4 × R Substituting R = 1.987 cal mol ^ -1 K ^ -1 : E_a = 1.25 × 10^ 4 × 1.987 E_a = 24837.5 cal mol ^ -1 E_a = 24.8375 kcal mol ^ -1 24.84 kcal mol ^ -1 Answer: 24.84

Given below is an expression for the rate constant of a first order...

Options

Correct answer

Step-by-step solution

More from Chemical Kinetics