Question

The rate constants of a reaction at 500K is 0.02 S-1. Its
Activation Energy (E) is 18.230 KJ. Calculate Arrhenius
constant?
(A) 1.3
B) 1.2

(C) 1.4

(D) 1.6
​

Answer 1

Explanation:

1.6 is the correct answer after substituting the given values in arhenius equation

Answer 2

Answer:

Arrhenius constant= (D) 1.6.

Explanation:

The Arrhenius equation in physical chemistry is a formula for the temperature sensitivity of reaction rates. Based on the research of Dutch chemist Jacobus Henricus van 't Hoff, who had noted in 1884 that the van 't Hoff equation for the temperature dependence of equilibrium constants suggests such a formula for the rates of both forward and reverse reactions, Svante Arrhenius proposed the equation in 1889. This equation has numerous and significant applications in calculating the energy of activation and the rate of chemical processes. Arrhenius explained and justified the calculation using physical principles.

It is represented as = $k=Ae^{\frac{-Ea}{RT} }$

Where, k= Rate constant

A= Pre exponential constant or Arrhenius constant

Ea= Activation energy

R= Universal gas constant

T= temperature

In the given problem,

k= 0.02 s⁻¹

E= 18.230 KJ= 18230 J

R= 8.314 J⋅mol⁻¹⋅K⁻¹

T= 500K

According to the Arrhenius Equation, $k=Ae^{\frac{-Ea}{RT} }$,

$0.02= Ae^{\frac{-18230}{8.314* 500 }$

or, ln 0.02= lnA + ($\frac{-18230}{4157}$)

or, -3.912= lnA+  (-4.385)

or, ln A= 4.385- 3.912= 0.473

or, A= 1.604≅ 1.6.

So, the option D= 1.6 is the correct answer.

To learn more about Arrhenius equation, please visit:

https://brainly.in/question/12223513

https://brainly.in/textbook-solutions/q-define-average-rate-instantaneous-rate-1?source=qa-qp-match#q-write-arrhenius-equation-explains-terms-involved

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