Question

A rate constant obeys the Arrhenius equation, the factor A being 2.2  10^13 s-1 and the
activation energy being 150. kJ mol-1. What is the value of the rate constant at 227C, in
s-1?

Answer 1

4.743 x $10^{-3}$ s-1 is the value of the rate constant.

What is an Arrhenius equation?

The Arrhenius equation describes the relationship between the rate of reaction and temperature for many physical and chemical reactions.

As per Arrhenius equation,

k = Ae-Ea÷RT

T = 227 = 500.15 K

R = 0.008314 kJ/K mol

Ea = 150 kJ/mol

Ea÷RT

= 150÷(0.008314 x 500.15)

= 36.073

k = Ae-36.073 = (2.2 x $10^{13}$ s-1) (2.156 x $10-{16}$)

k = 4.743 x $10^{-3}$ s-1

So, the correct answer is option d) i.e. 4.7 x $10^{-3}$ s-1

As per Arrhenius equation,

k = Ae-Ea/RT

T = 227 = 500.15 K

R = 0.008314 kJ/K mol

Ea = 150 kJ/mol

Ea÷RT = 150÷(0.008314 x 500.15) = 36.073

k = Ae-36.073 = (2.2 x $10^{13}$ s-1)(2.156 x $10^{-16}$)

k = 4.743 x $10^{-3}$ s-1

Hence,  4.743 x $10^{-3}$ s-1 is the value of the rate constant.

Learn more about the Arrhenius equation here:

https://brainly.com/question/17924702

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