Question

The activation energy of a reaction is 55.6 kJ/mol and the frequency factor is 1.5×1011/s. Calculate the rate constant of the reaction at 23 ∘C. Express your answer using two significant figures.

Answer #1

Given data:

Activation energy Ea = 55.6 kJ/mole = 55600 J/mole.

Frequency Factor A = 1.5 x 1011 s^{-1}.

T = 23 ^{o}C = 23 + 273 = 296 K

Molar gas constant = R = 8.314
J.K^{-1}.mole^{-1}.

Rate constant (k) = ?

Arrhenius equation stated as

k=A*exp^{(-Ea/R*T)}

On substituting all the known values,

k=A*exp^{(-Ea/R*T)}.

k= (1.5 x
10^{11}) exp^{[-55600 / (8.314 x 296)]}.

k= (1.5 x
10^{11}) exp^{[-22.59]}.

k= (1.5 x
10^{11}) (1.54 x 10^{-10})

k= 23.1
s^{-1}.

Is the rate constant for the reaction under given condition.

**====================XXXXXXXXXXXXXXXX=======================**

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