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what is the activation energy(Ea) of a first order reaction is the reaction rate constant(k) increases...

what is the activation energy(Ea) of a first order reaction is the reaction rate constant(k) increases from 0.0300 min to 0.500 min as the temperature increases from 20.0 C to 45.0 C?

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Answer #1

The temperature dependency of rate constant is given by Arrhenius equation.

According to Arrhenius equation,

k = k0e-Ea/RT Where Ea is the activation energy and k0 is the frequency factor. Applying logarithm both sides and applying for two different states, we get the relation independant of frequency factor.

ln(k1/k2) = - Ea/R * [(1/T1)-(1/T2)]

Substituting the values at two different states,

We get

ln(0.3/0.5) = -Ea/8.314 [ 1/293 - 1/318]

Ea comes out to be = 15.828 kJ/mol

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