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A second‐order reaction was observed. The reaction rate constant at 3 °C was found to be...

A second‐order reaction was observed. The reaction rate constant at 3 °C was found to be 8.9 x 10‐3 L/mol and 7.1 x 10‐2 L/mol at 35 °C. What is the activation energy of this reaction? 

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Homework Answers

Answer #1

Given,

Rate constant(k1) = 8.9 x 10-3 L/mol

Rate constant(k2) = 7.1 x 10-2 L/mol

Temperature(T1) = 3oC + 273.15 = 276.15 K

Temperature(T2) = 35oC + 273.15 = 308.15 K

We know the relation between Rate constant, temperature and activation energy,

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

Substituting the known values,

ln [7.1 x 10-2 L/mol /8.9 x 10-3 L/mol] = Ea /8.314 J /K.mol [ 1/276.15 -1/308.15]

2.0766 = Ea /8.314 J /K.mol x (0.0003760)

Ea = 45912 J/mol

Ea = 45.9 kJ/mol

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