The rate of a reaction quadruples when the temperature changes from 293K to 313K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.
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Solution
The Arrhenius equation at two different temperatures is as follows: log(k′k)=Ea2.303R[1T−1T′] k′k=4 log(4)=Ea2.303×8.314[1293−1313]
The energy of activation, Ea=52863.3J/mol=52.86kJ/mol.