Abstract
The value of energy and entropy of activation, obtained by applying the theory of absolute reaction rates for the diffusion of ·002 M ferric ion in 1-N sulphuric acid at varying temperatures, is found to be 9·8 K-cals. and −23·8 cal./degree respectively. The negative value of entropy of activation can be explained due to stronger polarization of the solvent by the enhanced electrostatic field, which is caused as a result of approaching of the two reactants of like sign towards each other.
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