The rate constant of the reaction I⁻(aq) + H₂O₂(aq) → H₂O(l) + IO−(aq) varies slowly with ionic strength, even though the Debye–Hückel limiting law predicts no effect. Use the following data from 25°C to find the dependence of log k_r on the ionic strength:

Evaluate the limiting value of k_r at zero ionic strength. What does the result suggest for the dependence of log γ on ionic strength for a neutral molecule in an electrolyte solution?

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I/(mol kg-¹) k₁/(dm³ mol-¹ min-¹) 0.0207 0.663 0.0525 0.670 0.0925 0.679 0.1575 0.694