Abstract:
The kinetics of the interactions between silver nitrate and methyl iodide in aqueous solution
have been followed using a conductivity technique. The observed second-order rate constant
increases with initial concentration of silver nitrate so as to suggest that the true order is between 2
and 3. A simple formulation of the mechanism has been proposed. There is no noticeable change
in the rate of reaction due to the initial addition of the product of the reaction, viz., silver iodide.
It is concluded that the reaction is essentially homogeneous and that nitrate ion takes no chemical
part. The energies of activation are temperature dependent.
