500 mL of 0.150 M AgNO₃ solution were added in 500 mL of 1.09 M Fe²⁺ solution and the reaction is allowed to reach an equilibrium at $25^{\circ }\text{C}$.

${\text{Ag}}^{+}\left(\text{aq}\right)+{\text{Fe}}^{2+}\left(\text{aq}\right)\rightleftharpoons {\text{Fe}}^{3+}\left(\text{aq}\right)+\text{Ag}\left(\text{s}\right)$

For 25 mL of the solution, 30 mL of 0.0832 M KMnO₄ were required for oxidation. Calculate equilibrium constant (M^-1) of the reaction at $25^{\circ }\text{C}$.
[Report your answer by rounding it upto nearset whole number]