1. Tardigrade
  2. Question
  3. Chemistry
  4. 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 2 5° textC . ( textAg)+ ( textaq) + ( textFe)2 + ( textaq) leftharpoons ( textFe)3 + ( textaq) + textAg ( texts) For 25 mL of the final solution, 30 mL of 0.0832 M KMnO4 were required for oxidation. Calculate the equilibrium constant (in M-1) of the reaction at 2 5° textC . [Report your answer by rounding it up to the nearest whole number]

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Q. 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 $2 5^{^\circ } \text{C}$ .
$\left(\text{Ag}\right)^{+} \left(\text{aq}\right) + \left(\text{Fe}\right)^{2 +} \left(\text{aq}\right) \rightleftharpoons \left(\text{Fe}\right)^{3 +} \left(\text{aq}\right) + \text{Ag} \left(\text{s}\right)$
For 25 mL of the final solution, 30 mL of 0.0832 M KMnO4 were required for oxidation. Calculate the equilibrium constant (in M-1) of the reaction at $2 5^{^\circ } \text{C}$ .
[Report your answer by rounding it up to the nearest whole number]

NTA AbhyasNTA Abhyas 2022

Solution:

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