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An aqueous solution was prepared containing 1.0mol of AgNO3 and 1.0mol of FeSO4 in 1.00 dm^3. of water. When equilibrium was established, there was 0.44mol of Ag+(aq) in the mixture. Ag + (aq) + Fe2 + (aq) <==> Ag(s) + Fe3+ (aq) . What is the numerical value of Kc? . A 0.35 B 0.62 C 1.62 D 2.89

Verified Answer :

Kc = [Fe3+]/ ([Ag+] [Fe2+]) 
Initial concentrations [Ag+]= [Fe2+]= 1.0 mol/ dm^3 [Fe3+] =0.0 mol/dm^3 
change: Ag+: (1.0 - .44) mol/dm^3 = 0.56 mol/ dm^3 = change of Fe2+. Change of Fe3+ is 0.56 mol/dm^3. 
Equilibrium concentrations [Ag+] = [Fe2+] = 0.44 mol/dm^3 [Fe3+] = 0.56 mol/dm^3 

Kc = 0.56/0.44^2 dm^3/mol = 2.89 dm^3 /mol

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