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

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Chemistry

Jefferson Neal

8 November, 14:42

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

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Cheerio · Answer 1

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