A quantity of 6.539 × 10^–2 g of metallic zinc is added to 100 ml of saturated solution of AgCl. The — Electrochemistry Chemistry Question

💡 Solution & Explanation

The relevant reaction is Zn(s) + 2Ag^+(aq) <=> Zn^2+(aq) + 2Ag(s). The standard cell potential for this is E°_cell = E°_Ag - E°_Zn = 0.80 - (-0.76) = 1.56 V. At equilibrium, log(Keq) = log([Zn^2+]/[Ag^+]^2) = (n × E°_cell) / 0.0591 = (2 × 1.56) / 0.0591 = 3.12 / 0.0591 = 52.79. Depending on the exact rounding used for 2.303RT/F (like 0.059 instead of 0.0591), it closely equals 52.88. Therefore, correct answer is B.