For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃) ₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V
Mg₂+(aq) + 2 e- → Mg(s) E° = -2.356 V
Estimate Keq at 25°C.

Question

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg₂+(aq) + 2 e- → Mg(s) E° = -2.356 V Estimate Keq at 25°C.

Quizplus · Accepted Answer

The standard cell potential (E°cell) is calculated as E°cell = E°cathode - E°anode = 0.800 V - (-2.356 V) = 3.156 V. Using the Nernst equation, ΔG° = -nFE°cell and ΔG° = -RTlnKeq, we find Keq = e^(nFE°cell/RT). With n = 2, F = 96485 C/mol, R = 8.314 J/mol·K, and T = 298 K, Keq ≈ 5.7 × 10^106.

For the Reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq)

For the Reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq)