Given the following standard reduction potentials, Ag⁺(aq) + e^- $\rarr$ Ag(s) E° = 0.80 V
Ag(NH₃) ₂⁺(aq) + e^- $\rarr$ Ag(s) + 2NH₃(aq) E° = 0.04 V
Calculate the formation constant of Ag(NH₃) ₂⁺at 25°C.

Question

Given the following standard reduction potentials, Ag⁺(aq) + e^-

\rarr

Ag(s) E° = 0.80 V
Ag(NH₃) ₂⁺(aq) + e^-

\rarr

Ag(s) + 2NH₃(aq) E° = 0.04 V
Calculate the formation constant of Ag(NH₃) ₂⁺at 25°C.

Quizplus · Accepted Answer

To calculate the formation constant, we need to use the Nernst equation: E°cell = E°cathode - E°anode = -0.76 V ΔG° = -nFE°cell = -2*96485*0.76 = -146946.4 J/mol ΔG° = -RTlnK K = e^(-ΔG°/RT) = e^(-(-146946.4)/(8.314*298)) = 6.9 x 10^10 Therefore, the formation constant of Ag(NH₃)₂⁺ is 6.9 x 10^10. The correct answer is C.

Given the Following Standard Reduction Potentials, Ag+(aq)+ E- →\rarr→ Ag(s)E° = 0

Given the Following Standard Reduction Potentials, Ag⁺(aq)+ E^- $\rarr$ Ag(s)E° = 0