20. Electrochemistry

Given the following standard reduction potentials, determine Ksp for Hg₂Cl₂₍s) at 25 °C.

Hg₂²⁺ (aq) + 2 e^– → 2 Hg (l)                           E°red = + 0.789 V

Hg₂Cl₂ (s) + 2 e^– → 2 Hg (l) + 2 Cl ^– (aq)                E°red = + 0.271 V

What is the value of the cell potential for the 4 electron transfer reaction below if the equilibrium mixture contains 0.255 M of CH₄, 1.10 M CO₂, 0.388 M CO and 0.250 M H₂ at 25ºC?

                                     CH₄ (g) + CO₂ (g)  ⇌. 2 CO (g) + 2 H₂ (g)

Given the reaction: 2 Cl2 (g) + 2 H2O (g) ⇌ 4 HCl (g) + O2 (g) Kp = 7.5x10-2, calculate the Gibbs Free Energy change for the reaction below at 30ºC.

8 HCl (g) + 2 O2 (g) ⇌ 4 Cl2 (g) + 4 H2O (g)

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (a) Aqueous iodide ion is oxidized to I21s2 by Hg22+1aq2.

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion.

Calculate the equilibrium constant for each of the reactions in Problem 65.