Consider the galvanic cell shown below with a potential of 1.369 V at 25°C

Pb(s) | PbCl₂(s) | Cl^–(0.20 M) || Cr₂O₇^2–(0.20 M), Cr³⁺(0.20 M), H⁺(0.20 M) | Pt(s)

Determine the K_sp value for PbCl₂(s). 

Cr₂O₇^2–(aq) + 14 H⁺(aq) + 6 e^– → 2 Cr³⁺(aq) + 7 H₂O(l)          E°_red = 1.232 V
Pb²⁺(aq) + 2 e^– → Pb(s)                                                            E°_red = –0.126 V

For the given cell notation, write an overall cell reaction:

Mn(s) | Mn²⁺(aq) || Fe²⁺(aq) | Fe(s)

Draw the cell diagram, label which electrode is the anode and the cathode. Draw arrows to show the directions in which the ions and electrons flow.

Consider the following redox reaction:

2 NH₄⁺(aq) + MnO₄⁻(aq) → 2 MnO₂(s) + N₂(g) + 4 H₂O(l)

Write a shorthand notation for this reaction. In your notation, you can use an inert metal if necessary.

For the given cell notation, write an overall cell reaction:

Ni(s) | Ni²⁺(aq) || Br₂(l) | Br⁻(aq) | Pt(s)

Explain why we need an inert electrode at the cathode.

For the given electrochemical cell, cell potential is dependent on the copper concentration in the cathode half-cell.

Pt(s) | H₂(g, 1.0 atm) | H⁺(aq, 1.0 M) || Cu⁺(aq, ? M) | Cu(s)

This cell has an E_cell of 0.34 V. Determine the [Cu⁺] of the solution.

For the given electrochemical cell, cell potential is dependent on the pH of the solution.

Pt(s) | H₂(g, 1.0 atm) | H⁺(aq, ? M) || Ag⁺(aq, 1.0 M) | Ag(s)

This cell has an E_cell of 923 mV. Determine the pH of the solution.