Chloride ions are added to the Ag|Ag* half-cell of the cell Ag|Ag*||Cu2|Cu to precipitate AgCl (s). The cell voltage is then measured to be +0.072 V at 298 K. If [Cu²*] = 1.0 M in the Cu2+|Cu half cell, what is [Ag*] in the Ag|Ag* half-cell? (First step: You will need to use the data in Table 17-1 to calculate E'cell.) Give your answer to two significant figures. Ecell = E°cell - (0.0257 V/n) In(Q) E'cell = E'ox + E°red

2+ Consider an electrochemical cell made up of Cu Cu²+ and Ag | Agt half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E £º =0 ロ→ロ V 2+ Calculate the standard emf of a cell that uses the Cu Cu²+ and Ag | Ag* half-cell reaction at 25 °C. Round your answer to 3 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. X ปี x10 Ś X Ś

A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 ∘C. The initial concentrations of Pb2+ and Cu2+ are 5.30×10−2 M and 1.50 MM, respectively. What is the cell potential when the concentration of Cu2+ has fallen to 0.250 M ? What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.35 V?   I think an ICE table needs to be used for these questions but im not sure.

Please explain, answer 0.57 V