CuSO4 (aq) + 2Ag(s) Ag2SO4(aq) + + Cu(s) write out the oxidation half reaction and identify which chemical a) species is oxidized b) species is reduced → write out the reduction half reaction and identify which chemical c) Calculate the cell potential for a galvanic cell with this reaction. Predict whether the reaction will proceed spontaneously.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential CrO2−4 (aq)+4H2O(l)+3e−→  CrOH3(s)+5OH−(aq) =E0red−0.13V Cl2(g)+2e−→  2Cl−(aq) =E0red+1.359V   Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode.   Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell voltage under standard conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits. V

Write the half-cell equations, cell reaction equation and cell representation for the following galvanic cells: Nickel-Cadmium battery Cds) + NiO(OH)e) '(s) Cd(OH)2(s) + Ni(OH)2(s)

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)