A quantity of electricity equal to 6.95 × 104 C passes through an electrolytic cell that contains a solution of Sn4+(aq) ions. Compute the maximum chemical amount, in moles, of Sn(s) that can be deposited at the cathode.

4. Write the overall balanced equation for the spontaneous process occurring in the following cell. (Hint: this is the combination of two half-reactions. One is a reduction half-reaction, and the other is an oxidation half-reaction.) Then, calculate the standard potential, E°, for the cell. Zn (s) | Zn *2 (aq) || Cu +2 (aq) | Cu (s)

Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left half-cell contains 0.115 M Cu(NO₃)₂ (aq). Express your answer to three significant figures.

4. For the following redox reaction in a galvanic cell, write the oxidation half-reaction and the reduction-half reaction, and calculate the standard cell potential of the reaction. Use Table 1 from the background as needed. Explain how you identified which substance was oxidized and which was reduced. Show all of your work. Redox reaction: Cu(s) + 2 Fe* (aq) → Cu?+ (aq) + 2 Fe* (aq) Table 1. Standard reduction potentials. Half-Reaction E°(Volts) F,(g) + 2e → 2F (aq) CI, (g) + 2e → 2CI(aq) Br, () + 2e → 2Br(aq) Ag*(aq) + e¯ → Ag(s) +2.87 +1.36 +1.07 +0.80 Fe*(aq) + e → Fe²"(aq) +0.77 Cu²*(aq) + 2e' → Cu(s) +0.34 2H*(aq) + 2e¯ → H,(g) 0.00 Fe2*(aq) + 2e' → Fe(s) -0.44 Zn*(aq) + 2e' → Zn(s) -0.76 Al³*(aq) + 3e' → Al(s) -1.66 Mg"(aq) + 2e' → Mg(s) -2.37 Ca²"(aq) + 2e" → Ca(s) -2.87 K*(aq) + e' → K(s) -2.93 В U T T O Word(s)