PART A: Balance each redox reaction occurring in acidic aqueous solution. MnO4−(aq)+Al(s)→Mn2+(aq)+Al3+(aq). Express your answer as a chemical equation. Identify all of the phases in your answer.

PART B: The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction. Type the half-cell reaction that takes place at the anode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation.

PART C: The half-cell is a chamber in the voltaic cell where one half-cell is the site of an oxidation reaction and the other half-cell is the site of a reduction reaction. Type the half-cell reaction that takes place at the cathode for the iron-silver voltaic cell. Indicate the physical states of atoms and ions using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not include phases for electrons. Express your answer as a chemical equation.

PART D: How many minutes will it take to electroplate 15.1 g of gold by running 5.00 A of current through a solution of Au+(aq)? Express your answer to three significant figures and include the appropriate units.

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PART 1 Half the reactions are as follows 5AIs 5 Al3 aq ... View the full answer