Step 1 Zn 4OH Zn(OH) 4 2 2e Step 2 Zn(OH) 4 2 ZnO H 2 O 2OH (a) Verify that Step 2 of the Zn reaction is not an electrochemical reaction In other words, show that the oxidation states of all the elements stays the same (b) Commercial AA batteries use the same Zn anode and alkaline electrolyte as the one in the mercury cell, but use a MnO 2 cathode, which changes to MnOOH during the reaction Determine the balanced cathodic half reaction and overall reactions ( Hint Species in the half reactions may cancel out when they are added together to make the overall reaction Also, keep in mind that in an alkaline electrolyte, you will not have protons dissolved in water, but rather hydroxide ions )

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Question: Step 1: Zn + 4OH - Zn(OH) 4 2- + 2e - Step 2: Zn(OH) 4 2- ZnO + H 2 O + 2OH -

Step 1: Zn + 4OH^- Zn(OH)₄^2- + 2e^-

Step 2: Zn(OH)₄^2- ZnO + H₂O + 2OH^-

(a) Verify that Step 2 of the Zn reaction is not an electrochemical reaction. In other words, show that the oxidation states of all the elements stays the same.

(b) Commercial AA batteries use the same Zn anode and alkaline electrolyte as the one in the mercury cell, but use a MnO₂ cathode, which changes to MnOOH during the reaction. Determine the balanced cathodic half-reaction and overall reactions. (Hint: Species in the half-reactions may cancel out when they are added together to make the overall reaction. Also, keep in mind that in an alkaline electrolyte, you will not have protons dissolved in water, but rather hydroxide ions.)

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