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Electrochemistry and balancing redox equations

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Electrochemistry Part III

1- Balance each redox reaction occurring in acidic aqueous solution. Express your answer as a chemical equation. Identify all of the phases in your answer.

Ni(s)+Cd 2+ (aq)→Ni 2+ (aq)+Cd(s)
Ni(s)+Cd 2+ (aq)→Ni 2+ (aq)+Cd(s)
3MnO 4 − (aq)+5Al(s) + 24H+(aq)→3Mn 2+ (aq)+5Al 3+ (aq) + 12H2O (aq).

2- Balance each redox reaction occurring in basic aqueous solution.

2MnO − 4 (aq)+Br − (aq) +H2O→2MnO 2 (s)+BrO − 3 (aq) + 2OH-
4Ag(s)+8CN − (aq)+O 2 (g) +2H2O→4Ag(CN) − 2 (aq) +4OH-
O − 2 (aq)+Al(s)→NH 3 (g)+AlO − 2 (aq) (provide double check this equation since the left since the left side has no N.)

3- Calculate the standard cell potential (E ∘ ) for the reaction X(s)+Y + (aq)→X + (aq)+Y(s) if K = 5.82×10−3.Express your answer to three significant figures and include the ...

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The solution assists in solving the electrochemistry and balancing redox equations.

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