The half-reaction at the cathode in an electrochemical cell is given below. What other half-reaction would most likely occur at the anode to produce a spontaneous reaction?Zn2+(aq) + 2e- Zn(s)Click for a reduction potential chartA.H2(g) 2H+(aq) + 2e-B.K+(aq) + e- K(s)C.Al(s) Al3+(aq) + 3e-D.Zn(s) Zn2+(aq) + 2e-
Question
The half-reaction at the cathode in an electrochemical cell is given below. What other half-reaction would most likely occur at the anode to produce a spontaneous reaction?Zn2+(aq) + 2e- Zn(s)Click for a reduction potential chartA.H2(g) 2H+(aq) + 2e-B.K+(aq) + e- K(s)C.Al(s) Al3+(aq) + 3e-D.Zn(s) Zn2+(aq) + 2e-
Solution
The half-reaction at the cathode is a reduction reaction, where Zn2+ is gaining electrons to become Zn. For a spontaneous reaction to occur, the half-reaction at the anode must be an oxidation reaction, where a substance loses electrons.
Looking at the options:
A. H2(g) 2H+(aq) + 2e- is a reduction reaction (gaining electrons), so it cannot occur at the anode.
B. K+(aq) + e- K(s) is also a reduction reaction, so it cannot occur at the anode.
C. Al(s) Al3+(aq) + 3e- is an oxidation reaction (losing electrons), so it could occur at the anode.
D. Zn(s) Zn2+(aq) + 2e- is also an oxidation reaction, but it's the reverse of the cathode reaction. It's unlikely for the same substance to be both oxidized and reduced in the same cell.
Therefore, the most likely half-reaction to occur at the anode is C. Al(s) Al3+(aq) + 3e-.
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