QuestionJuly 15, 2025

If E^circ (red) of a given half-cell is more negative than E^circ (red) for a standard hydrogen electrode, the half-cell will: A & tend to oxidize. B & tend to reduce. C & be at equilibrium. D & Not enough information is given.

If E^circ (red) of a given half-cell is more negative than E^circ (red) for a standard hydrogen electrode, the half-cell will: A & tend to oxidize. B & tend to reduce. C & be at equilibrium. D & Not enough information is given.
If E^circ (red) of a given half-cell is more negative than E^circ (red) for a standard hydrogen electrode, the half-cell will: A & tend to oxidize. B & tend to reduce. C & be at equilibrium. D & Not enough information is given.

Solution
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Answer

The half-cell will act as an anode and undergo oxidation. Explanation 1. Understand the concept of standard reduction potential The standard reduction potential (E^{\circ }(red)) indicates a half-cell's tendency to gain electrons. A more negative E^{\circ }(red) means it is less likely to be reduced compared to the standard hydrogen electrode (SHE), which has E^{\circ }(red) = 0 V. 2. Determine the behavior of the half-cell If a half-cell has a more negative E^{\circ }(red) than SHE, it will act as an anode in a galvanic cell, meaning it will undergo oxidation and lose electrons.

Explanation

1. Understand the concept of standard reduction potential<br /> The standard reduction potential ($E^{\circ }(red)$) indicates a half-cell's tendency to gain electrons. A more negative $E^{\circ }(red)$ means it is less likely to be reduced compared to the standard hydrogen electrode (SHE), which has $E^{\circ }(red) = 0$ V.<br /><br />2. Determine the behavior of the half-cell<br /> If a half-cell has a more negative $E^{\circ }(red)$ than SHE, it will act as an anode in a galvanic cell, meaning it will undergo oxidation and lose electrons.
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