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Chapter 17: Problem 33

Which half-reaction would be more likely to be an oxidation: one with a standard electrode potential of \(-0.42 \mathrm{V}\) , or one with a standard electrode potential of \(+0.42 \mathrm{V} ?\) Explain your answer.

Short Answer

Expert verified
The half-reaction with a standard electrode potential of -0.42 V is more likely to be an oxidation.

Step by step solution

01

Understanding Standard Electrode Potentials

Firstly, comprehend the fundamentals of Standard Electrode Potentials (SEPs). A Redox reaction involves both reduction and oxidation half-reactions. When an element loses electrons, it is said to be oxidized, and when it gains, it's reduced. The SEP measures the tendency of a half-cell to either gain or lose electrons - in essence, be reduced or oxidized.
02

Interpreting SEPs

An element with a negative SEP better prefers to lose its electrons and become oxidized, while a positive SEP favors gaining electrons, or reduction. As such, an electrode with a lower (more negative) SEP will function as the anode (where oxidation occurs) while the other with higher (more positive) SEP will act as the cathode (where reduction takes place).
03

Comparison

Given the SEP values of -0.42 V and +0.42 V, we have to decide which half-reaction is more likely to be an oxidation. Given the principles laid out in step 2, it can be deduced that the half-reaction with an SEP of -0.42 V is more likely to be an oxidation.

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