## electrochemical series 6.45

$E_{cell} = E_{cell}^{\circ}-\frac{RT}{nF}\ln Q$

705121606
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### electrochemical series 6.45

We are given a list of metals and asked to order them starting with the most strongly reducing metal. I looked up the standard values in the appendix and this list was from most negative to most positive. Since these values correlate to the reduction potentials, why does a more negative value parallel to the most strongly reduced? I thought it meant that the more positive it is the greater the reduction potential. Is the question asking which is more strongly reduced or which is the strongest reducing agent?

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### Re: electrochemical series 6.45

The question asks you to order the metals starting with the most strongly reducing metal. The "most strongly reducing metal" is the strongest reducing agent, which is the metal half-reaction with the most negative E^0 value (in this question, Al). You are right that the more positive the E^0, the greater the reduction potential for a metal. Reduction potential refers to the metal's propensity to be reduced, not its strength as a reducing agent. Species that are strongly reducing (large negative E^0) are likely to get oxidized in a redox reaction.

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