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Oxidation and Reduction in Standard Conditions

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At standard conditions indicate whether each of the following is true. Explain for each

A. Pb(s) can reduce NI2+
b. Hg2 2+( aq) can reduce Cu2+ n(aq)
c. H+ (g) can oxidize Sn(s).

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At standard conditions indicate wheather each of the following is true. Explain for each.

Response: To answer these questions you need to examine the table that shows standard reduction potentials in aqueous solution at 25 degrees C. These tables are usually found as an appendix near the back of most chemistry textbooks.

First, you identify the relevant half reactions. Then you need to determine which half reaction will proceed in the direction given. The reaction with the most ...

Solution Summary

This solution contains detailed explanations on why the statements of oxidation and reduction are true or false at standard conditions.

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Determination of Electrochemical Cell Potentials Under Non-Standard Conditions Using the Nernst Equation

Consider the electrochemical cell:
Pt|Cr2+(0.2752 M), Cr3+(1.705 M)||Co2+(0.2008 M)|Co
a. What is the cell potential (hint: you can solve the problem by half-reactions or by the over-all reaction, both will give you the same answer so you can double check yourself)?
b. Is the cell galvanic or electrolytic (must show math in part (a) to get credit for answer)?

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