Thursday
September 18, 2014

Homework Help: Chem

Posted by Alex on Tuesday, February 26, 2008 at 9:45pm.

The following equations represent spontaneous reactions. From this evidence, set up a table of relative strengths of oxidizing and reducing agents. Write half-reaction equations and label the strongest oxidizing agent and reducing agent.

Co + Pd2+ ----> Co2+ + Pd
Pd + Pt2+ ----> Pd2+ + Pt
Mg + Co2+ ----> Mg2+ + Co

Of all the reactants all the ones on the left side were reducing agents and I labeled the rest oxidizing agents.

SOA
Pt2+
Pb2+
Co2+

SRA
Pd
Co
Mg

Table
Pe2+ + 2e ---> Pe
Pd2+ + 2e ---> Pd
Co2+ + 2e ---> Co
Mg2+ + 2e ---> Mg

Is that right?

Can someone help me with these questions..

1) A student is required to store an aqueous solution of iron (III) nitrate. She has a choice of a copper, tin, iron, or silver container. Predict wchihc container would be mos suitable for storing the solution.

2) An analytical chemist reacts an unknown metal X with a copper (II) sulfate solution, plating out copper metal. Metal X does not react with aqueous zinc nitrate. What is the order for these metal ions in decreasing tendency of the unknown metal? What other solutions might next be chosen to help identify the unknown metal?

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