Part A) Use the table \'Standard Reduction Potentials\' located in the \'Tables\

Question

Part A) Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Cd metal is put into a 1M aqueous Cu2+ solution. If a reaction will occur, write a balanced net ionic equation for the reaction.

Part B) Use a table of Standard Reduction Potentials to predict if a reaction will occur between Cd metal and F2(g), when the two are brought in contact via standard half-cells in a voltaic cell.If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution.

Reference (standard reduction potentials): http://cxp.cengage.com/contentservice/assets/owms01h/references/chemtables/gen_chem/eo.html

Explanation / Answer

Part A)

net-ionic equation,

Cd(s) + Cu2+(aq) --> Cd2+(aq) + Cu(s)

Eo = Ecathode - Eanode

     = 0.337 - (- 0.403)

     = 0.740 V

Eo for the reaction as written is +ve, therefore the reaction would occur when Cd is placed into Cu2+ solution.

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Part B)

net-ionic equation,

Cd(s) + F2(g) ---> Cd2+(aq) + 2F-(aq)

Eo = Ecathode - Eanode

     = 2.87 - (- 0.403)

     = 3.273 V

Eo for the reaction as written is +ve, therefore the reaction would occur when Cd is placed into F2(g).

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