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Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will...

Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur between Mn metal and Cl2(g), when the two are brought in contact via 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. If no reaction will occur, leave all boxes blank. + +

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Answer #1

We first write the reduction half cell reactions for both Mn and Cl using the standard reduction potential table:

Mn2+ + 2e- ---> Mn(s) ; E = -1.185

Cl2(g) + 2e- ---> 2Cl-(aq) ; E = +1.36

So yes a reaction can occur, if we make Cl2 the cathode and Mn the anode.

So the oxidation reaction is:

Mn(s) ---> Mn2+(aq) + 2e- ; Eox = +1.185 V

Reduction reaction is:

Cl2(g) + 2e- ---> 2Cl-(aq) ; Ered = +1.36 V

The balanced net reaction is:

Mn(s) + Cl2(g) ---> 2Cl-(aq) + Mn2+(aq)

The standard potential for this cell is:

E0cell = Eox + Ered = 1.185+1.36 = 2.545 V

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