A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction:

3Cu^+2(aq)+2Al(s) ---> 3Cu(s)+2Al^3+(aq)

Suppose the cell is prepared with 7.97 M Cu+2 in one half-cell and 2.50 M Al+3 in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.

2.01V ( To three significant digits)

Explanation:

First we show the standard reduction potentials of Cu2+(aq)/Cu(s) system and Al3+(aq)/Al(s) system. We can clearly see from the balanced redox reaction equation that aluminium is the anode and was the oxidized specie while copper is the cathode and was the reduced specie. This observation is necessary when substituting values of concentration into the Nernst equation.

The next thing to do is to obtain the standard cell potential as shown in the image attached and subsequently substitute values of concentration and standard cell potential into the Nernst equation as shown. This gives the cell potential under the given conditions.

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