Calculate the value of e°cell for the following reaction: 2au(s) + 3ca2+(aq) → 2au3+(aq) + 3ca(s)au3+(aq) + 3e- → au(s) e° = 1.50vca2+(aq) + 2e- → ca(s) e° = -2.87va) -4.37 vb) -1.37 vc) -11.6 vd) 1.37 ve) 4.37 v

The standard electrode potential of the cell is -4.37 V

Explanation:

For the given cell reaction:

The half reactions follows:

Oxidation half reaction:       ( × 2 )

Reduction half reaction:       ( × 3 )

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the of the reaction, we use the equation:

Putting values in above equation, we get:

Hence, the standard electrode potential of the cell is -4.37 V

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