Calculate the potential difference (in volts) between two half-cells when one half-cell contains a copper (Cu) electrode immersed in a 0.10 M Cu²⁺ solution and the other half-cell contains a silver (Ag) electrode immersed in a 0.20 M Ag⁺ solution. (Use standard reduction potentials)
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The standard reduction potential for the Cu2+ / Cu half-reaction is +0.34 V, and the standard reduction potential for the Ag+ / Ag half-reaction is +0.80 V.
The potential difference between two half-cells is determined by subtracting the reduction potential of the anode half-reaction from the reduction potential of the cathode half-reaction (or adding the oxidation potentials in reverse).
Here, the Cu2+ / Cu half-reaction is the anode and the Ag+ / Ag half-reaction is the cathode. Therefore, we subtract the standard reduction potential of the Cu2+ / Cu half-reaction from the standard reduction potential of the Ag+ / Ag half-reaction:
Potential difference = (+0.80 V) - (+0.34 V)
= 0.46 V
Therefore, the potential difference between the two half-cells is 0.46 volts.
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