## Calculate the E^o cell for the following equation. Use these standard potentials .

### Question:

Calculate the E^o cell for the following equation. Use these standard potentials.

### Answer & Explanation:

Cu(s)+Ag+(aq)>>>>Cu+(aq)+Ag(s)

Standard Cell Potential

Oxidation and reduction-half reactions classify the redox reactions. The value of standard cell potential, which is denoted by Eocell is calculated when the value of Eoanode is subtracted by the value of Eocathode.

**The complete redox reaction of an electrochemical cell is shown below.**

Cu(s)+Ag+(aq)→Cu+(aq)+Ag(s)

In this reaction, copper is oxidized and acts as the reducing agent. Silver is reduced in the reaction and acts as the oxidising agent.

In an electrochemical cell, the oxidation process occurs at anode. The oxidation half-reaction is shown below.

Cu(s)→Cu+(aq)+e−Eooxi=−0.52V

The standard oxidation potential of the above reaction is -0.52 V. Therefore, the standard reduction potential is 0.52 V.

The reduction process occurs at cathode. The reduction half-reaction is shown below.

Ag+(aq)+e−→Ag(s)Eored=0.80V

Now, the standard cell potential is calculated by the formula.

Eocell=Eocathode−Eoanode

Substitute the values in the above equation.

Eocell=0.80V−0.52V=0.28V

Hence, the standard cell potential is

0.28V.

## Answer ( 1 )

Answer Above.