Cell Potential Calculation

Question

For cell: Zn(s)|Zn²⁺(1 M)||Cu²⁺(1 M)|Cu(s), E°(Zn²⁺/Zn) = -0.76 V, E°(Cu²⁺/Cu) = +0.34 V. E°cell is:

RankGuru · Accepted Answer

1. **Identify Electrodes**: In the cell notation, the left side is always the **Anode** ($Zn$) and the right side is the **Cathode** ($Cu$).
2. **Formula**: $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$ (using reduction potentials).
3. **Values**:
   - $E^\circ_{cathode} = +0.34$ V.
   - $E^\circ_{anode} = -0.76$ V.
4. **Calculation**: $E^\circ_{cell} = (+0.34) - (-0.76) = 0.34 + 0.76 = +1.10$ V.
5. **Significance**: A positive $E^\circ_{cell}$ confirms that the cell reaction is spontaneous in the forward direction.

Cell Potential Calculation

Select the correct option:

🔒 Solution Hidden from View

More electrochemistry Practice Questions

In a spontaneous redox reaction, electrons flow from:

Primary function of a salt bridge in a galvanic cell is to:

More positive standard reduction potential indicates:

Nernst equation relates electrode potential to:

In a concentration cell with identical electrodes, driving force arises from:

Faraday's first law states mass deposited is proportional to:

According to Faraday's second law, masses of different substances liberated by same charge are propo...

How many faradays required to deposit 1.0 mol of Al (Al³⁺ + 3e⁻ → Al)?

During discharge of a lead storage battery, both electrodes are converted to:

Metal higher in electrochemical series (more negative E°) tends to:

Rusting of iron in moist air is electrochemical because:

In an electrolytic cell (as opposed to galvanic), the anode is:

About This Question

Solution