We’re being asked to calculate the initial potential (voltage) of the electrochemical cell.

We will use the **Nernst Equation** to calculate the cell potential. The Nernst Equation relates the concentrations of compounds and cell potential.

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{}}{\mathbf{-}}{\mathbf{}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}\mathbf{}\mathbf{V}}{\mathbf{n}}\mathbf{\right)}{\mathbf{logQ}}}$

E_{cell} = cell potential under non-standard conditions

E°_{cell} = standard cell potential

n = number of e^{-} transferred

Q= reaction quotient = [products]/[reactants]

We go through the following steps to solve the problem:

*Step 1**. Write the two half-cell reactions **Step 2**. Identify the oxidation half-reaction (anode) and the reduction half-reaction (cathode)**Step 3**. Determine the half-cell potentials (refer to the Standard Reduction Potential Table)**Step 4**. Calculate E**° _{cell }(standard).*

An electrochemical cell (battery) consists of a Cu plate immersed in 100 mL of 0.055 M Cu^{2+} solution and a Zn plate immersed in 100 mL of 0.550 M Zn^{2+} solution. The two compartments are connected by a salt bridge and the cell is maintained at 25 °C. The cell is discharged by passing a 10.00 mA current for 10^{5} seconds.

The standard reduction potentials are given below:

Cu^{2+} (aq) + 2 e^{-} → Cu (s) ε°_{red} = + 0.34 V

Zn^{2+} (aq) + 2 e^{-} → Zn (s) ε°_{red} = - 0.76 V

What is the initial potential (voltage) of the electrochemical cell? Please circle your answer.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.