# Problem: An electrochemical cell (battery) consists of a Cu plate immersed in 100 mL of 0.055 M Cu2+ solution and a Zn plate immersed in 100 mL of 0.550 M Zn2+ 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 105 seconds.The standard reduction potentials are given below:Cu2+ (aq) + 2 e- → Cu (s)              ε°red = + 0.34 VZn2+ (aq) + 2 e- → Zn (s)               ε°red = - 0.76 VWhat are the concentrations of cations (Cu2+ and Zn2+) in the respective compartments after the discharge? Please circle your answer(s).

###### FREE Expert Solution

We are asked to calculate the concentrations of cations (Cu2+ and Zn2+) in the respective compartments after the discharge.

We go through the following steps to solve the problem:

Step 1. Calculate the moles electrons transferred
Step 2. Calculate moles Zn2+ produced and and Cu2+ consumed
Step 3Calculate moles initially present
Step 4. Calculate new concentrations

Step 1. Calculate the moles electrons transferred

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###### Problem Details

An electrochemical cell (battery) consists of a Cu plate immersed in 100 mL of 0.055 M Cu2+ solution and a Zn plate immersed in 100 mL of 0.550 M Zn2+ 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 105 seconds.

The standard reduction potentials are given below:

Cu2+ (aq) + 2 e- → Cu (s)              ε°red = + 0.34 V

Zn2+ (aq) + 2 e- → Zn (s)               ε°red = - 0.76 V

What are the concentrations of cations (Cu2+ and Zn2+) in the respective compartments after the discharge? Please circle your answer(s).

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 Electroplating concept. If you need more Electroplating practice, you can also practice Electroplating practice problems.