Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a cell containing 0.150 L of a 0.250 M solution of CuSO4 for 2.00 hours. The cathodic half-reaction is Cu2+ + 2e- → Cu and the anodic half-reaction is Zn → Zn2+ + 2e-. The cell has a standard potential of 1.10 V at 298 K. What is the current density of the cell?

Question

Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a cell containing 0.150 L of a 0.250 M solution of CuSO4 for 2.00 hours. The cathodic half-reaction is Cu2+ + 2e- → Cu and the anodic half-reaction is Zn → Zn2+ + 2e-. The cell has a standard potential of 1.10 V at 298 K. What is the cu

Answer 1

To calculate the current density, we need to know the area of the electrode through which the current is passing. However, this information is not provided in the problem. If you can provide the area of the electrode, we can calculate the current density using the formula:Current density  J  = Current  I  / Electrode area  A If you provide the electrode area, I can help you calculate the current density.