Consider a zinc-copper electrochemical cell in which the half-reaction Zn(s) → Zn²⁺(aq) + 2e⁻ occurs at the anode and the half-reaction Cu²⁺(aq) + 2e⁻ → Cu(s) occurs at the cathode. If the concentration of Zn²⁺(aq) in the anode compartment is 0.500 M and the concentration of Cu²⁺(aq) in the cathode compartment is 0.0250 M, calculate the current density when a current of 2.50 A is passed through the cell. (Assume that the temperature and pressure are constant and that the electrodes are inert.)

Question

Consider a zinc-copper electrochemical cell in which the half-reaction Zn(s) → Zn²⁺(aq) + 2e⁻ occurs at the anode and the half-reaction Cu²⁺(aq) + 2e⁻ → Cu(s) occurs at the cathode. If the concentration of Zn²⁺(aq) in the anode compartment is 0.500 M and the concentration of Cu²⁺(aq) in the cathode compartment is 0.0250 M, calculate the current density when a current of 2.50

Answer 1

To calculate the current density, we need to know the area of the electrode. However, since the area of the electrode is not provided, we can only calculate the current density in terms of the electrode area.Current density  J  is defined as the current  I  divided by the area  A  of the electrode:J = I / AGiven that the current  I  is 2.50 A, we can express the current density as:J = 2.50 A / AThis means that the current density is 2.50 A per unit area of the electrode. Without knowing the actual area of the electrode, we cannot provide a numerical value for the current density.