Neco 2023 Chemistry Question 34

A galvanic cell is constructed with the half‑reactions:\n\n\(\text{Fe}^{3+}+e^{-}\rightleftharpoons\text{Fe}^{2+}\) \(E^{\circ}=+0.771\,\text{V}\)\n\n\(\text{Cu}^{2+}+2e^{-}\rightleftharpoons\text{Cu(s)}\) \(E^{\circ}=+0.340\,\text{V}\)\n\nThe cell operates at 25 °C with the following concentrations: \([\text{Fe}^{3+}]=0.010\,\text{M},\;[\text{Fe}^{2+}]=0.100\,\text{M},\;[\text{Cu}^{2+}]=0.050\,\text{M}.\n\n(a) Calculate the cell potential under these conditions using the Nernst equation.\n(b) State which electrode is the cathode and which is the anode.\n(c) If a current of 0.5 A flows for 30 min, how many grams of copper are deposited on the cathode? (Molar mass of Cu = 63.55 g mol⁻¹).