This physics problem tests your understanding of fundamental physical laws and their applications. The step-by-step solution below breaks down the problem using relevant equations and physical reasoning.
ScanSolve AI Answer
To calculate the quantity of electricity required, we will use Faraday's laws of electrolysis. We need the molar mass of copper and Faraday's constant. We will assume copper is in the +2 oxidation state (Cu²⁺), which is common in copper compounds. Step 1: Determine the molar mass of copper and Faraday's constant. • Molar mass of copper (M_Cu) = 63.5 g/mol • Faraday's constant (F) = 96485 C/mol e⁻ Step 2: Write the half-reaction for the liberation of copper. Assuming copper is in the +2 oxidation state, the reduction half-reaction is: Cu^2+(aq) + 2e^- Cu(s) This reaction shows that 2 moles of electrons are required to liberate 1 mole of copper. Step 3: Calculate the number of moles of copper to be liberated. Given mass of copper (m) = 10 g. Number of moles (n_Cu) = massmolar mass n_Cu = 10 g63.5 g/mol n_Cu ≈ 0.15748 mol Step 4: Calculate the total moles of electrons required. From the half-reaction, 2 moles of electrons are needed per mole of copper. Moles of electrons (n_e) = n_Cu × 2 n_e = 0.15748 mol × 2 n_e ≈ 0.31496 mol e⁻ Step 5: Calculate the quantity of electricity (charge) in coulombs. Quantity of electricity (Q) = n_e × F Q = 0.31496 mol e⁻ × 96485 C/mol e⁻ Q ≈ 30398.9 C Rounding to three significant figures: Q ≈ 30400 C The quantity of electricity required is: 30400 C What's next?