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
Fresh day bazuunelson, let's solve. Step 1: Write the half-reaction for copper deposition. During electrolysis, copper(II) ions gain electrons to form solid copper. Cu^2+(aq) + 2e^- Cu(s) Step 2: Calculate the moles of copper deposited. The molar mass of copper (Cu) is 63.5 g/mol. Moles of Cu = Mass of CuMolar mass of Cu Moles of Cu = 1.48 g63.5 g/mol Moles of Cu ≈ 0.023307 mol Step 3: Calculate the moles of electrons transferred. From the half-reaction, 1 mole of Cu requires 2 moles of electrons. Moles of electrons = Moles of Cu × 2 Moles of electrons = 0.023307 mol × 2 Moles of electrons ≈ 0.046614 mol Step 4: Calculate the total charge (Q) passed. Faraday's constant is 96500 C/mol e^-. Charge (Q) = Moles of electrons × Faraday's constant Charge (Q) = 0.046614 mol × 96500 C/mol Charge (Q) ≈ 4500.85 C Step 5: Convert time to seconds. The time given is 2.5 hours. Time (t) = 2.5 hours × 60 min/hour × 60 s/min Time (t) = 9000 s Step 6: Calculate the amount of current (I) passed. The relationship between charge, current, and time is Q = I × t. I = (Q)/(t) I = 4500.85 C9000 s I ≈ 0.500 A The amount of current passed is approximately 0.500 A. Send me the next one 📸