This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Right bazuunelson, let's go. Step 1: Calculate the total charge (Q) passed. The current (I) is 40,000 A and the time (t) is 1 hour. First, convert time to seconds: t = 1 hour × 60 min/hour × 60 s/min = 3600 s Now, calculate the charge: Q = I × t Q = 40,000 A × 3600 s Q = 144,000,000 C Step 2: Determine the number of moles of electrons (n_e) transferred. Using Faraday's constant (F = 96,500 C/mol e⁻): n_e = (Q)/(F) n_e = 144,000,000 C96,500 C/mol e⁻ n_e ≈ 1492.228 mol e⁻ Step 3: Write the half-reaction for aluminum deposition and find the mole ratio. Aluminum is produced from Al^3+ ions, which gain electrons to form solid aluminum: Al^3+ + 3e^- Al From this reaction, 3 moles of electrons are required to produce 1 mole of aluminum. Step 4: Calculate the moles of aluminum (n_Al) produced. n_Al = (n_e)/(3) n_Al = 1492.228 mol e⁻3 mol e⁻/mol Al n_Al ≈ 497.409 mol Al Step 5: Calculate the mass of aluminum (m_Al) produced. The molar mass of aluminum (Al) is 27 g/mol. m_Al = n_Al × M_Al m_Al = 497.409 mol × 27 g/mol m_Al ≈ 13430.043 g Step 6: Convert the mass to kilograms. m_Al = 13430.043 g1000 g/kg m_Al ≈ 13.43 kg The mass of aluminum produced is 13.4 kg. Send me the next one 📸