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
Step 1: Write the half-reaction for the liberation of oxygen gas. During the electrolysis of dilute sodium chloride, oxygen gas is produced at the anode from the oxidation of water. 2H_2O(l) O_2(g) + 4H^+(aq) + 4e^- Step 2: Determine the moles of electrons required per mole of oxygen. From the balanced half-reaction, 4 moles of electrons are required to produce 1 mole of oxygen gas. Step 3: Calculate the total moles of electrons needed for 0.125 mole of oxygen. Moles of electrons = 0.125 mol O_2 × 4 mol e^-1 mol O_2 = 0.500 mol e^- Step 4: Calculate the quantity of electricity in coulombs. Using Faraday's constant (F = 96500 C/mol e^-): Quantity of electricity = Moles of electrons × F Quantity of electricity = 0.500 mol e^- × 96500 C/mol e^- Quantity of electricity = 48250 C The quantity of electricity required is 48250 C. Send me the next one 📸