During a period of discharge of a lead–acid battery, 402 g of Pb from the anode is converted into PbSO₄(s). (b) How many coulombs of electrical charge are transferred from Pb to PbO₂?

Verified step by step guidance

1. Identify the chemical reaction occurring in the lead-acid battery during discharge. The anode reaction is: \[ \text{Pb} + \text{SO}_4^{2-} \rightarrow \text{PbSO}_4 + 2e^- \].
2. Determine the moles of Pb involved in the reaction. Use the molar mass of Pb (207.2 g/mol) to convert the given mass of Pb (402 g) to moles: \[ \text{moles of Pb} = \frac{402 \text{ g}}{207.2 \text{ g/mol}} \].
3. Calculate the total number of moles of electrons transferred. Since each mole of Pb produces 2 moles of electrons, multiply the moles of Pb by 2.
4. Use Faraday's constant to convert moles of electrons to coulombs. Faraday's constant is approximately 96485 C/mol. Multiply the moles of electrons by Faraday's constant to find the total charge in coulombs.
5. Summarize the process: The total charge transferred is the product of the moles of electrons and Faraday's constant, which gives the number of coulombs of electrical charge transferred from Pb to PbO2.