What mass of lead sulfate is formed in a lead–acid storage battery when 1.00 g of Pb undergoes oxidation?

Verified step by step guidance

1. Identify the chemical reaction involved in the oxidation of lead (Pb) in a lead-acid battery. The reaction is: Pb + HSO4- → PbSO4 + H+ + 2e-.
2. Calculate the molar mass of lead (Pb) using the periodic table. This will be used to convert the mass of Pb to moles.
3. Using stoichiometry, determine the moles of lead sulfate (PbSO4) produced per mole of lead (Pb) oxidized. From the balanced chemical equation, the mole ratio of Pb to PbSO4 is 1:1.
4. Calculate the molar mass of lead sulfate (PbSO4) using the periodic table. This will be used to convert moles of PbSO4 to mass.
5. Multiply the moles of PbSO4 by its molar mass to find the mass of lead sulfate formed.

Key Concepts

Oxidation-Reduction Reactions

Oxidation-reduction (redox) reactions involve the transfer of electrons between substances. In this context, lead (Pb) is oxidized, meaning it loses electrons, which is essential for understanding how lead sulfate (PbSO4) is formed in the battery. Recognizing the oxidation states of the elements involved helps in determining the products of the reaction.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. To find the mass of lead sulfate produced, one must use the molar ratios from the balanced equation of the reaction between lead and sulfuric acid, which is crucial for converting grams of Pb to grams of PbSO4.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. It is necessary to calculate the mass of lead sulfate formed from the mass of lead oxidized. Knowing the molar masses of lead (Pb) and lead sulfate (PbSO4) allows for accurate conversions between the mass of reactants and products in the reaction.