Solutions of sulfuric acid and lead(II) acetate react to form solid lead(II) sulfate and a solution of acetic acid. If 5.00 g of sulfuric acid and 5.00 g of lead(II) acetate are mixed, calculate the number of grams of lead(II) acetate present in the mixture after the reaction is complete.

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \( \text{H}_2\text{SO}_4 + \text{Pb(CH}_3\text{COO)}_2 \rightarrow \text{PbSO}_4 + 2\text{CH}_3\text{COOH} \).
2. Calculate the molar mass of sulfuric acid (\( \text{H}_2\text{SO}_4 \)) and lead(II) acetate (\( \text{Pb(CH}_3\text{COO)}_2 \)).
3. Determine the number of moles of sulfuric acid and lead(II) acetate using their respective masses and molar masses.
4. Identify the limiting reactant by comparing the mole ratio from the balanced equation to the moles calculated.
5. Calculate the amount of lead(II) acetate remaining after the reaction by using the stoichiometry of the reaction and the initial moles of the limiting reactant.

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of each substance is consumed or produced. Understanding stoichiometry is essential for solving problems related to the amounts of reactants and products in a reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the amounts of products and remaining reactants after the reaction. In this case, it will help determine how much lead(II) acetate remains after the reaction with sulfuric acid.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is used to convert between the mass of a substance and the number of moles, which is essential for stoichiometric calculations. Knowing the molar masses of sulfuric acid and lead(II) acetate allows for the determination of how many moles are present in the given masses, facilitating the stoichiometric analysis of the reaction.