Lead ions can be precipitated from solution with KCl according to the reaction: Pb2+ (aq) + 2 KCl(aq) → PbCl2(s) + 2 K+ (aq). When 28.5 g KCl is added to a solution containing 25.7 g Pb2+, a PbCl2 precipitate forms. The precipitate is filtered, dried, and found to have a mass of 29.4 g. Determine the percent yield for the reaction. Determine the theoretical yield of PbCl2. Determine the limiting reactant.

Verified step by step guidance

Step 1: Calculate the moles of KCl and Pb^{2+}.

Step 2: Use the balanced chemical equation to determine the stoichiometric ratio and identify the limiting reactant.

Step 3: Calculate the theoretical yield of PbCl_2 based on the limiting reactant.

Step 4: Use the actual yield of PbCl_2 to calculate the percent yield.

Step 5: Summarize the findings: theoretical yield, limiting reactant, and percent yield.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the quantities of substances involved in a reaction. In this case, stoichiometry will help identify how much PbCl2 can theoretically be produced from the given amounts of Pb2+ and KCl.

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. To find the limiting reactant, one must compare the mole ratios of the reactants based on the balanced equation. In this scenario, identifying the limiting reactant is crucial for calculating the theoretical yield of PbCl2.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to its theoretical yield. It is expressed as a percentage and provides insight into how much of the expected product was actually obtained. In this problem, calculating the percent yield will involve using the mass of the dried PbCl2 precipitate and the theoretical yield derived from stoichiometric calculations.

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