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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.4 - Chemical Quantities & Aqueous Reactions문제 49
4장, 문제 49

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.

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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.

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

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.
추천 영상:
가이드 코스
01:30
Limiting Reagent Concept

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.
추천 영상:
가이드 코스
03:09
Percent Yield in Reactions
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