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Ch.4 - Chemical Reactions and Chemical Quantities
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 6th EditionCh.4 - Chemical Reactions and Chemical Quantities문제 56
4장, 문제 56

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O2(g) → 2 MgO(s) When 13.1 g of Mg reacts with 13.6 g O2, 12.4 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

검증된 단계별 안내
1
Step 1: Calculate the moles of Mg and O2 using their molar masses. For Mg, use the molar mass of 24.31 g/mol, and for O2, use 32.00 g/mol.
Step 2: Use the balanced chemical equation to determine the mole ratio between Mg and O2. The equation shows a 2:1 ratio, meaning 2 moles of Mg react with 1 mole of O2.
Step 3: Determine the limiting reactant by comparing the mole ratio from Step 2 with the actual moles calculated in Step 1. The reactant that produces the least amount of product is the limiting reactant.
Step 4: Calculate the theoretical yield of MgO using the moles of the limiting reactant and the stoichiometry of the reaction. Convert the moles of MgO to grams using its molar mass (40.31 g/mol).
Step 5: Calculate the percent yield using the formula: \( \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \). Use the actual yield of 12.4 g MgO and the theoretical yield from Step 4.

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주요 개념

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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 identify the limiting reactant, one must compare the mole ratios of the reactants based on the balanced chemical equation. The reactant that produces the lesser amount of product is the limiting reactant.
추천 영상:
가이드 코스
01:30
Limiting Reagent Concept

Theoretical Yield

The theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, as calculated from the balanced chemical equation. It assumes complete conversion of the limiting reactant into product without any losses. Theoretical yield is typically expressed in grams or moles and serves as a benchmark for evaluating the efficiency of a reaction.
추천 영상:
가이드 코스
03:09
Percent Yield in Reactions

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product obtained from the experiment to the theoretical yield. It is expressed as a percentage using the formula: (actual yield / theoretical yield) × 100%. A high percent yield indicates a successful reaction with minimal losses, while a low percent yield suggests inefficiencies or side reactions.
추천 영상:
가이드 코스
03:09
Percent Yield in Reactions
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교과서 질문

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s) + 6 Cl2( g) → 4 PCl3(l) A reaction mixture initially contains 91.38 g P4 and 262.6 g Cl2. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 45.10 g Fe2O3 and 29.56 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

교과서 질문

For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F2( g) → TiF4(s) c. 0.233 g Ti, 0.288 g F2

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교과서 질문

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 177.4 kg of SiO2 reacts with 100.1 kg of carbon to produce 71.2 kg of silicon. Determine the percent yield for the reaction.

교과서 질문

Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2 NH3(aq) + CO2(aq) → CH4N2O(aq) + H2O(l) In an industrial synthesis of urea, a chemist combines 149.4 kg of ammonia with 231.1 kg of carbon dioxide and obtains 172.3 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.