The combustion of liquid ethanol (C₂H₅OH) produces carbon dioxide and water. After 4.62 mL of ethanol (density = 0.789 g/mL) is allowed to burn in the presence of 15.55 g of oxygen gas, 3.72 mL of water (density = 1.00 g/mL) is collected. Determine the percent yield for the reaction. (Hint: Write a balanced equation for the combustion of ethanol.)

검증된 단계별 안내

Write the balanced chemical equation for the combustion of ethanol (C₂H₅OH). The balanced equation is: C₂H₅OH(l) + 3O₂(g) ightarrow 2CO₂(g) + 3H₂O(l).

Calculate the mass of ethanol used by multiplying the volume of ethanol by its density. Use the formula: mass = volume imes density.

Convert the mass of ethanol to moles using its molar mass (46.07 g/mol for ethanol). Use the formula: moles = mass / molar mass.

Calculate the theoretical yield of water in grams. Use the stoichiometry of the balanced equation to find the moles of water produced per mole of ethanol, then convert these moles of water to grams using the molar mass of water (18.02 g/mol).

Calculate the percent yield by comparing the actual yield (mass of water collected) to the theoretical yield. Use the formula: percent yield = (actual yield / theoretical yield) imes 100.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

주요 개념

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

Combustion Reaction

A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, producing heat and light. In the case of ethanol, the balanced equation for its combustion is C2H5OH + 3O2 → 2CO2 + 3H2O. Understanding this reaction is crucial for determining the stoichiometry involved and the theoretical yield of products.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine how much product can be formed from a given amount of reactant. In this question, stoichiometry is used to find the theoretical yield of water produced from the combustion of ethanol, which is essential for calculating percent yield.

Percent Yield

Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield. It is expressed as a percentage: (actual yield / theoretical yield) × 100%. In this scenario, calculating the percent yield of water produced from the combustion of ethanol will help assess how effectively the reaction occurred.

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교과서 질문

Many home barbeques are fueled with propane gas (C₃H₈). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 37.8 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)

교과서 질문

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 10.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

교과서 질문

The reaction of NH₃ and O2 forms NO and water. The NO can be used to convert P₄ to P₄O₆, forming N₂ in the process. The P₄O₆ can be treated with water to form H₃PO₃, which forms PH₃ and H₃PO₄ when heated. Find the mass of PH₃ that forms from the reaction of 1.00 g of NH₃.

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교과서 질문

A liquid fuel mixture contains 30.35% hexane (C₆H₁₄), 15.85% heptane (C₇H₁₆), and the rest octane (C₈H₁₈). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

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교과서 질문

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO₂ from Fe₂O₃ and CO. Determine the mass of Fe₂O₃ required to form 910 kg of iron. Determine the amount of CO₂ that forms in this process.

Aspirin can be made in the laboratory by reacting acetic anhydride (C₄H₆O₃) with salicylic acid (C₇H₆O₃) to form aspirin (C₉H₈O₄) and acetic acid (C₂H₄O₂). The balanced equation is: C₄H₆O₃ + C₇H₆O₃ → C₉H₈O₄ + C₂H₄O₂ In a laboratory synthesis, a student begins with 6.00 mL of acetic anhydride (density= 1.08 g/ mL) and 2.50 g of salicylic acid. Once the reaction is complete, the student collects 1.82 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield forthe reaction.