Ch.10 - Gases: Their Properties & Behavior

McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경

McMurry 8th Edition

Ch.10 - Gases: Their Properties & Behavior

문제 142

10장, 문제 142

A 5.00-L vessel contains 25.0 g of PCl3 and 3.00 g of O2 at 15 °C. The vessel is heated to 200.0 °C, and the contents react to give POCl3. What is the final pressure in the vessel, assuming that the reaction goes to completion and that all reactants and products are in the gas phase?

검증된 단계별 안내

Identify the balanced chemical equation for the reaction: \( \text{PCl}_3 + \text{O}_2 \rightarrow \text{POCl}_3 \).

Calculate the number of moles of \( \text{PCl}_3 \) and \( \text{O}_2 \) using their respective molar masses.

Determine the limiting reactant by comparing the mole ratio from the balanced equation with the calculated moles of reactants.

Use the stoichiometry of the reaction to find the moles of \( \text{POCl}_3 \) produced, which will be equal to the moles of the limiting reactant.

Apply the ideal gas law \( PV = nRT \) to calculate the final pressure, using the total moles of gas (\( \text{POCl}_3 \) produced) and the final temperature of 200.0 °C converted to Kelvin.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

14m

주요 개념

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

Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the final pressure in the vessel after the reaction, as it allows us to determine how changes in temperature and the number of moles affect the pressure of the gas mixture.

Stoichiometry of the Reaction

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. Understanding the stoichiometry of the reaction between PCl3 and O2 to form POCl3 is crucial for determining the moles of each substance before and after the reaction, which directly influences the final pressure.

Gas Phase Reactions

Gas phase reactions occur when reactants and products are in the gaseous state, allowing for the application of gas laws. In this scenario, recognizing that all substances are gases and that the reaction goes to completion is vital for accurately calculating the final pressure, as it affects the total number of moles present in the vessel.

관련 실천

교과서 질문

When 10.0 g of a mixture of Ca(ClO₃)₂ and Ca(ClO)₂ is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O₂(g) and CaCl₂(s). The final pressure inside the vessel is 1.00 atm. (a) Write balanced equations for the decomposition reactions.

328

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교과서 질문

When 10.0 g of a mixture of Ca1ClO322 and Ca1ClO22 is heated to 700 °C in a 10.0-L vessel, both compounds decompose, forming O21g2 and CaCl21s2. The final pressure inside the vessel is 1.00 atm. (b) What is the mass of each compound in the original mixture?

596

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교과서 질문

A mixture of CS21g2 and excess O21g2 is placed in a 10.0-L reaction vessel at 100.0 °C and a pressure of 3.00 atm. A spark causes the CS2 to ignite, burning it completely, according to the equation CS21g2 + 3 O21g2¡CO21g2 + 2 SO21g2 After reaction, the temperature returns to 100.0 °C, and the mixture of product gases (CO2, SO2, and unreacted O2) is found to have a pressure of 2.40 atm. What is the partial pressure of each gas in the product mixture?

416

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교과서 질문

A steel container with a volume of 500.0 mL is evacuated, and 25.0 g of CaCO₃ is added. The container and contents are then heated to 1500 K, causing the CaCO₃ to decompose completely, according to the equation CaCO₃(s) → CaO(s) + CO₂(g). (b) Now make a more accurate calculation of the pressure inside the container. Take into account the volume of solid CaO (density = 3.34 g/mL) in the container, and use the van der Waals equation to calculate the pressure. The van der Waals constants for CO₂(g) are a = 3.59 (L²-atm)/mol² and b = 0.0427 L/mol.

507

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교과서 질문

A steel container with a volume of 500.0 mL is evacuated, and 25.0 g of CaCO₃ is added. The container and contents are then heated to 1500 K, causing the CaCO₃ to decompose completely, according to the equation CaCO₃(s) → CaO(s) + CO₂(g). (a) Using the ideal gas law and ignoring the volume of any solids remaining in the container, calculate the pressure inside the container at 1500 K.

433

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