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Each container with varying volume has 1.0 mole of oxygen gas at 30.0 will pressure be the lowest? C. In which container a. b. C. d.

Each container with varying volume has 1.0 mole of oxygen gas at 30.0 will pressure be the lowest? C. In which container a. b. C. d.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Educational Resource - Understanding Tire Explosions and Gas Behavior in a Closed Vessel #### Tire Explosions During Summer **Question 6:** Records show that the incident of tire explosions is high during the summer season. Which of the following gives the best explanation for this observation? Choices: a. There are more travelers during the summer vacation. b. High temperatures during the summer season cause the air inside the tire to expand. c. Vehicles' tires are not well maintained. d. There is too much air inside the tire. **Explanation**: The most accurate explanation is option (b). High temperatures during the summer season cause the air inside the tire to expand. When the air inside a tire heats up, it expands, increasing the pressure inside the tire, which can lead to tire explosions. #### Behavior of Gas in a Closed Vessel **Question 7:** Which is most likely to happen when a closed vessel filled with gas is shaken for 2 minutes? Choices: a. The temperature inside the vessel increases. b. The pressure inside the vessel increases. c. The temperature and pressure inside the vessel increase. d. Both the temperature and pressure inside the vessel increase. **Explanation**: The most appropriate outcome is option (b). Shaking a closed vessel filled with gas typically increases the pressure inside the vessel due to the increased kinetic energy of the gas molecules, leading to more frequent and forceful collisions with the vessel walls. ### Summary and Key Concepts: 1. **Tire Explosions in Hot Weather**: In hot weather, the temperature-related expansion of air within tires can increase the internal pressure, sometimes resulting in tire blowouts. 2. **Gas Behavior in Closed Vessels**: Shaking a closed vessel with gas predominantly increases the pressure inside due to heightened molecular collisions. Understanding these fundamental principles helps in practical applications such as vehicle maintenance and handling pressurized gas containers safely.
Transcribed Image Text:### Educational Resource - Understanding Tire Explosions and Gas Behavior in a Closed Vessel #### Tire Explosions During Summer **Question 6:** Records show that the incident of tire explosions is high during the summer season. Which of the following gives the best explanation for this observation? Choices: a. There are more travelers during the summer vacation. b. High temperatures during the summer season cause the air inside the tire to expand. c. Vehicles' tires are not well maintained. d. There is too much air inside the tire. **Explanation**: The most accurate explanation is option (b). High temperatures during the summer season cause the air inside the tire to expand. When the air inside a tire heats up, it expands, increasing the pressure inside the tire, which can lead to tire explosions. #### Behavior of Gas in a Closed Vessel **Question 7:** Which is most likely to happen when a closed vessel filled with gas is shaken for 2 minutes? Choices: a. The temperature inside the vessel increases. b. The pressure inside the vessel increases. c. The temperature and pressure inside the vessel increase. d. Both the temperature and pressure inside the vessel increase. **Explanation**: The most appropriate outcome is option (b). Shaking a closed vessel filled with gas typically increases the pressure inside the vessel due to the increased kinetic energy of the gas molecules, leading to more frequent and forceful collisions with the vessel walls. ### Summary and Key Concepts: 1. **Tire Explosions in Hot Weather**: In hot weather, the temperature-related expansion of air within tires can increase the internal pressure, sometimes resulting in tire blowouts. 2. **Gas Behavior in Closed Vessels**: Shaking a closed vessel with gas predominantly increases the pressure inside due to heightened molecular collisions. Understanding these fundamental principles helps in practical applications such as vehicle maintenance and handling pressurized gas containers safely.
**Question 3: Gas Pressure in Varying Volumes** Consider four containers, each holding 1.0 mole of oxygen gas at a temperature of 30.0 °C. These containers differ only in their volumes. The goal is to determine which container will have the lowest gas pressure. **Diagrams of Containers:** - **Container a:** This container is the smallest. - **Container b:** This container is larger than container a. - **Container c:** This container is larger than container b. - **Container d:** This container is the largest. **Key Concept:** The pressure of a gas in a container is determined by the Ideal Gas Law, which is expressed as: \[ PV = nRT \] Where: - \( P \) is the pressure, - \( V \) is the volume, - \( n \) is the amount of gas in moles, - \( R \) is the ideal gas constant, - \( T \) is the temperature in Kelvin. Given that \( n \), \( R \), and \( T \) are constant for all containers, the pressure \( P \) will be inversely proportional to the volume \( V \) (`P ∝ 1/V`). **Analysis:** Since gas pressure decreases as the container volume increases, the container with the largest volume will have the lowest pressure. **Answer:** Select **container d** for the lowest pressure, as it has the largest volume.
Transcribed Image Text:**Question 3: Gas Pressure in Varying Volumes** Consider four containers, each holding 1.0 mole of oxygen gas at a temperature of 30.0 °C. These containers differ only in their volumes. The goal is to determine which container will have the lowest gas pressure. **Diagrams of Containers:** - **Container a:** This container is the smallest. - **Container b:** This container is larger than container a. - **Container c:** This container is larger than container b. - **Container d:** This container is the largest. **Key Concept:** The pressure of a gas in a container is determined by the Ideal Gas Law, which is expressed as: \[ PV = nRT \] Where: - \( P \) is the pressure, - \( V \) is the volume, - \( n \) is the amount of gas in moles, - \( R \) is the ideal gas constant, - \( T \) is the temperature in Kelvin. Given that \( n \), \( R \), and \( T \) are constant for all containers, the pressure \( P \) will be inversely proportional to the volume \( V \) (`P ∝ 1/V`). **Analysis:** Since gas pressure decreases as the container volume increases, the container with the largest volume will have the lowest pressure. **Answer:** Select **container d** for the lowest pressure, as it has the largest volume.
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