An ideal gas is contained in a cylinder with a volume of 5.0x102 mL at a temperature of 30.0°C and a pressure of 710. torr. The gas is then compressed to a volume of 25 mL, and the temperature is raised to 820.0°C. What is the new pressure of the gas?
An ideal gas is contained in a cylinder with a volume of 5.0x102 mL at a temperature of 30.0°C and a pressure of 710. torr. The gas is then compressed to a volume of 25 mL, and the temperature is raised to 820.0°C. What is the new pressure of the gas?
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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### Gas Laws and Chemical Reactions in Safety Devices
**Problem 3: Ideal Gas Law Application**
An ideal gas is contained in a cylinder with a volume of \(5.0 \times 10^2 \, \text{mL}\) at a temperature of \(30.0^\circ \text{C}\) and a pressure of \(710 \, \text{torr}\). The gas is then compressed to a volume of \(25 \, \text{mL}\), and the temperature is raised to \(820.0^\circ \text{C}\). What is the new pressure of the gas?
**Problem 4: Chemical Reaction in Airbags**
Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN₃) to decompose explosively according to the following reaction:
\[ 2 \text{NaN}_3(s) \rightarrow 2 \text{Na}(s) + 3 \text{N}_2(g) \]
What mass of \(\text{NaN}_3(s)\) must be reacted to inflate an air bag to \(70.0 \, \text{L}\) at \(25^\circ \text{C}\) and \(0.995 \, \text{atm}\)?
### Explanation of Concepts
- **Ideal Gas Law**: This problem requires applying the combined gas law to find the new pressure after a change in volume and temperature.
- **Chemical Reaction in Airbags**: Sodium azide is used in airbags to rapidly produce nitrogen gas and inflate the bag during a collision.
The above chemical reaction equation shows the decomposition of sodium azide, crucial for the inflation step.
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Transcribed Image Text:Here's a transcription and explanation suitable for an educational website:
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### Gas Laws and Chemical Reactions in Safety Devices
**Problem 3: Ideal Gas Law Application**
An ideal gas is contained in a cylinder with a volume of \(5.0 \times 10^2 \, \text{mL}\) at a temperature of \(30.0^\circ \text{C}\) and a pressure of \(710 \, \text{torr}\). The gas is then compressed to a volume of \(25 \, \text{mL}\), and the temperature is raised to \(820.0^\circ \text{C}\). What is the new pressure of the gas?
**Problem 4: Chemical Reaction in Airbags**
Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN₃) to decompose explosively according to the following reaction:
\[ 2 \text{NaN}_3(s) \rightarrow 2 \text{Na}(s) + 3 \text{N}_2(g) \]
What mass of \(\text{NaN}_3(s)\) must be reacted to inflate an air bag to \(70.0 \, \text{L}\) at \(25^\circ \text{C}\) and \(0.995 \, \text{atm}\)?
### Explanation of Concepts
- **Ideal Gas Law**: This problem requires applying the combined gas law to find the new pressure after a change in volume and temperature.
- **Chemical Reaction in Airbags**: Sodium azide is used in airbags to rapidly produce nitrogen gas and inflate the bag during a collision.
The above chemical reaction equation shows the decomposition of sodium azide, crucial for the inflation step.
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