Starting with 39.5 moles of O₂ in a bottle, calculate the volume of O₂ the bottle could deliver to a climber at an altitude where the temperature is -38.0°C and the atmospheric pressure is 0.282 atm. L
Starting with 39.5 moles of O₂ in a bottle, calculate the volume of O₂ the bottle could deliver to a climber at an altitude where the temperature is -38.0°C and the atmospheric pressure is 0.282 atm. L
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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![### Problem Statement
**Objective:**
Calculate the volume of oxygen gas (O₂) that can be delivered to a climber, given the following conditions:
- Amount of O₂: 39.5 moles
- Temperature: -38.0°C
- Atmospheric Pressure: 0.282 atm
### Instructions
1. **Utilize the Ideal Gas Law**:
\[ PV = nRT \]
Where:
\( P \) = Pressure (atm)
\( V \) = Volume (L)
\( n \) = Number of moles
\( R \) = Ideal gas constant (0.0821 L·atm/mol·K)
\( T \) = Temperature (K)
2. **Convert Temperature**:
Convert the given temperature from Celsius to Kelvin:
\[ T(K) = T(°C) + 273.15 \]
3. **Solve for Volume (V)**:
Rearrange the Ideal Gas Law to solve for volume \( V \):
\[ V = \frac{{nRT}}{P} \]
4. **Insert the Given Values**:
Substitute the provided values into the equation to calculate the volume.
Ensure the units are consistent and calculations are accurate. Use resources such as the periodic table or provided hints if needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Feac4d301-280e-44a9-9b77-05aa59bdadf8%2Fc1acbce1-eb81-41f3-823e-8a5c3ddc4602%2Fm93mb7b_processed.png&w=3840&q=75)
Transcribed Image Text:### Problem Statement
**Objective:**
Calculate the volume of oxygen gas (O₂) that can be delivered to a climber, given the following conditions:
- Amount of O₂: 39.5 moles
- Temperature: -38.0°C
- Atmospheric Pressure: 0.282 atm
### Instructions
1. **Utilize the Ideal Gas Law**:
\[ PV = nRT \]
Where:
\( P \) = Pressure (atm)
\( V \) = Volume (L)
\( n \) = Number of moles
\( R \) = Ideal gas constant (0.0821 L·atm/mol·K)
\( T \) = Temperature (K)
2. **Convert Temperature**:
Convert the given temperature from Celsius to Kelvin:
\[ T(K) = T(°C) + 273.15 \]
3. **Solve for Volume (V)**:
Rearrange the Ideal Gas Law to solve for volume \( V \):
\[ V = \frac{{nRT}}{P} \]
4. **Insert the Given Values**:
Substitute the provided values into the equation to calculate the volume.
Ensure the units are consistent and calculations are accurate. Use resources such as the periodic table or provided hints if needed.
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