A cylinder of oxygen gas contains 31.9 g 02. If the volume of the cylinder is 1.71 L, what is the pressure of the O2 if the gas temperature is 23°C? Pressure atm
A cylinder of oxygen gas contains 31.9 g 02. If the volume of the cylinder is 1.71 L, what is the pressure of the O2 if the gas temperature is 23°C? Pressure atm
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:**
A cylinder of oxygen gas contains 31.9 g of O₂. If the volume of the cylinder is 1.71 L, what is the pressure of the O₂ if the gas temperature is 23°C?
**Calculation Required:**
To find:
\[ \text{Pressure} = \underline{\hspace{20px}} \, \text{atm} \]
**Explanation:**
This problem involves the application of the ideal gas law to determine the pressure of a given mass of oxygen gas at a specified volume and temperature.
**The Ideal Gas Law:**
\[ PV = nRT \]
Where:
- \( P \) is the pressure in atm
- \( V \) is the volume in liters (L)
- \( n \) is the number of moles of the gas
- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) is the temperature in Kelvin
The steps required include:
1. Converting the temperature from Celsius to Kelvin.
2. Calculating the number of moles of O₂ from the given mass.
3. Substituting known values into the ideal gas law to solve for pressure.
**Variables Given:**
- Mass of O₂ = 31.9 g
- Volume \( V \) = 1.71 L
- Temperature \( T \) = 23°C
**Unknown:**
- Pressure \( P \) in atm
Note: The diagram or graph is not provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2F51b3a3c7-7712-447f-a122-8509cec2e45c%2Fbzn75vi_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
A cylinder of oxygen gas contains 31.9 g of O₂. If the volume of the cylinder is 1.71 L, what is the pressure of the O₂ if the gas temperature is 23°C?
**Calculation Required:**
To find:
\[ \text{Pressure} = \underline{\hspace{20px}} \, \text{atm} \]
**Explanation:**
This problem involves the application of the ideal gas law to determine the pressure of a given mass of oxygen gas at a specified volume and temperature.
**The Ideal Gas Law:**
\[ PV = nRT \]
Where:
- \( P \) is the pressure in atm
- \( V \) is the volume in liters (L)
- \( n \) is the number of moles of the gas
- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) is the temperature in Kelvin
The steps required include:
1. Converting the temperature from Celsius to Kelvin.
2. Calculating the number of moles of O₂ from the given mass.
3. Substituting known values into the ideal gas law to solve for pressure.
**Variables Given:**
- Mass of O₂ = 31.9 g
- Volume \( V \) = 1.71 L
- Temperature \( T \) = 23°C
**Unknown:**
- Pressure \( P \) in atm
Note: The diagram or graph is not provided.
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