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:**
If 53.5 mol of an ideal gas occupies 79.5 L at 311 K, what is the pressure of the gas?
**Solution:**
pressure: [Answer box] atm
**Explanation:**
To solve this problem, you can use the Ideal Gas Law:
\[ PV = nRT \]
Where:
- \( P \) is the pressure of the gas.
- \( V \) is the volume of the gas (79.5 L).
- \( n \) is the number of moles (53.5 mol).
- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K).
- \( T \) is the temperature in Kelvin (311 K).
Rearrange the equation to solve for \( P \):
\[ P = \frac{nRT}{V} \]
Plug in the values:
\[ P = \frac{53.5 \times 0.0821 \times 311}{79.5} \]
Calculate the pressure to find the answer in atm.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbfab9a7f-9ea4-456a-bb57-050ea1ff4d68%2F3a121f6e-a0be-4d51-b439-d5e285338a68%2Fvf651rh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
If 53.5 mol of an ideal gas occupies 79.5 L at 311 K, what is the pressure of the gas?
**Solution:**
pressure: [Answer box] atm
**Explanation:**
To solve this problem, you can use the Ideal Gas Law:
\[ PV = nRT \]
Where:
- \( P \) is the pressure of the gas.
- \( V \) is the volume of the gas (79.5 L).
- \( n \) is the number of moles (53.5 mol).
- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K).
- \( T \) is the temperature in Kelvin (311 K).
Rearrange the equation to solve for \( P \):
\[ P = \frac{nRT}{V} \]
Plug in the values:
\[ P = \frac{53.5 \times 0.0821 \times 311}{79.5} \]
Calculate the pressure to find the answer in atm.
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