Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter5: Gases
Section: Chapter Questions
Problem 5.108PAE
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Question
![**Problem Statement:**
36. How many *grams* of gaseous boron trifluoride, BF₃, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm?
**Answer Box:**
[ ] g BF₃
**Explanation:**
To solve this problem, you would typically use the Ideal Gas Law, which is given by:
\[ PV = nRT \]
Where:
- \( P \) is the pressure (in atm)
- \( V \) is the volume (in liters)
- \( n \) 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)
To find the mass in grams, calculate \( n \) using the above equation and then convert moles to grams using the molar mass of boron trifluoride (BF₃).
**Steps:**
1. Substitute the given values into the Ideal Gas Law to find \( n \).
2. Calculate the molar mass of BF₃.
3. Multiply the number of moles by the molar mass to get the mass in grams.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8512a4d6-a9a9-457e-80d0-a059d4b0c49a%2Fedabc0e1-0a68-4c9f-ab5e-4574bb4f27ab%2F6sieihy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
36. How many *grams* of gaseous boron trifluoride, BF₃, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm?
**Answer Box:**
[ ] g BF₃
**Explanation:**
To solve this problem, you would typically use the Ideal Gas Law, which is given by:
\[ PV = nRT \]
Where:
- \( P \) is the pressure (in atm)
- \( V \) is the volume (in liters)
- \( n \) 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)
To find the mass in grams, calculate \( n \) using the above equation and then convert moles to grams using the molar mass of boron trifluoride (BF₃).
**Steps:**
1. Substitute the given values into the Ideal Gas Law to find \( n \).
2. Calculate the molar mass of BF₃.
3. Multiply the number of moles by the molar mass to get the mass in grams.
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