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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![**Question:** What is the mass (in grams) of 6.00 L of propane vapor (C₃H₈) at STP?
**Explanation:**
To find the mass of 6.00 L of propane vapor at STP (Standard Temperature and Pressure), we need to use the ideal gas law and the molar volume of a gas at STP.
1. **Molar Volume at STP:** At STP, 1 mole of any ideal gas occupies 22.4 L.
2. **Molar Mass of Propane (C₃H₈):** Calculate the molar mass using atomic masses:
- Carbon (C): 12.01 g/mol
- Hydrogen (H): 1.01 g/mol
- Molar mass of C₃H₈ = (3 × 12.01) + (8 × 1.01) = 44.09 g/mol
3. **Volume-Mole Relationship:**
\[
\text{Moles of propane} = \frac{6.00 \, \text{L}}{22.4 \, \text{L/mol}}
\]
4. **Calculate Mass:**
- Mass = Moles × Molar Mass
- Use the moles obtained from the volume-mole relationship to find the mass.
This calculation provides the mass of 6.00 L of propane vapor at STP.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe5e5e412-f9ab-493e-8169-7197b3039da3%2F8a5eca3a-9b3c-487c-b01e-a3ecc52267f2%2Fy2wxlcy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:** What is the mass (in grams) of 6.00 L of propane vapor (C₃H₈) at STP?
**Explanation:**
To find the mass of 6.00 L of propane vapor at STP (Standard Temperature and Pressure), we need to use the ideal gas law and the molar volume of a gas at STP.
1. **Molar Volume at STP:** At STP, 1 mole of any ideal gas occupies 22.4 L.
2. **Molar Mass of Propane (C₃H₈):** Calculate the molar mass using atomic masses:
- Carbon (C): 12.01 g/mol
- Hydrogen (H): 1.01 g/mol
- Molar mass of C₃H₈ = (3 × 12.01) + (8 × 1.01) = 44.09 g/mol
3. **Volume-Mole Relationship:**
\[
\text{Moles of propane} = \frac{6.00 \, \text{L}}{22.4 \, \text{L/mol}}
\]
4. **Calculate Mass:**
- Mass = Moles × Molar Mass
- Use the moles obtained from the volume-mole relationship to find the mass.
This calculation provides the mass of 6.00 L of propane vapor at STP.
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