Calculate the molecular weight of Freon-12, if 122.70 liters of its vapor at 200.00°C and 790.00 mm Hg has a mass of 397.00 g. Show your work.
Calculate the molecular weight of Freon-12, if 122.70 liters of its vapor at 200.00°C and 790.00 mm Hg has a mass of 397.00 g. Show your work.
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: Calculation of Molecular Weight**
Calculate the molecular weight of Freon-12, if 122.70 liters of its vapor at 200.00°C and 790.00 mm Hg has a mass of 397.00 g. **Show your work.**
**Solution Approach**
To find the molecular weight of Freon-12, we can use the Ideal Gas Law, which is given by:
\[ PV = nRT \]
Where:
- \( P \) = Pressure in atm
- \( V \) = Volume in liters
- \( n \) = Number of moles
- \( R \) = Ideal gas constant = 0.0821 L·atm/(mol·K)
- \( T \) = Temperature in Kelvin
**Steps:**
1. Convert the given pressure from mm Hg to atm:
\[ P = \frac{790.00 \, \text{mm Hg}}{760.00 \, \text{mm Hg/atm}} \]
2. Convert the given temperature from Celsius to Kelvin:
\[ T = 200.00 + 273.15 \, \text{K} \]
3. Rearrange the Ideal Gas Law to solve for \( n \) (number of moles):
\[ n = \frac{PV}{RT} \]
4. Use the mass of Freon-12 to find the molecular weight:
\[ \text{Molecular Weight} = \frac{\text{Mass}}{n} \]
Plug in the values and calculate accordingly.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6d32c2dd-6c61-4daf-8dd5-59d048b4a395%2F17bc00d1-1d4b-4091-86f4-83409b205e32%2Fru2pf9j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem: Calculation of Molecular Weight**
Calculate the molecular weight of Freon-12, if 122.70 liters of its vapor at 200.00°C and 790.00 mm Hg has a mass of 397.00 g. **Show your work.**
**Solution Approach**
To find the molecular weight of Freon-12, we can use the Ideal Gas Law, which is given by:
\[ PV = nRT \]
Where:
- \( P \) = Pressure in atm
- \( V \) = Volume in liters
- \( n \) = Number of moles
- \( R \) = Ideal gas constant = 0.0821 L·atm/(mol·K)
- \( T \) = Temperature in Kelvin
**Steps:**
1. Convert the given pressure from mm Hg to atm:
\[ P = \frac{790.00 \, \text{mm Hg}}{760.00 \, \text{mm Hg/atm}} \]
2. Convert the given temperature from Celsius to Kelvin:
\[ T = 200.00 + 273.15 \, \text{K} \]
3. Rearrange the Ideal Gas Law to solve for \( n \) (number of moles):
\[ n = \frac{PV}{RT} \]
4. Use the mass of Freon-12 to find the molecular weight:
\[ \text{Molecular Weight} = \frac{\text{Mass}}{n} \]
Plug in the values and calculate accordingly.
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