A reaction at 34.0 °C evolves 436. mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits. volume: |
A reaction at 34.0 °C evolves 436. mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits. volume: |
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 reaction at 34.0 °C evolves 436. mmol of boron trifluoride gas.
Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits.
### Input Field:
- **Volume:** A text input box is provided for the user to enter the calculated volume in liters (L).
### Additional Interface Details:
- A checkbox labeled "x10" is available, possibly to indicate if scientific notation should be used.
- There are three buttons:
- A checkmark (✔) button, likely to submit or confirm the entered answer.
- A circular arrow (↻) button, probably to reset or clear the input.
- A question mark (?) button, which might provide help or hints for solving the problem.
### Analytical Approach:
To solve the problem, utilize the Ideal Gas Law equation:
\[ PV = nRT \]
Where:
- \( P \) is the pressure (in atm)
- \( V \) is the volume (in liters)
- \( n \) is the number of moles (in this case, mmol of boron trifluoride gas converted to moles)
- \( R \) is the ideal gas constant \( (0.0821 \, \text{L·atm·K}^{-1}\text{·mol}^{-1}) \)
- \( T \) is the temperature in Kelvin (K)
#### Conversion:
1. Convert mmol to moles:
\[ 436 \, \text{mmol} = 0.436 \, \text{mol} \]
2. Convert °C to K:
\[ T = 34.0 + 273.15 = 307.15 \, \text{K} \]
Now, substitute the values into the Ideal Gas Law equation and solve for \( V \):
\[ V = \frac{nRT}{P} \]
Substitute:
\[ V = \frac{(0.436 \, \text{mol}) (0.0821 \, \text{L·atm·K}^{-1}\text{·mol}^{-1}) (307.15 \, \text{K})}{1 \, \text{atm}} \]
Calculate to find \( V \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F47bace65-e928-444e-9199-b108470afcd9%2F6a27ce31-5101-4937-b116-c90efcf4b8f8%2Fd33e569_processed.png&w=3840&q=75)
Transcribed Image Text:### Problem Statement:
A reaction at 34.0 °C evolves 436. mmol of boron trifluoride gas.
Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits.
### Input Field:
- **Volume:** A text input box is provided for the user to enter the calculated volume in liters (L).
### Additional Interface Details:
- A checkbox labeled "x10" is available, possibly to indicate if scientific notation should be used.
- There are three buttons:
- A checkmark (✔) button, likely to submit or confirm the entered answer.
- A circular arrow (↻) button, probably to reset or clear the input.
- A question mark (?) button, which might provide help or hints for solving the problem.
### Analytical Approach:
To solve the problem, utilize the Ideal Gas Law equation:
\[ PV = nRT \]
Where:
- \( P \) is the pressure (in atm)
- \( V \) is the volume (in liters)
- \( n \) is the number of moles (in this case, mmol of boron trifluoride gas converted to moles)
- \( R \) is the ideal gas constant \( (0.0821 \, \text{L·atm·K}^{-1}\text{·mol}^{-1}) \)
- \( T \) is the temperature in Kelvin (K)
#### Conversion:
1. Convert mmol to moles:
\[ 436 \, \text{mmol} = 0.436 \, \text{mol} \]
2. Convert °C to K:
\[ T = 34.0 + 273.15 = 307.15 \, \text{K} \]
Now, substitute the values into the Ideal Gas Law equation and solve for \( V \):
\[ V = \frac{nRT}{P} \]
Substitute:
\[ V = \frac{(0.436 \, \text{mol}) (0.0821 \, \text{L·atm·K}^{-1}\text{·mol}^{-1}) (307.15 \, \text{K})}{1 \, \text{atm}} \]
Calculate to find \( V \).
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