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Questions and Answers
A gas occupies 5.0 L at a pressure of 2.0 atm. If the volume is increased to 10.0 L while keeping the temperature constant, what will be the new pressure?
A gas occupies 5.0 L at a pressure of 2.0 atm. If the volume is increased to 10.0 L while keeping the temperature constant, what will be the new pressure?
- 0.5 atm
- 2.0 atm
- 4.0 atm
- 1.0 atm (correct)
A container of gas has a volume of 6.0 L at standard pressure (1 atm). If the pressure is changed to 3 atm, what is the new volume, assuming constant temperature?
A container of gas has a volume of 6.0 L at standard pressure (1 atm). If the pressure is changed to 3 atm, what is the new volume, assuming constant temperature?
- 9.0 L
- 2.0 L (correct)
- 18.0 L
- 3.0 L
A gas occupies 22.4 L at a pressure of 760 mmHg. What volume will it occupy if the pressure is increased to 1520 mmHg while maintaining a constant temperature?
A gas occupies 22.4 L at a pressure of 760 mmHg. What volume will it occupy if the pressure is increased to 1520 mmHg while maintaining a constant temperature?
- 33.6 L
- 44.8 L
- 11.2 L (correct)
- 22.4 L
A balloon contains 10 L of air at 27 degrees C and 1 atm pressure. If the pressure is doubled, and the temperature is kept constant, what is the new volume of the balloon?
A balloon contains 10 L of air at 27 degrees C and 1 atm pressure. If the pressure is doubled, and the temperature is kept constant, what is the new volume of the balloon?
A gas occupies a volume of 10.0 L at standard pressure. If the pressure is tripled, what will the new volume be, assuming the temperature remains constant?
A gas occupies a volume of 10.0 L at standard pressure. If the pressure is tripled, what will the new volume be, assuming the temperature remains constant?
A gas has a volume of 250 mL at 2 atm. If the pressure is reduced to 0.5 atm, what is the new volume if the temperature is held constant?
A gas has a volume of 250 mL at 2 atm. If the pressure is reduced to 0.5 atm, what is the new volume if the temperature is held constant?
A sample of gas occupies 2.0 L at 1.0 atm. If the pressure is increased to 4.0 atm while keeping the temperature constant, what is the new volume?
A sample of gas occupies 2.0 L at 1.0 atm. If the pressure is increased to 4.0 atm while keeping the temperature constant, what is the new volume?
A gas occupies 500 mL at a pressure of 700 torr. What volume will it occupy at standard atmospheric pressure, ≈760 torr, assuming constant temperature?
A gas occupies 500 mL at a pressure of 700 torr. What volume will it occupy at standard atmospheric pressure, ≈760 torr, assuming constant temperature?
Flashcards
Boyle's Law
Boyle's Law
Boyle's Law states that the volume of a gas is inversely proportional to its pressure, assuming constant temperature and amount of gas.
Boyle's Law Formula
Boyle's Law Formula
P1V1 = P2V2, where P is pressure and V is volume. The '1' and '2' subscripts denote initial and final conditions.
Standard Pressure
Standard Pressure
Standard pressure is defined as 1 atmosphere (atm), which is equal to 760 mmHg or 101.3 kPa.
Consistent Units
Consistent Units
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Inverse Relationship
Inverse Relationship
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Solving for Volume/Pressure
Solving for Volume/Pressure
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Halving the Pressure
Halving the Pressure
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Pressure conversions
Pressure conversions
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Study Notes
Boyle's Law
- Boyle's Law describes the relationship between the pressure and volume of a gas
- The formula for Boyle's Law is P₁V₁ = P₂V₂
- P represents pressure
- V represents volume
- As volume increases, pressure decreases (V ↑ P↓)
Worked Example
- A gas occupies 12.3 liters at a pressure of 40.0 mmHg
- Volume is calculated when the pressure is increased to 60.0 mmHg as follows:
- P₁ = 40.0 mmHg
- V₁ = 12.3 liters
- P₂ = 60.0 mmHg
- V₂ = ?
- Using Boyle's Law: P₁V₁ = P₂V₂
- Substituting the values: (40.0 mmHg) (12.3 liters) = (60.0 mmHg) (x)
- Solving for x: x = 8.20 L
Conversions
- 1 atm (atmospheric pressure, "atmosphere," or standard pressure) = 760 mmHg
- 1 torr = 1 mmHg
Practice Problems
- Problem #2: Calculate the volume of a gas initially at 25.0 °C occupying 3.60 liters at 1.00 atm, when the pressure becomes 2.50 atm
- Problem #3: Calculate the pressure needed to compress a gas from 400.0 cubic feet to fit into a 3.00 cubic foot tank at standard pressure
- Problem #4: Calculate the volume of a gas initially occupying 1.56 L at 1.00 atm, when the pressure increases to 3.00 atm
- Problem #5: Determine the pressure of a gas initially occupying 11.2 liters at 0.860 atm, when the volume changes to 15.0 L
- Problem #6: Calculate the volume of 500.0 mL of gas collected at 745.0 mmHg at standard pressure
- Problem #7: Convert 350.0 mL of gas at 740.0 mmHg to its new volume at standard pressure
- Problem #8: Convert 338 L of gas at 63.0 atm to its new volume at standard pressure
- Problem #9: Convert 273.15 mL of gas at 166.0 kPa to its new volume at standard pressure
- Problem #10: Convert 77.0 L of gas at 18.0 mmHg to its new volume at standard pressure
- Problem #11: Determine whether the volume increase or decrease when pressure on a gas increases
- Problem #12: Find out how the volume changes when the pressure on a gas is halved
- Problem #13: Calculate the volume of a gas initially occupying 4.31 liters at 0.755 atm, when the pressure increases to 1.25 atm
- Problem #14: Calculate the volume of a gas initially at 600.0 mL at 8.00 atm, when the pressure decreases to 2.00 atm
- Problem #15: Calculate the volume of a gas initially at 400.0 mL under 800.0 torr, when the pressure increases to 1000.0 torr
Bonus Problem
- A balloon is designed to inflate to a max volume of 2.5 liters
- The balloon is filled with 2.0 liters of helium at sea level (101.3 kPa)
- Determine if the balloon will burst as it rises to an altitude where the boiling temperature of water is 88 degrees Celsius
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Description
Explanation of Boyle's Law, which defines the relationship between the pressure and volume of a gas at constant temperature and mass. Includes a worked example and practice questions. Also contains some useful conversions.
