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Questions and Answers
Which statement best describes an ideal gas according to the Kinetic Molecular Theory?
Which statement best describes an ideal gas according to the Kinetic Molecular Theory?
Real gases behave ideally at low temperatures and high pressures.
Real gases behave ideally at low temperatures and high pressures.
False
What is the universal gas constant in liter·atm/(K·mol)?
What is the universal gas constant in liter·atm/(K·mol)?
0.0821
According to Boyle's Law, when the volume of a gas increases, its _____ decreases.
According to Boyle's Law, when the volume of a gas increases, its _____ decreases.
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Match each term with the correct description:
Match each term with the correct description:
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Which of the following scenarios illustrates gas diffusion?
Which of the following scenarios illustrates gas diffusion?
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At STP, the temperature of a gas is measured in Celsius.
At STP, the temperature of a gas is measured in Celsius.
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What effect does increasing temperature have on the average kinetic energy of gas particles?
What effect does increasing temperature have on the average kinetic energy of gas particles?
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According to Charles' Law, what happens to the volume of a gas when the temperature increases, assuming constant mass and pressure?
According to Charles' Law, what happens to the volume of a gas when the temperature increases, assuming constant mass and pressure?
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Gay-Lussac's Law states that the pressure and volume of a gas are directly related.
Gay-Lussac's Law states that the pressure and volume of a gas are directly related.
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What is the relationship described by the Combined Gas Law?
What is the relationship described by the Combined Gas Law?
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According to Gay-Lussac's Law, P/T = _____ (where k is a constant).
According to Gay-Lussac's Law, P/T = _____ (where k is a constant).
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Match the gas law with its application:
Match the gas law with its application:
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What is the value of the universal gas constant (R) in the Ideal Gas Law?
What is the value of the universal gas constant (R) in the Ideal Gas Law?
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Avogadro's Principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
Avogadro's Principle states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
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What happens to the volume of a gas when pressure is increased, according to Boyle's Law?
What happens to the volume of a gas when pressure is increased, according to Boyle's Law?
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What is the ideal gas constant R in the ideal gas law PV = nRT?
What is the ideal gas constant R in the ideal gas law PV = nRT?
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Dalton's Law states that the total pressure of a mixture of gases is equal to the product of the individual gas pressures.
Dalton's Law states that the total pressure of a mixture of gases is equal to the product of the individual gas pressures.
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What volume of CO2 is produced from 5.25 g of CaCO3 at 103 kPa and 25ºC?
What volume of CO2 is produced from 5.25 g of CaCO3 at 103 kPa and 25ºC?
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The temperature must be converted to ______ for gas law calculations.
The temperature must be converted to ______ for gas law calculations.
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Match the gas parameters to their corresponding values in the first problem:
Match the gas parameters to their corresponding values in the first problem:
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How many grams of Al2O3 are formed from 15.0 L of O2 at 97.3 kPa and 21°C?
How many grams of Al2O3 are formed from 15.0 L of O2 at 97.3 kPa and 21°C?
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To find the partial pressure of a gas, you subtract the water vapor pressure from the total pressure.
To find the partial pressure of a gas, you subtract the water vapor pressure from the total pressure.
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What is the partial pressure of dry hydrogen gas if the atmospheric pressure is 94.4 kPa and the water vapor pressure is 2.72 kPa?
What is the partial pressure of dry hydrogen gas if the atmospheric pressure is 94.4 kPa and the water vapor pressure is 2.72 kPa?
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Study Notes
Chapter 11 - Gases
- Gases expand to fill any container.
- Gases are fluids (like liquids).
- Gases have very low densities.
- Gases can be compressed.
- Gases undergo diffusion and effusion.
I. Physical Properties (of gases)
-
Kinetic Molecular Theory (ideal gas):
- Particles have no volume.
- Particles have elastic collisions.
- Particles are in constant, random, straight-line motion.
- Particles do not attract or repel each other.
- Average kinetic energy is directly related to Kelvin temperature.
-
Real Gases:
- Particles have their own volume.
- Particles attract each other.
- Gas behavior is most ideal:
- At low pressure.
- At high temperatures.
- Nonpolar atoms/molecules.
II. Temperature
- Always use absolute temperature (Kelvin) when working with gases.
- °C = 5/9 (°F - 32)
- K = °C + 273
III. Pressure
- Pressure = force/area
- Which shoes create the most pressure? (This question relates to the concept of pressure on different areas, not the actual shoes.)
-
Barometer: Measures atmospheric pressure
- Mercury Barometer
- Aneroid Barometer
-
Key Units at Sea Level:
- 101.325 kPa (kilopascal)
- 1 atm
- 760 mm Hg
- 760 torr
- 14.7 psi
IV. STP (Standard Temperature & Pressure)
- 0°C or 273 K
- 1 atm or 101.325 kPa
V. Gas Laws
-
Boyle's Law:
- Pressure and volume are inversely related (at constant mass and temperature)
- PV = k
-
Charles' Law:
- Volume and absolute temperature are directly related (at constant mass and pressure)
- V/T = k
-
Gay-Lussac's Law:
- Pressure and absolute temperature are directly related (at constant mass and volume)
- P/T = k
-
Combined Gas Law:
- P₁V₁/T₁ = P₂V₂/T₂ (or P₁V₁T₂ = P₂V₂T₁)
VI. Ideal Gas Law
-
PV = nRT
-
R=0.0821 L⋅atm/mol⋅K or 8.315 dm³⋅kPa/mol⋅K (Universal Gas Constant)
-
Note: n = moles, P = pressure, V = volume, T = temperature, and R = the Ideal Gas Law constant
VII. Gas Stoichiometry
- Moles to Liters of a Gas
- STP: Use 22.4 L/mol.
- Non-STP: Use the Ideal Gas Law.
- Non-STP Problems
- Given liters of gas: Start with Ideal Gas Law.
- Looking for liters of gas: Start with stoichiometry conversion.
VIII. Dalton's Law
- The total pressure of a mixture of gases equals the sum of the partial pressures of the individual gases.
- Ptotal = P1 + P2 + ...
IX. Graham's Law
- Diffusion: Spreading of gas molecules until evenly distributed.
- Effusion: Passing of gas molecules through a tiny opening.
- Speed of diffusion/effusion
- Kinetic energy is determined by the temperature of the gas.
- At the same temp & KE, heavier molecules move more slowly.
- Rate of diffusion is inversely related to the square root of its molar mass
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Description
Explore the fascinating properties of gases in this quiz based on Chapter 11. Learn about the Kinetic Molecular Theory, the behavior of real gases, and the relationship between temperature and pressure. Test your knowledge on key concepts and definitions related to gases.
