Podcast
Questions and Answers
When carbon dioxide sublimates, transitioning from a solid to a gaseous state, which property undergoes a change?
When carbon dioxide sublimates, transitioning from a solid to a gaseous state, which property undergoes a change?
- Particle arrangement (correct)
- Molecular polarity
- Gram-formula mass
- Bond type
A container holds particles that are widely spaced and move independently of each other. According to the kinetic molecular theory, which state of matter is most likely represented in the container?
A container holds particles that are widely spaced and move independently of each other. According to the kinetic molecular theory, which state of matter is most likely represented in the container?
- Gas (correct)
- Plasma
- Liquid
- Solid
Four different gas samples are at the temperatures 12°C, 27°C, 267 K, and 298 K. Which gas sample exhibits the highest average kinetic energy?
Four different gas samples are at the temperatures 12°C, 27°C, 267 K, and 298 K. Which gas sample exhibits the highest average kinetic energy?
- 267 K
- 27°C
- 298 K (correct)
- 12°C
Which statement best describes the motion of ideal gas molecules, according to the kinetic molecular theory?
Which statement best describes the motion of ideal gas molecules, according to the kinetic molecular theory?
Which of the following statements is a fundamental assumption about the particles in an ideal gas?
Which of the following statements is a fundamental assumption about the particles in an ideal gas?
Under which conditions does a real gas behave most like an ideal gas?
Under which conditions does a real gas behave most like an ideal gas?
Two sealed containers of equal volume are compared. Container A holds 2.0 grams of hydrogen gas, and container B holds 2.0 grams of oxygen gas, both at the same temperature. Which statement correctly compares the pressures in the two containers?
Two sealed containers of equal volume are compared. Container A holds 2.0 grams of hydrogen gas, and container B holds 2.0 grams of oxygen gas, both at the same temperature. Which statement correctly compares the pressures in the two containers?
A rigid container holds a gas at a certain pressure and temperature. If the temperature of the gas is doubled in Kelvin, what happens to the pressure of the gas, assuming the volume and number of moles remain constant?
A rigid container holds a gas at a certain pressure and temperature. If the temperature of the gas is doubled in Kelvin, what happens to the pressure of the gas, assuming the volume and number of moles remain constant?
Under which conditions is a gas most likely to deviate significantly from ideal behavior?
Under which conditions is a gas most likely to deviate significantly from ideal behavior?
Which of the following gases will diffuse most slowly, assuming all are at the same temperature and pressure?
Which of the following gases will diffuse most slowly, assuming all are at the same temperature and pressure?
A gas is at standard temperature and pressure (STP). Which of the following conditions correctly describes STP?
A gas is at standard temperature and pressure (STP). Which of the following conditions correctly describes STP?
A rigid container holds a sample of gas. If the temperature of the gas is increased, what happens to the frequency of collisions between the gas particles and the walls of the container?
A rigid container holds a sample of gas. If the temperature of the gas is increased, what happens to the frequency of collisions between the gas particles and the walls of the container?
A gas occupies a volume of 10.0 L at a pressure of 2.0 atm. If the pressure is decreased to 1.0 atm while keeping the temperature constant, what will be the new volume of the gas?
A gas occupies a volume of 10.0 L at a pressure of 2.0 atm. If the pressure is decreased to 1.0 atm while keeping the temperature constant, what will be the new volume of the gas?
Which graph best represents the relationship between pressure and volume of a gas at constant temperature?
Which graph best represents the relationship between pressure and volume of a gas at constant temperature?
A container of gas at 200 K is heated until it reaches 600 K, while the pressure remains constant. If the initial volume of the gas was 6.00 L, what is the final volume?
A container of gas at 200 K is heated until it reaches 600 K, while the pressure remains constant. If the initial volume of the gas was 6.00 L, what is the final volume?
A gas sample is heated in a closed, rigid container. Which of the following describes the effect of increasing the temperature on the pressure of the gas?
A gas sample is heated in a closed, rigid container. Which of the following describes the effect of increasing the temperature on the pressure of the gas?
A gas occupies a certain volume at 200 K. To double the volume while keeping the pressure constant, what should the new temperature be?
A gas occupies a certain volume at 200 K. To double the volume while keeping the pressure constant, what should the new temperature be?
A container holds a mixture of gases: nitrogen, oxygen, and carbon dioxide. If the total pressure in the container is 760 mm Hg, and the partial pressures of nitrogen and oxygen are 300 mm Hg and 200 mm Hg respectively, what is the partial pressure of carbon dioxide?
A container holds a mixture of gases: nitrogen, oxygen, and carbon dioxide. If the total pressure in the container is 760 mm Hg, and the partial pressures of nitrogen and oxygen are 300 mm Hg and 200 mm Hg respectively, what is the partial pressure of carbon dioxide?
Flashcards
CO₂ Sublimation Change
CO₂ Sublimation Change
Change only in the particle arrangement. Solids have fixed structures, gases have widely spaced, random particles.
Identifying a Gas
Identifying a Gas
Look for particles that are far apart and moving randomly.
Highest Kinetic Energy
Highest Kinetic Energy
Kinetic energy increases with temperature (in Kelvin).
Ideal Gas Motion
Ideal Gas Motion
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Ideal Gas Volume
Ideal Gas Volume
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Ideal Gas Conditions
Ideal Gas Conditions
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Gas Deviation from Ideal
Gas Deviation from Ideal
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Gas Diffusion Rate
Gas Diffusion Rate
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Standard Temp & Pressure (STP)
Standard Temp & Pressure (STP)
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Temp Increase effect on gas
Temp Increase effect on gas
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Pressure Decrease Effect on Volume
Pressure Decrease Effect on Volume
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Boyle's Law Formula
Boyle's Law Formula
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Charles's Law
Charles's Law
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Gay-Lussac's Law
Gay-Lussac's Law
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Dalton's Law
Dalton's Law
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Partial Pressure Calculation
Partial Pressure Calculation
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Study Notes
Change in CO₂ State (Solid to Gas)
- When CO₂(s) sublimates, only the particle arrangement changes.
- The arrangement changes from a fixed, ordered structure in solids to widely spaced, randomly moving particles in gases.
- Bond type, molecular polarity, and gram-formula mass remain unchanged.
Identifying a Gas in a Particle Diagram
- Gases are identified by widely spaced, randomly moving particles.
- Solids have closely packed particles in a fixed arrangement.
- Liquids have particles that are close but move freely.
Highest Kinetic Energy
- Kinetic energy (KE) is directly proportional to temperature in Kelvin.
- To convert Celsius to Kelvin, add 273.
- 298 K is the highest temperature among the options, indicating the highest kinetic energy.
Kinetic Molecular Theory: Ideal Gas Motion
- Ideal gas particles move in random, straight-line motion until they collide.
- There are no significant attraction forces between ideal gas particles.
Properties of an Ideal Gas
- In ideal gases, individual gas molecules are considered to have no volume.
- This is in comparison to the total volume of the gas.
- Real gases deviate from this assumption at high pressures and low temperatures.
Conditions for Ideal Gas Behavior
- Gases behave ideally at high temperatures and low pressures.
- High temperature causes gas particles to move fast, reducing intermolecular attraction.
- Low pressure causes gas particles to be far apart, reducing interactions.
Gas Least Likely to Follow Ideal Gas Laws
- Larger gas molecules (like Xe) have stronger intermolecular forces.
- Stronger intermolecular forces cause deviation from ideal behavior.
- Lighter gases like He and Ne behave more ideally.
Slowest Diffusing Gas
- According to Graham’s Law of Diffusion, lighter gases diffuse faster.
- The gas with the greatest molecular mass diffuses the slowest.
Standard Temperature and Pressure (STP)
- STP is 1 atm (760 mm Hg or 101.3 kPa) and 273 K (0°C).
Effect of Increasing Temperature on a Rigid Gas Sample
- Higher temperature causes faster-moving particles.
- Faster-moving particles causes more frequent collisions.
Pressure-Volume Relationship at Constant Temperature
- If pressure decreases, volume increases proportionally, according to Boyle’s Law.
- Boyle's Law Formula: P₁V₁ = P₂V₂
Pressure-Volume Graph
- Boyle’s Law states pressure and volume have an inverse relationship.
- The graph representing this relationship is a curved downward slope.
Mathematical Relationship of Pressure and Volume
- Boyle’s Law formula states that pressure times volume remains constant: P × V = k
Volume-Temperature Relationship
- Volume is directly proportional to temperature (in Kelvin), as described by Charles’s Law.
- Charles's Law Formula: V₁ / T₁ = V₂ / T₂
Volume vs. Temperature Graph at Constant Pressure
- Charles’s Law shows a direct proportionality between temperature and volume.
- The graph is a straight, upward-sloping line.
Volume Change When Temperature Increases
- Use Charles’s Law: V₁ / T₁ = V₂ / T₂
- If you have:
- V₁ = 6.00 L
- T₁ = 200 K
- T₂ = 600 K
- Then V₂ = 6.00 × (600/200) = 12.0 L
Effect of Increasing Temperature on Pressure (Constant Volume)
- Higher temperature results in higher pressure, according to Gay-Lussac’s Law.
- Gay-Lussac's Law Formula: P₁ / T₁ = P₂ / T₂
Pressure-Temperature Graph for an Ideal Gas
- Gay-Lussac’s Law shows a direct relationship between pressure and temperature.
- The graph is a straight, upward-sloping line.
Doubling Volume While Keeping Pressure Constant
- According to Charles’s Law, if temperature doubles in Kelvin, volume also doubles.
- Example doubling: 200 K to 400 K
Volume of CH₄ Gas at a New Temperature
- Charles’s Law applies: V₂ = V₁ × (T₂/T₁)
Changing Volume Based on Pressure & Temperature
- The Combined Gas Law should be used.
- The Combined Gas Law is: (P₁V₁) / T₁ = (P₂V₂) / T₂
Finding New Pressure
- Use the Combined Gas Law and solve for P₂.
Partial Pressure Calculations
- Use Dalton’s Law: Ptotal = PA + PB + PC
- Solve for unknown pressures.
Partial Pressure of Hydrogen
- Partial pressure equals total pressure multiplied by hydrogen’s mole fraction.
- Formula: P(H₂) = (3 / (4+3+1)) × P(total)
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Description
Covers the change in CO₂ state from solid to gas (sublimation). Identifies gases in particle diagrams and explains kinetic energy relative to Kelvin temperature. Describes ideal gas motion according to kinetic molecular theory.
