AP Physics 2 Flashcards: Kinetic Theory Of Temperature And Pressure

What this deck covers

This deck focuses on Kinetic Theory Of Temperature And Pressure, giving you a quick way to review the definitions, rules, and examples that matter most for AP Physics 2.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What assumption about particle size is made in the kinetic theory of gases?

Answer: Particles are point-like with negligible volume. Ideal gas approximation assumption.

Flashcard 2: Identify the constant in Charles's Law.

Answer: Pressure. Volume and temperature vary at fixed pressure.

Flashcard 3: Which law relates volume and amount of gas at constant temperature?

Answer: Avogadro's Law. Volume proportional to gas quantity.

Flashcard 4: What is the molar volume of an ideal gas at STP?

Answer: $22.4 \text{ L/mol}$. Standard molar volume for ideal gases.

Flashcard 5: Which gas law states that $PV/T$ is a constant for a given amount of gas?

Answer: Combined Gas Law. Combines Boyle's, Charles's, and Gay-Lussac's laws.

Flashcard 6: What does Charles's Law state about temperature and volume?

Answer: Volume is directly proportional to temperature. At constant pressure, $\frac{V}{T} = k$.

Flashcard 7: How does kinetic theory describe the energy distribution among particles?

Answer: Energy is distributed according to a Maxwell-Boltzmann distribution. Statistical description of particle energies.

Flashcard 8: Which variable remains constant in Boyle's Law?

Answer: Temperature. Pressure and volume vary inversely.

Flashcard 9: Which gas law states that $PV/T$ is a constant for a given amount of gas?

Answer: Combined Gas Law. Combines Boyle's, Charles's, and Gay-Lussac's laws.

Flashcard 10: State the equation for Dalton's Law.

Answer: $P_{total} = P_1 + P_2 + \text{...}$. Additive pressures in gas mixtures.

Flashcard 11: Calculate the pressure when a gas expands to double its volume at constant temperature.

Answer: Pressure is halved. Application of Boyle's Law calculation.

Flashcard 12: What is the relationship between temperature and kinetic energy?

Answer: Kinetic energy is directly proportional to temperature. Temperature measures average kinetic energy.

Flashcard 13: How does kinetic theory describe the energy distribution among particles?

Answer: Energy is distributed according to a Maxwell-Boltzmann distribution. Statistical description of particle energies.

Flashcard 14: What is the assumption about particle collisions in kinetic theory?

Answer: Collisions are elastic. No energy lost in collisions.

Flashcard 15: Which variable remains constant in Boyle's Law?

Answer: Temperature. Pressure and volume vary inversely.

Flashcard 16: What happens to particle speed as temperature increases?

Answer: Particle speed increases. Higher temperature means more kinetic energy.

Flashcard 17: What is the definition of thermal equilibrium in kinetic theory?

Answer: No net energy transfer between objects. Same temperature means equal average energies.

Flashcard 18: What is the value of the universal gas constant $R$?

Answer: $8.314 \frac{J}{mol \times K}$. Standard value for gas calculations.

Flashcard 19: Define the term 'pressure' in the context of gases.

Answer: Force exerted by gas particles per unit area. Molecular collisions create force.

Flashcard 20: What assumption about particle size is made in the kinetic theory of gases?

Answer: Particles are point-like with negligible volume. Ideal gas approximation assumption.

Flashcard 21: State the equation for Dalton's Law.

Answer: $P_{total} = P_1 + P_2 + \text{...}$. Additive pressures in gas mixtures.

Flashcard 22: What is the significance of the gas constant $R$?

Answer: It relates energy units in the ideal gas law. Proportionality constant in gas equations.

Flashcard 23: State the relationship between temperature and pressure in Gay-Lussac's Law.

Answer: Pressure is directly proportional to temperature. At constant volume, $\frac{P}{T} = k$.

Flashcard 24: What is the formula for kinetic energy of a gas particle?

Answer: $KE = \frac{1}{2}mv^2$. Energy from mass and velocity squared.

Flashcard 25: What is the effect of temperature on the speed of sound in a gas?

Answer: Speed of sound increases with temperature. Sound speed depends on molecular motion.

Flashcard 26: What is the assumption about particle collisions in kinetic theory?

Answer: Collisions are elastic. No energy lost in collisions.

Flashcard 27: Identify the unit of temperature used in gas law calculations.

Answer: Kelvin (K). Absolute temperature scale required.

Flashcard 28: What is the formula for the number of moles $n$ in terms of mass $m$?

Answer: $n = \frac{m}{M}$. Mass divided by molar mass gives moles.

Flashcard 29: State the relationship between pressure and volume in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, $PV = k$.

Flashcard 30: What happens to pressure if volume is halved at constant temperature?

Answer: Pressure doubles. Inverse relationship from Boyle's Law.

Flashcard 31: State the relationship between pressure and volume in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, $PV = k$.

Flashcard 32: What is the formula for calculating pressure?

Answer: $P = \frac{F}{A}$. Force divided by contact area.

Flashcard 33: Define the term 'molar volume' at STP.

Answer: The volume occupied by one mole of gas at STP. Standard volume at 0°C and 1 atm.

Flashcard 34: What does Dalton's Law of Partial Pressures state?

Answer: Total pressure is the sum of partial pressures. Each gas contributes independently.

Flashcard 35: Calculate the pressure when a gas expands to double its volume at constant temperature.

Answer: Pressure is halved. Application of Boyle's Law calculation.

Flashcard 36: If the pressure of a gas is tripled, what happens to its volume at constant temperature?

Answer: Volume is reduced to one-third. Inverse pressure-volume relationship applied.

Flashcard 37: What is the molar volume of an ideal gas at STP?

Answer: $22.4 \text{ L/mol}$. Standard molar volume for ideal gases.

Flashcard 38: What is the value of the universal gas constant $R$?

Answer: $8.314 \frac{J}{mol \times K}$. Standard value for gas calculations.

Flashcard 39: What causes gas pressure on a container's walls?

Answer: Collisions of gas particles with the walls. Momentum transfer from particle impacts.

Flashcard 40: What is the equation for the ideal gas law?

Answer: $PV = nRT$. Combines pressure, volume, moles, and temperature.

Flashcard 41: Identify the unit of temperature used in gas law calculations.

Answer: Kelvin (K). Absolute temperature scale required.

Flashcard 42: What happens to pressure if volume is halved at constant temperature?

Answer: Pressure doubles. Inverse relationship from Boyle's Law.

Flashcard 43: What does the kinetic theory of gases state about particle motion?

Answer: Particles are in constant random motion. Foundation of kinetic molecular theory.

Flashcard 44: What causes gas pressure on a container's walls?

Answer: Collisions of gas particles with the walls. Momentum transfer from particle impacts.

Flashcard 45: What is the equation for calculating density from pressure and temperature?

Answer: $\rho = \frac{P \times M}{R \times T}$. Derived from ideal gas law rearrangement.

Flashcard 46: What does Charles's Law state about temperature and volume?

Answer: Volume is directly proportional to temperature. At constant pressure, $\frac{V}{T} = k$.

Flashcard 47: If the pressure of a gas is tripled, what happens to its volume at constant temperature?

Answer: Volume is reduced to one-third. Inverse pressure-volume relationship applied.

Flashcard 48: What happens to particle speed as temperature increases?

Answer: Particle speed increases. Higher temperature means more kinetic energy.

Flashcard 49: State the relationship between temperature and pressure in Gay-Lussac's Law.

Answer: Pressure is directly proportional to temperature. At constant volume, $\frac{P}{T} = k$.

Flashcard 50: Define the term 'pressure' in the context of gases.

Answer: Force exerted by gas particles per unit area. Molecular collisions create force.

Flashcard 51: What is the formula for converting Celsius to Kelvin?

Answer: $K = C + 273.15$. Converts to absolute temperature scale.

Flashcard 52: What is the equation for the ideal gas law?

Answer: $PV = nRT$. Combines pressure, volume, moles, and temperature.

Flashcard 53: What is the definition of thermal equilibrium in kinetic theory?

Answer: No net energy transfer between objects. Same temperature means equal average energies.

Flashcard 54: What is the relationship between temperature and kinetic energy?

Answer: Kinetic energy is directly proportional to temperature. Temperature measures average kinetic energy.

Flashcard 55: What is the formula for calculating pressure?

Answer: $P = \frac{F}{A}$. Force divided by contact area.

Flashcard 56: What is the effect of temperature on the speed of sound in a gas?

Answer: Speed of sound increases with temperature. Sound speed depends on molecular motion.

Flashcard 57: Identify the constant in Charles's Law.

Answer: Pressure. Volume and temperature vary at fixed pressure.

Flashcard 58: What is the SI unit for pressure?

Answer: Pascal (Pa). Newton per square meter.

Flashcard 59: What is the effect of lowering temperature on the kinetic energy of gas particles?

Answer: Kinetic energy decreases. Temperature directly affects molecular energy.

Flashcard 60: What is Avogadro's Law in terms of volume and moles?

Answer: Volume is directly proportional to moles. Equal volumes contain equal moles at STP.

Flashcard 61: What is the formula for converting Celsius to Kelvin?

Answer: $K = C + 273.15$. Converts to absolute temperature scale.

Flashcard 62: What is Avogadro's Law in terms of volume and moles?

Answer: Volume is directly proportional to moles. Equal volumes contain equal moles at STP.

Flashcard 63: What is the equation for calculating density from pressure and temperature?

Answer: $\rho = \frac{P \times M}{R \times T}$. Derived from ideal gas law rearrangement.

Flashcard 64: What does Dalton's Law of Partial Pressures state?

Answer: Total pressure is the sum of partial pressures. Each gas contributes independently.

Flashcard 65: Which law relates volume and amount of gas at constant temperature?

Answer: Avogadro's Law. Volume proportional to gas quantity.

Flashcard 66: What does the kinetic theory of gases state about particle motion?

Answer: Particles are in constant random motion. Foundation of kinetic molecular theory.

Flashcard 67: What is the SI unit for pressure?

Answer: Pascal (Pa). Newton per square meter.

Flashcard 68: What is the formula for the number of moles $n$ in terms of mass $m$?

Answer: $n = \frac{m}{M}$. Mass divided by molar mass gives moles.

Flashcard 69: What is the formula for kinetic energy of a gas particle?

Answer: $KE = \frac{1}{2}mv^2$. Energy from mass and velocity squared.

Flashcard 70: What is the definition of absolute zero?

Answer: The temperature at which particle motion stops. Zero kinetic energy at -273.15°C.

Flashcard 71: Define the term 'molar volume' at STP.

Answer: The volume occupied by one mole of gas at STP. Standard volume at 0°C and 1 atm.

Flashcard 72: What is the significance of the gas constant $R$?

Answer: It relates energy units in the ideal gas law. Proportionality constant in gas equations.

Flashcard 73: What is the definition of absolute zero?

Answer: The temperature at which particle motion stops. Zero kinetic energy at -273.15°C.

Flashcard 74: What is the effect of lowering temperature on the kinetic energy of gas particles?

Answer: Kinetic energy decreases. Temperature directly affects molecular energy.