AP Physics 2 Flashcards: The Ideal Gas Law

What this deck covers

This deck focuses on The Ideal Gas Law, 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: How does the Ideal Gas Law change if $n$ is constant but $P$, $V$ change?

Answer: Boyle's Law. Special case where $PV =$ constant at fixed amount.

Flashcard 2: Convert temperature from Celsius to Kelvin for gas law calculations.

Answer: $K = °C + 273.15$. Converts to absolute scale required for gas laws.

Flashcard 3: Identify the units for $R$ when pressure is in Pascals.

Answer: Joules per mole Kelvin. Energy units appropriate for Pascal pressure measurements.

Flashcard 4: What happens to volume if both $P$ and $T$ double, while $n$ is constant?

Answer: Volume remains constant. Effects of pressure and temperature changes cancel out.

Flashcard 5: What units must pressure be in for the Ideal Gas Law when using $R = 0.0821$?

Answer: Atmospheres (atm). Required unit to match the gas constant $R$ value.

Flashcard 6: Identify the relationship between volume and temperature in the Ideal Gas Law.

Answer: Directly proportional. Both increase or decrease together (Charles's Law).

Flashcard 7: If $T$ doubles and $n$ and $V$ are constant, what happens to $P$?

Answer: Pressure doubles. Temperature is directly proportional to pressure.

Flashcard 8: What happens to volume when temperature increases at constant $P$ and $n$?

Answer: Volume increases. Higher kinetic energy causes gas to expand.

Flashcard 9: Identify the relationship between pressure and volume in the Ideal Gas Law.

Answer: Inversely proportional. When one increases, the other decreases (Boyle's Law).

Flashcard 10: Find the volume of 1 mole of gas at 1 atm and 273 K.

Answer: $V = 22.4$ L. Standard molar volume at STP conditions.

Flashcard 11: What is the ideal gas constant $R$ value in $J/(mol \times K)$?

Answer: $8.314 \text{ J}/(\text{mol} \times \text{K})$. Used when pressure is in Pascals and volume in cubic meters.

Flashcard 12: Calculate the volume if $P = 2$ atm, $n = 1$ mol, $T = 273$ K.

Answer: $V = 11.2$ L. Using $PV = nRT$: $V = \frac{(1)(0.0821)(273)}{2} = 11.2$ L.

Flashcard 13: Find the pressure of 2 moles of gas at 300 K in a 10 L container.

Answer: $P = 4.92$ atm. Using $PV = nRT$: $P = \frac{(2)(0.0821)(300)}{10} = 4.92$ atm.

Flashcard 14: Identify the relationship between volume and temperature in the Ideal Gas Law.

Answer: Directly proportional. Both increase or decrease together (Charles's Law).

Flashcard 15: What is the ideal gas constant $R$ value in $J/(mol \times K)$?

Answer: $8.314 \text{ J}/(\text{mol} \times \text{K})$. Used when pressure is in Pascals and volume in cubic meters.

Flashcard 16: Convert 100°C to Kelvin for use in gas law calculations.

Answer: $373.15$ K. Add 273.15 to Celsius temperature.

Flashcard 17: What happens to pressure when volume decreases at constant $n$ and $T$?

Answer: Pressure increases. Gas molecules compress into smaller space, creating higher pressure.

Flashcard 18: Calculate pressure when 0.5 mol of gas is at 350 K in a 5 L container.

Answer: $P = 2.87$ atm. Using $PV = nRT$: $P = \frac{(0.5)(0.0821)(350)}{5} = 2.87$ atm.

Flashcard 19: What happens to pressure when temperature decreases at constant $V$ and $n$?

Answer: Pressure decreases. Lower kinetic energy reduces molecular collisions with walls.

Flashcard 20: Find the number of moles for $P = 4$ atm, $V = 15$ L, $T = 300$ K.

Answer: $n = 2.44$ mol. Using $PV = nRT$: $n = \frac{(4)(15)}{(0.0821)(300)} = 2.44$ mol.

Flashcard 21: Find the temperature if $P = 3$ atm, $V = 10$ L, $n = 1$ mol.

Answer: $T = 366$ K. Using $PV = nRT$: $T = \frac{(3)(10)}{(1)(0.0821)} = 366$ K.

Flashcard 22: What does the variable $n$ represent in the Ideal Gas Law?

Answer: Number of moles of gas. Amount of substance measured in molecular units.

Flashcard 23: Determine $n$ for $P = 2$ atm, $V = 5$ L, $T = 298$ K.

Answer: $n = 0.41$ mol. Using $PV = nRT$: $n = \frac{(2)(5)}{(0.0821)(298)} = 0.41$ mol.

Flashcard 24: What is the value of the ideal gas constant $R$ in $L \times atm/(mol \times K)$?

Answer: $0.0821 \text{ L} \times \text{atm}/(\text{mol} \times \text{K})$. Standard value when using atm and L units.

Flashcard 25: What does the variable $V$ represent in the Ideal Gas Law?

Answer: Volume of the gas. Space occupied by the gas in three dimensions.

Flashcard 26: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. Relates pressure, volume, moles, and temperature for ideal gases.

Flashcard 27: What does the variable $n$ represent in the Ideal Gas Law?

Answer: Number of moles of gas. Amount of substance measured in molecular units.

Flashcard 28: What is the value of the ideal gas constant $R$ in $L \times atm/(mol \times K)$?

Answer: $0.0821 \text{ L} \times \text{atm}/(\text{mol} \times \text{K})$. Standard value when using atm and L units.

Flashcard 29: Identify the units for $R$ when using $8.314$ as the constant.

Answer: $J/(mol \times K)$. Energy per amount per temperature unit.

Flashcard 30: Determine $n$ for $P = 2$ atm, $V = 5$ L, $T = 298$ K.

Answer: $n = 0.41$ mol. Using $PV = nRT$: $n = \frac{(2)(5)}{(0.0821)(298)} = 0.41$ mol.

Flashcard 31: Identify the relationship between moles and volume in the Ideal Gas Law.

Answer: Directly proportional. More gas molecules occupy more space (Avogadro's Law).

Flashcard 32: Find the number of moles for $P = 4$ atm, $V = 15$ L, $T = 300$ K.

Answer: $n = 2.44$ mol. Using $PV = nRT$: $n = \frac{(4)(15)}{(0.0821)(300)} = 2.44$ mol.

Flashcard 33: What is the temperature if $P = 5$ atm, $V = 20$ L, $n = 2$ mol?

Answer: $T = 609$ K. Using $PV = nRT$: $T = \frac{(5)(20)}{(2)(0.0821)} = 609$ K.

Flashcard 34: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. Relates pressure, volume, moles, and temperature for ideal gases.

Flashcard 35: What units must pressure be in for the Ideal Gas Law when using $R = 0.0821$?

Answer: Atmospheres (atm). Required unit to match the gas constant $R$ value.

Flashcard 36: Determine $V$ for $P = 1.5$ atm, $n = 2$ mol, $T = 298$ K.

Answer: $V = 32.6$ L. Using $PV = nRT$: $V = \frac{(2)(0.0821)(298)}{1.5} = 32.6$ L.

Flashcard 37: If $V$ is halved and $n$ and $T$ are constant, what happens to $P$?

Answer: Pressure doubles. Volume is inversely proportional to pressure.

Flashcard 38: What does the variable $T$ represent in the Ideal Gas Law?

Answer: Temperature in Kelvin. Absolute temperature scale starting at absolute zero.

Flashcard 39: Calculate the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol.

Answer: $T = 273$ K. Using $PV = nRT$: $T = \frac{(1)(22.4)}{(1)(0.0821)} = 273$ K.

Flashcard 40: If $V$ is halved and $n$ and $T$ are constant, what happens to $P$?

Answer: Pressure doubles. Volume is inversely proportional to pressure.

Flashcard 41: Identify the units for $R$ when pressure is in Pascals.

Answer: Joules per mole Kelvin. Energy units appropriate for Pascal pressure measurements.

Flashcard 42: Identify the relationship between pressure and volume in the Ideal Gas Law.

Answer: Inversely proportional. When one increases, the other decreases (Boyle's Law).

Flashcard 43: What does the variable $P$ represent in the Ideal Gas Law?

Answer: Pressure of the gas. Force per unit area exerted by gas molecules on container walls.

Flashcard 44: How does the Ideal Gas Law change if $n$ is constant but $P$, $V$ change?

Answer: Boyle's Law. Special case where $PV =$ constant at fixed amount.

Flashcard 45: What happens to pressure when temperature decreases at constant $V$ and $n$?

Answer: Pressure decreases. Lower kinetic energy reduces molecular collisions with walls.

Flashcard 46: Identify the relationship between moles and volume in the Ideal Gas Law.

Answer: Directly proportional. More gas molecules occupy more space (Avogadro's Law).

Flashcard 47: What happens to volume when temperature increases at constant $P$ and $n$?

Answer: Volume increases. Higher kinetic energy causes gas to expand.

Flashcard 48: What happens to pressure when volume decreases at constant $n$ and $T$?

Answer: Pressure increases. Gas molecules compress into smaller space, creating higher pressure.

Flashcard 49: What does the variable $T$ represent in the Ideal Gas Law?

Answer: Temperature in Kelvin. Absolute temperature scale starting at absolute zero.

Flashcard 50: Find the temperature if $P = 3$ atm, $V = 10$ L, $n = 1$ mol.

Answer: $T = 366$ K. Using $PV = nRT$: $T = \frac{(3)(10)}{(1)(0.0821)} = 366$ K.

Flashcard 51: Determine $V$ for $P = 1.5$ atm, $n = 2$ mol, $T = 298$ K.

Answer: $V = 32.6$ L. Using $PV = nRT$: $V = \frac{(2)(0.0821)(298)}{1.5} = 32.6$ L.

Flashcard 52: Calculate the pressure if $n = 1$ mol, $V = 22.4$ L, $T = 273$ K.

Answer: $P = 1$ atm. Using $PV = nRT$: $P = \frac{(1)(0.0821)(273)}{22.4} = 1$ atm.

Flashcard 53: If $T$ doubles and $n$ and $V$ are constant, what happens to $P$?

Answer: Pressure doubles. Temperature is directly proportional to pressure.

Flashcard 54: In the Ideal Gas Law, what units must volume be in when using $R = 0.0821$?

Answer: Liters (L). Volume unit that corresponds to the standard $R$ value.

Flashcard 55: Convert 100°C to Kelvin for use in gas law calculations.

Answer: $373.15$ K. Add 273.15 to Celsius temperature.

Flashcard 56: What does the variable $P$ represent in the Ideal Gas Law?

Answer: Pressure of the gas. Force per unit area exerted by gas molecules on container walls.

Flashcard 57: Calculate the volume if $P = 2$ atm, $n = 1$ mol, $T = 273$ K.

Answer: $V = 11.2$ L. Using $PV = nRT$: $V = \frac{(1)(0.0821)(273)}{2} = 11.2$ L.

Flashcard 58: What happens to volume if both $P$ and $T$ double, while $n$ is constant?

Answer: Volume remains constant. Effects of pressure and temperature changes cancel out.

Flashcard 59: Calculate the pressure if $n = 1$ mol, $V = 22.4$ L, $T = 273$ K.

Answer: $P = 1$ atm. Using $PV = nRT$: $P = \frac{(1)(0.0821)(273)}{22.4} = 1$ atm.

Flashcard 60: Find the volume of 1 mole of gas at 1 atm and 273 K.

Answer: $V = 22.4$ L. Standard molar volume at STP conditions.

Flashcard 61: Identify the units for $R$ when using $8.314$ as the constant.

Answer: $J/(mol \times K)$. Energy per amount per temperature unit.

Flashcard 62: Find the pressure of 2 moles of gas at 300 K in a 10 L container.

Answer: $P = 4.92$ atm. Using $PV = nRT$: $P = \frac{(2)(0.0821)(300)}{10} = 4.92$ atm.

Flashcard 63: What does the variable $R$ represent in the Ideal Gas Law?

Answer: Ideal gas constant. Universal proportionality constant relating gas properties.

Flashcard 64: Calculate the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol.

Answer: $T = 273$ K. Using $PV = nRT$: $T = \frac{(1)(22.4)}{(1)(0.0821)} = 273$ K.

Flashcard 65: Calculate pressure when 0.5 mol of gas is at 350 K in a 5 L container.

Answer: $P = 2.87$ atm. Using $PV = nRT$: $P = \frac{(0.5)(0.0821)(350)}{5} = 2.87$ atm.

Flashcard 66: What is the temperature if $P = 5$ atm, $V = 20$ L, $n = 2$ mol?

Answer: $T = 609$ K. Using $PV = nRT$: $T = \frac{(5)(20)}{(2)(0.0821)} = 609$ K.

Flashcard 67: In the Ideal Gas Law, what units must volume be in when using $R = 0.0821$?

Answer: Liters (L). Volume unit that corresponds to the standard $R$ value.