AP Chemistry Flashcards: Ideal Gas Law

What this deck covers

This deck focuses on Ideal Gas Law, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

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: Convert 25°C to Kelvin.

Answer: 298 K. Add 273.15 to convert Celsius to Kelvin.

Flashcard 2: What is an ideal gas?

Answer: A hypothetical gas with perfectly elastic collisions. Gas with no intermolecular forces and negligible particle volume.

Flashcard 3: Identify the unit of pressure in the Ideal Gas Law.

Answer: Atmospheres (atm). Standard unit of pressure in gas law calculations.

Flashcard 4: What is the relationship between temperature and kinetic energy?

Answer: Directly proportional. Higher temperature means faster-moving gas molecules.

Flashcard 5: What does the variable $P$ represent in the Ideal Gas Law?

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

Flashcard 6: State the formula for Boyle's Law.

Answer: $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

Flashcard 7: Find $n$ if $P = 1$ atm, $V = 24.4$ L, $T = 298$ K.

Answer: 1 mol. Using $n = \frac{PV}{RT} = \frac{1 \times 24.4}{298 \times 0.0821}$.

Flashcard 8: Identify the proportionality in Charles's Law.

Answer: Volume is directly proportional to temperature. At constant pressure, volume increases linearly with temperature.

Flashcard 9: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

Flashcard 10: What is the effect on pressure if moles double at constant $V$ and $T$?

Answer: Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

Flashcard 11: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

Flashcard 12: Identify the proportionality in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

Flashcard 13: Identify the unit of the ideal gas constant $R$.

Answer: L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

Flashcard 14: What is the effect on pressure if moles double at constant $V$ and $T$?

Answer: Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

Flashcard 15: If $P = 2$ atm, $V = 5$ L, $T = 300$ K, find the moles of gas.

Answer: 0.406 mol. Using $n = \frac{PV}{RT} = \frac{2 \times 5}{0.0821 \times 300}$.

Flashcard 16: Find the pressure when $V=10$ L, $T=300$ K, $n=1$ mol, $R=0.0821$

Answer: 2.46 atm. Using $P = \frac{nRT}{V} = \frac{1 \times 0.0821 \times 300}{10}$.

Flashcard 17: Identify the proportionality in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

Flashcard 18: Identify the unit of temperature in the Ideal Gas Law.

Answer: Kelvin (K). Absolute temperature scale required for gas law calculations.

Flashcard 19: State the combined gas law formula.

Answer: $\frac{P_1V_1}{T_1} = \frac{P_2V_2}{T_2}$. Relates initial and final states when moles remain constant.

Flashcard 20: What does the variable $V$ stand for in the Ideal Gas Law?

Answer: Volume. Space occupied by the gas, typically measured in liters.

Flashcard 21: State the formula for Boyle's Law.

Answer: $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

Flashcard 22: Calculate $T$ if $P = 3$ atm, $V = 5$ L, $n = 0.5$ mol, $R = 0.0821$.

Answer: 366 K. Using $T = \frac{PV}{nR} = \frac{3 \times 5}{0.5 \times 0.0821}$.

Flashcard 23: What happens to volume if both $P$ and $T$ double?

Answer: Volume remains the same. Both pressure and temperature changes cancel out in the ideal gas law.

Flashcard 24: Identify the proportionality in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

Flashcard 25: What happens to pressure if volume halves at constant $n$ and $T$?

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

Flashcard 26: State the formula for Avogadro's Law.

Answer: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$. Volume-moles relationship at constant pressure and temperature.

Flashcard 27: If $P = 3$ atm and $T$ doubles, what is new $P$ at constant $V$?

Answer: 6 atm. Direct proportionality from Gay-Lussac's Law.

Flashcard 28: State the formula for Boyle's Law.

Answer: $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

Flashcard 29: Identify the unit of volume in the Ideal Gas Law.

Answer: Liters (L). Standard unit of volume in gas law calculations.

Flashcard 30: What does the variable $R$ represent in the Ideal Gas Law?

Answer: Ideal gas constant. Universal constant relating gas properties, equal to 0.0821 L atm mol$^{-1}$ K$^{-1}$.

Flashcard 31: What happens to pressure if volume halves at constant $n$ and $T$?

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

Flashcard 32: What condition must be met for an ideal gas?

Answer: Low pressure and high temperature. Minimal intermolecular forces and particle volume for ideal behavior.

Flashcard 33: What is the effect on pressure if moles double at constant $V$ and $T$?

Answer: Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

Flashcard 34: What condition must be met for an ideal gas?

Answer: Low pressure and high temperature. Minimal intermolecular forces and particle volume for ideal behavior.

Flashcard 35: State the formula for Boyle's Law.

Answer: $P_1V_1 = P_2V_2$. Pressure-volume relationship at constant temperature and moles.

Flashcard 36: State Gay-Lussac's Law formula.

Answer: $\frac{P_1}{T_1} = \frac{P_2}{T_2}$. Pressure-temperature relationship at constant volume and moles.

Flashcard 37: Calculate the pressure when $n = 2$, $V = 10$ L, $T = 300$ K, $R = 0.0821$.

Answer: 4.92 atm. Using $P = \frac{nRT}{V} = \frac{2 \times 0.0821 \times 300}{10}$.

Flashcard 38: If $P = 2$ atm, $V = 5$ L, $T = 300$ K, find the moles of gas.

Answer: 0.406 mol. Using $n = \frac{PV}{RT} = \frac{2 \times 5}{0.0821 \times 300}$.

Flashcard 39: State the formula for Charles's Law.

Answer: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$. Volume-temperature relationship at constant pressure and moles.

Flashcard 40: State the value of the ideal gas constant $R$.

Answer: 0.0821 L atm mol$^{-1}$ K$^{-1}$. Standard value used in ideal gas calculations.

Flashcard 41: Find the pressure when $V=10$ L, $T=300$ K, $n=1$ mol, $R=0.0821$

Answer: 2.46 atm. Using $P = \frac{nRT}{V} = \frac{1 \times 0.0821 \times 300}{10}$.

Flashcard 42: What does the variable $T$ represent in the Ideal Gas Law?

Answer: Temperature in Kelvin. Absolute temperature scale where molecular motion ceases at 0 K.

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

Answer: Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

Flashcard 44: Find $n$ if $P = 1$ atm, $V = 24.4$ L, $T = 298$ K.

Answer: 1 mol. Using $n = \frac{PV}{RT} = \frac{1 \times 24.4}{298 \times 0.0821}$.

Flashcard 45: What is the standard temperature in Kelvin?

Answer: 273 K. Absolute zero on the Kelvin scale, equivalent to 0°C.

Flashcard 46: What happens to volume if both $P$ and $T$ double?

Answer: Volume remains the same. Both pressure and temperature changes cancel out in the ideal gas law.

Flashcard 47: What is the effect on volume if pressure triples at constant $T$?

Answer: Volume decreases to one-third. Inverse relationship from Boyle's Law.

Flashcard 48: Calculate $T$ if $P = 3$ atm, $V = 5$ L, $n = 0.5$ mol, $R = 0.0821$.

Answer: 366 K. Using $T = \frac{PV}{nR} = \frac{3 \times 5}{0.5 \times 0.0821}$.

Flashcard 49: Identify the unit of volume in the Ideal Gas Law.

Answer: Liters (L). Standard unit of volume in gas law calculations.

Flashcard 50: Convert 25°C to Kelvin.

Answer: 298 K. Add 273.15 to convert Celsius to Kelvin.

Flashcard 51: What does the variable $n$ represent in the Ideal Gas Law?

Answer: Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

Flashcard 52: Identify the unit of the ideal gas constant $R$.

Answer: L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

Flashcard 53: What does the variable $R$ represent in the Ideal Gas Law?

Answer: Ideal gas constant. Universal constant relating gas properties, equal to 0.0821 L atm mol$^{-1}$ K$^{-1}$.

Flashcard 54: Identify the proportionality in Charles's Law.

Answer: Volume is directly proportional to temperature. At constant pressure, volume increases linearly with temperature.

Flashcard 55: Identify the unit of the ideal gas constant $R$.

Answer: L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.

Flashcard 56: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

Flashcard 57: What is the effect on pressure if moles double at constant $V$ and $T$?

Answer: Pressure doubles. More gas particles create greater pressure at constant volume and temperature.

Flashcard 58: What happens to volume if temperature doubles at constant $P$ and $n$?

Answer: Volume doubles. Direct relationship from Charles's Law at constant pressure.

Flashcard 59: Determine the volume if $P = 1$ atm, $n = 1$ mol, $T = 273$ K, $R = 0.0821$.

Answer: 22.4 L. Molar volume of an ideal gas at STP (standard temperature and pressure).

Flashcard 60: State the value of the ideal gas constant $R$.

Answer: 0.0821 L atm mol$^{-1}$ K$^{-1}$. Standard value used in ideal gas calculations.

Flashcard 61: Convert 300 K to Celsius.

Answer: 27°C. Subtract 273.15 to convert Kelvin to Celsius.

Flashcard 62: Identify the law: Volume is constant as pressure and temperature change.

Answer: Gay-Lussac's Law. Describes pressure-temperature relationship at constant volume.

Flashcard 63: State the formula for the Ideal Gas Law.

Answer: $PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature for ideal gases.

Flashcard 64: What does the variable $n$ represent in the Ideal Gas Law?

Answer: Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

Flashcard 65: What does the variable $n$ represent in the Ideal Gas Law?

Answer: Amount of substance in moles. Number of moles quantifies the amount of gas particles present.

Flashcard 66: Identify the proportionality in Boyle's Law.

Answer: Pressure is inversely proportional to volume. At constant temperature, decreasing volume increases pressure proportionally.

Flashcard 67: Identify the proportionality in Avogadro's Law.

Answer: Volume is directly proportional to moles. At constant pressure and temperature, volume scales with particle number.

Flashcard 68: Find the temperature if $P = 1$ atm, $V = 22.4$ L, $n = 1$ mol, $R = 0.0821$.

Answer: 273 K. Using $T = \frac{PV}{nR} = \frac{1 \times 22.4}{1 \times 0.0821}$.

Flashcard 69: If $P = 3$ atm and $T$ doubles, what is new $P$ at constant $V$?

Answer: 6 atm. Direct proportionality from Gay-Lussac's Law.

Flashcard 70: Identify the unit of the ideal gas constant $R$.

Answer: L atm mol$^{-1}$ K$^{-1}$. Combines units of pressure, volume, temperature, and moles.