AP Chemistry Flashcards: Deviation From Ideal Gas Law

What this deck covers

This deck focuses on Deviation From 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: What effect does increasing pressure have on gas behavior?

Answer: Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.

Flashcard 2: Identify another assumption of the Ideal Gas Law.

Answer: Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.

Flashcard 3: What is the effect of intermolecular forces on gas pressure?

Answer: Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.

Flashcard 4: State the definition of an ideal gas.

Answer: An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.

Flashcard 5: What effect does increasing pressure have on gas behavior?

Answer: Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.

Flashcard 6: Identify a situation where Ideal Gas Law fails.

Answer: At very high pressures. Extreme pressure makes particle volume and forces significant.

Flashcard 7: Provide the value of the universal gas constant 'R'.

Answer: $R = 0.0821 \frac{L \times atm}{mol \times K}$. The standard value used in gas law calculations.

Flashcard 8: Name one assumption of the Ideal Gas Law.

Answer: Gas particles have no volume. Assumes particles are point masses with negligible size.

Flashcard 9: What is the significance of 'R' in the Ideal Gas Law?

Answer: 'R' is the universal gas constant. A proportionality constant linking pressure, volume, moles, and temperature.

Flashcard 10: What causes real gases to deviate from ideal behavior at high pressures?

Answer: Finite volume of gas particles. Molecular volume becomes significant fraction of container volume.

Flashcard 11: What is the Ideal Gas Law equation?

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

Flashcard 12: Name a condition under which real gases deviate from ideal behavior.

Answer: High pressure. Forces particles closer, making volume and intermolecular forces significant.

Flashcard 13: Find the pressure correction in Van der Waals equation for $1 \text{mol}$ of gas.

Answer: $\frac{a}{V^2}$. For 1 mole, $n = 1$, so the correction becomes $\frac{a}{V^2}$.

Flashcard 14: Identify the correction factor for intermolecular forces in Van der Waals.

Answer: $\frac{an^2}{V^2}$. Accounts for attractive forces reducing observed pressure.

Flashcard 15: Which gas law relates volume and temperature at constant pressure?

Answer: Charles's Law. States that $V/T$ is constant at fixed pressure.

Flashcard 16: What is the primary focus of the Van der Waals equation?

Answer: Correcting Ideal Gas Law for real gases. Modifies ideal gas law to account for real gas behavior.

Flashcard 17: Calculate $P$ if $V = 10 \text{L}$, $n = 1 \text{mol}$, $T = 300 \text{K}$, $R = 0.0821$.

Answer: $P = \frac{nRT}{V} = 2.463 \text{atm}$. Using $P = \frac{nRT}{V}$ with given values yields 2.463 atm.

Flashcard 18: What does a high value of 'a' indicate in Van der Waals equation?

Answer: Strong intermolecular forces. Large 'a' means strong attractive forces between molecules.

Flashcard 19: What happens to $PV/nRT$ for an ideal gas?

Answer: Equals 1. Compressibility factor equals 1 for perfect ideal behavior.

Flashcard 20: State the critical temperature's influence on gas behavior.

Answer: Above it, gases behave more ideally. Higher temperatures overcome intermolecular forces, approaching ideal behavior.

Flashcard 21: Identify a gas that behaves nearly ideally under ordinary conditions.

Answer: Helium. Small, light atoms with weak intermolecular forces.

Flashcard 22: Calculate pressure deviation using $P = 4 \text{atm}$, $a = 0.8$, $V = 20 \text{L}$.

Answer: $\text{Deviation} = \frac{0.8}{20^2}$. Pressure correction term: $\frac{a}{V^2}$ for 1 mole of gas.

Flashcard 23: Calculate corrected pressure using $P = 3 \text{atm}$, $a = 0.5$, $V = 10 \text{L}$.

Answer: $P' = 3 + \frac{0.5}{10^2} = 3.005 \text{atm}$. Adding pressure correction: $P + \frac{an^2}{V^2}$ for $n=1$.

Flashcard 24: What effect does increasing pressure have on gas behavior?

Answer: Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.

Flashcard 25: Identify another assumption of the Ideal Gas Law.

Answer: Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.

Flashcard 26: What is the effect of intermolecular forces on gas pressure?

Answer: Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.

Flashcard 27: State the definition of an ideal gas.

Answer: An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.

Flashcard 28: Name another condition for deviation from ideal behavior.

Answer: Low temperature. Reduces kinetic energy, allowing intermolecular forces to dominate.

Flashcard 29: What is the Van der Waals equation?

Answer: $(P + \frac{an^2}{V^2})(V - nb) = nRT$. Modified ideal gas law accounting for real gas behavior.

Flashcard 30: What does 'a' in Van der Waals equation account for?

Answer: Intermolecular attraction forces. Parameter representing strength of intermolecular attractive forces.