Deviation from Ideal Gas Law - AP Chemistry
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What effect does increasing pressure have on gas behavior?
What effect does increasing pressure have on gas behavior?
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Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
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Identify another assumption of the Ideal Gas Law.
Identify another assumption of the Ideal Gas Law.
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Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.
Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.
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What is the effect of intermolecular forces on gas pressure?
What is the effect of intermolecular forces on gas pressure?
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Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.
Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.
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State the definition of an ideal gas.
State the definition of an ideal gas.
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An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.
An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.
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What effect does increasing pressure have on gas behavior?
What effect does increasing pressure have on gas behavior?
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Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
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Identify a situation where Ideal Gas Law fails.
Identify a situation where Ideal Gas Law fails.
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At very high pressures. Extreme pressure makes particle volume and forces significant.
At very high pressures. Extreme pressure makes particle volume and forces significant.
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Provide the value of the universal gas constant 'R'.
Provide the value of the universal gas constant 'R'.
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$R = 0.0821 \frac{L \times atm}{mol \times K}$. The standard value used in gas law calculations.
$R = 0.0821 \frac{L \times atm}{mol \times K}$. The standard value used in gas law calculations.
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Name one assumption of the Ideal Gas Law.
Name one assumption of the Ideal Gas Law.
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Gas particles have no volume. Assumes particles are point masses with negligible size.
Gas particles have no volume. Assumes particles are point masses with negligible size.
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What is the significance of 'R' in the Ideal Gas Law?
What is the significance of 'R' in the Ideal Gas Law?
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'R' is the universal gas constant. A proportionality constant linking pressure, volume, moles, and temperature.
'R' is the universal gas constant. A proportionality constant linking pressure, volume, moles, and temperature.
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What causes real gases to deviate from ideal behavior at high pressures?
What causes real gases to deviate from ideal behavior at high pressures?
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Finite volume of gas particles. Molecular volume becomes significant fraction of container volume.
Finite volume of gas particles. Molecular volume becomes significant fraction of container volume.
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What is the Ideal Gas Law equation?
What is the Ideal Gas Law equation?
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$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature.
$PV = nRT$. The fundamental relationship between pressure, volume, moles, and temperature.
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Name a condition under which real gases deviate from ideal behavior.
Name a condition under which real gases deviate from ideal behavior.
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High pressure. Forces particles closer, making volume and intermolecular forces significant.
High pressure. Forces particles closer, making volume and intermolecular forces significant.
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Find the pressure correction in Van der Waals equation for $1 \text{mol}$ of gas.
Find the pressure correction in Van der Waals equation for $1 \text{mol}$ of gas.
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$\frac{a}{V^2}$. For 1 mole, $n = 1$, so the correction becomes $\frac{a}{V^2}$.
$\frac{a}{V^2}$. For 1 mole, $n = 1$, so the correction becomes $\frac{a}{V^2}$.
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Identify the correction factor for intermolecular forces in Van der Waals.
Identify the correction factor for intermolecular forces in Van der Waals.
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$\frac{an^2}{V^2}$. Accounts for attractive forces reducing observed pressure.
$\frac{an^2}{V^2}$. Accounts for attractive forces reducing observed pressure.
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Which gas law relates volume and temperature at constant pressure?
Which gas law relates volume and temperature at constant pressure?
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Charles's Law. States that $V/T$ is constant at fixed pressure.
Charles's Law. States that $V/T$ is constant at fixed pressure.
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What is the primary focus of the Van der Waals equation?
What is the primary focus of the Van der Waals equation?
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Correcting Ideal Gas Law for real gases. Modifies ideal gas law to account for real gas behavior.
Correcting Ideal Gas Law for real gases. Modifies ideal gas law to account for real gas behavior.
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Calculate $P$ if $V = 10 \text{L}$, $n = 1 \text{mol}$, $T = 300 \text{K}$, $R = 0.0821$.
Calculate $P$ if $V = 10 \text{L}$, $n = 1 \text{mol}$, $T = 300 \text{K}$, $R = 0.0821$.
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$P = \frac{nRT}{V} = 2.463 \text{atm}$. Using $P = \frac{nRT}{V}$ with given values yields 2.463 atm.
$P = \frac{nRT}{V} = 2.463 \text{atm}$. Using $P = \frac{nRT}{V}$ with given values yields 2.463 atm.
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What does a high value of 'a' indicate in Van der Waals equation?
What does a high value of 'a' indicate in Van der Waals equation?
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Strong intermolecular forces. Large 'a' means strong attractive forces between molecules.
Strong intermolecular forces. Large 'a' means strong attractive forces between molecules.
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What happens to $PV/nRT$ for an ideal gas?
What happens to $PV/nRT$ for an ideal gas?
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Equals 1. Compressibility factor equals 1 for perfect ideal behavior.
Equals 1. Compressibility factor equals 1 for perfect ideal behavior.
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State the critical temperature's influence on gas behavior.
State the critical temperature's influence on gas behavior.
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Above it, gases behave more ideally. Higher temperatures overcome intermolecular forces, approaching ideal behavior.
Above it, gases behave more ideally. Higher temperatures overcome intermolecular forces, approaching ideal behavior.
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Identify a gas that behaves nearly ideally under ordinary conditions.
Identify a gas that behaves nearly ideally under ordinary conditions.
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Helium. Small, light atoms with weak intermolecular forces.
Helium. Small, light atoms with weak intermolecular forces.
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Calculate pressure deviation using $P = 4 \text{atm}$, $a = 0.8$, $V = 20 \text{L}$.
Calculate pressure deviation using $P = 4 \text{atm}$, $a = 0.8$, $V = 20 \text{L}$.
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$\text{Deviation} = \frac{0.8}{20^2}$. Pressure correction term: $\frac{a}{V^2}$ for 1 mole of gas.
$\text{Deviation} = \frac{0.8}{20^2}$. Pressure correction term: $\frac{a}{V^2}$ for 1 mole of gas.
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Calculate corrected pressure using $P = 3 \text{atm}$, $a = 0.5$, $V = 10 \text{L}$.
Calculate corrected pressure using $P = 3 \text{atm}$, $a = 0.5$, $V = 10 \text{L}$.
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$P' = 3 + \frac{0.5}{10^2} = 3.005 \text{atm}$. Adding pressure correction: $P + \frac{an^2}{V^2}$ for $n=1$.
$P' = 3 + \frac{0.5}{10^2} = 3.005 \text{atm}$. Adding pressure correction: $P + \frac{an^2}{V^2}$ for $n=1$.
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What effect does increasing pressure have on gas behavior?
What effect does increasing pressure have on gas behavior?
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Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
Gases deviate more from ideal behavior. Higher pressure compresses gas, making particle volume more significant.
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Identify another assumption of the Ideal Gas Law.
Identify another assumption of the Ideal Gas Law.
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Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.
Gas particles exert no intermolecular forces. Assumes no attractive or repulsive forces between particles.
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What is the effect of intermolecular forces on gas pressure?
What is the effect of intermolecular forces on gas pressure?
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Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.
Decreases observed pressure. Attractive forces reduce pressure exerted on container walls.
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State the definition of an ideal gas.
State the definition of an ideal gas.
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An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.
An ideal gas perfectly follows the Ideal Gas Law. A theoretical gas that obeys all gas law assumptions perfectly.
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Name another condition for deviation from ideal behavior.
Name another condition for deviation from ideal behavior.
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Low temperature. Reduces kinetic energy, allowing intermolecular forces to dominate.
Low temperature. Reduces kinetic energy, allowing intermolecular forces to dominate.
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What is the Van der Waals equation?
What is the Van der Waals equation?
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$(P + \frac{an^2}{V^2})(V - nb) = nRT$. Modified ideal gas law accounting for real gas behavior.
$(P + \frac{an^2}{V^2})(V - nb) = nRT$. Modified ideal gas law accounting for real gas behavior.
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What does 'a' in Van der Waals equation account for?
What does 'a' in Van der Waals equation account for?
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Intermolecular attraction forces. Parameter representing strength of intermolecular attractive forces.
Intermolecular attraction forces. Parameter representing strength of intermolecular attractive forces.
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