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Questions and Answers
What is the primary reason gases can be compressed easily?
What is the primary reason gases can be compressed easily?
- Particles are in fixed positions.
- Particles are closely packed together.
- Particles have negligible volume.
- Particles are widely separated and have high energy. (correct)
The pressure exerted by a gas is the result of collisions of gas particles with the walls of their container.
The pressure exerted by a gas is the result of collisions of gas particles with the walls of their container.
True (A)
What is the equation that represents Boyle's Law?
What is the equation that represents Boyle's Law?
PV = constant
At standard atmospheric pressure, 1 atm is equal to _____ torr.
At standard atmospheric pressure, 1 atm is equal to _____ torr.
Match the following laws with their definitions:
Match the following laws with their definitions:
What happens to the volume of a gas if its temperature is increased while keeping pressure constant?
What happens to the volume of a gas if its temperature is increased while keeping pressure constant?
Gases have a definite shape and volume.
Gases have a definite shape and volume.
What unit is used to measure pressure in the metric system?
What unit is used to measure pressure in the metric system?
What is the compressibility factor of an ideal gas?
What is the compressibility factor of an ideal gas?
Gases behave non-ideally at high temperatures and low pressures.
Gases behave non-ideally at high temperatures and low pressures.
What is the primary characteristic of the compressibility factor for real gases at very high pressures?
What is the primary characteristic of the compressibility factor for real gases at very high pressures?
According to the van der Waals equation, the term 'b' measures the __________ occupied by gas molecules.
According to the van der Waals equation, the term 'b' measures the __________ occupied by gas molecules.
Match the van der Waals constants with their descriptions:
Match the van der Waals constants with their descriptions:
At low pressures, how do gases behave?
At low pressures, how do gases behave?
Boyle’s Law accurately predicts gas behavior under all pressure conditions.
Boyle’s Law accurately predicts gas behavior under all pressure conditions.
What phenomenon occurs due to intermolecular forces in gases at high pressures?
What phenomenon occurs due to intermolecular forces in gases at high pressures?
What is the relationship defined by Avogadro's Law?
What is the relationship defined by Avogadro's Law?
At standard temperature and pressure (STP), one mole of gas occupies 22.4 L.
At standard temperature and pressure (STP), one mole of gas occupies 22.4 L.
What is the ideal gas equation?
What is the ideal gas equation?
The standard temperature is __ degrees Celsius.
The standard temperature is __ degrees Celsius.
Match the gas law with its corresponding principle:
Match the gas law with its corresponding principle:
What is the molar volume of a gas at standard conditions?
What is the molar volume of a gas at standard conditions?
In a gas mixture, each gas behaves as if it is the only gas present in the container.
In a gas mixture, each gas behaves as if it is the only gas present in the container.
The compressibility factor measures how much a gas deviates from __ gas behavior.
The compressibility factor measures how much a gas deviates from __ gas behavior.
Flashcards
Gas pressure
Gas pressure
Force exerted by gas molecules on container walls.
Boyle's Law
Boyle's Law
At constant temperature, pressure and volume of a gas are inversely proportional.
Charles's Law
Charles's Law
At constant pressure, volume of a gas is directly proportional to its temperature (in Kelvin).
Gas
Gas
State of matter where particles are widely separated, move rapidly, and fill their container.
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Temperature (in gas)
Temperature (in gas)
Average kinetic energy of gas particles.
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Pressure (in gas)
Pressure (in gas)
Force per unit area exerted by gas particles.
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Ideal Gas Law
Ideal Gas Law
Combines Boyle's and Charles's Law
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Units of pressure
Units of pressure
Measurements of the force exerted by a gas.
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Kelvin Temperature
Kelvin Temperature
A temperature scale where 0 K represents absolute zero, the point at which molecular motion ceases.
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Avogadro's Law
Avogadro's Law
At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles present.
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Standard Temperature and Pressure (STP)
Standard Temperature and Pressure (STP)
Standard conditions (0°C, 1 atm) used to compare different gas properties.
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Ideal Gas Equation
Ideal Gas Equation
The equation PV = nRT that relates pressure (P), volume (V), number of moles (n), temperature (T), and the ideal gas constant (R).
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Dalton's Law of Partial Pressures
Dalton's Law of Partial Pressures
The total pressure of a mixture of gases is the sum of the partial pressures of each individual gas in the mixture.
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Mole Fraction
Mole Fraction
The ratio of the moles of a particular component to the total moles in a mixture.
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Partial Pressure
Partial Pressure
The pressure exerted by a particular gas in a mixture.
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Real Gases
Real Gases
Gases that do not behave ideally because of intermolecular forces and finite molecular volume, as opposed to ideal gases.
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Compressibility Factor
Compressibility Factor
A measure of how much a real gas deviates from ideal gas behavior.
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Ideal Gas
Ideal Gas
A gas whose behavior perfectly follows the gas laws.
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Van der Waals Equation
Van der Waals Equation
An equation of state that corrects for the non-ideal behavior of real gases.
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Van der Waals constant 'a'
Van der Waals constant 'a'
Measures the strength of the intermolecular attractive forces in a gas.
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Van der Waals constant 'b'
Van der Waals constant 'b'
Represents the volume occupied by the gas molecules themselves.
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Non-ideal gas behavior
Non-ideal gas behavior
Deviation from the predictions of the ideal gas law at high pressures or low temperatures.
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Ideal conditions
Ideal conditions
High temperatures and low pressures at which gases often behave nearly ideally.
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Gases
- Gases expand to fill their containers.
- Gases are highly compressible.
- Gases have extremely low densities.
- Gases are mainly composed of nonmetallic elements with simple formulas and low molar masses.
- Two or more gases form a homogeneous mixture.
Models for States of Matter
- Gas: Widely separated particles in continuous, rapid, disordered motion.
- Liquid: Particles in contact, able to move past each other.
- Solid: Particles in contact, unable to move past each other.
Properties Defining a Gas Sample
- Temperature: Average velocity of gas constituents.
- Volume: Size of the container.
- Amount: Number of moles (n).
- Pressure: Force exerted on container walls by gas constituents.
Pressure
- Pressure is the amount of force applied to an area (P = F/A).
- Pascal (Pa) is the SI unit of pressure (1 Pa = 1 N/m²).
- 1 bar = 10⁵ Pa = 100 kPa.
- Standard atmospheric pressure is the normal atmospheric pressure at sea level.
- 1.00 atm = 760 torr = 760 mmHg
Boyle's Law
- At constant temperature, gas volume is inversely proportional to pressure.
- P₁V₁ = P₂V₂
Charles's Law
- At constant pressure, gas volume is directly proportional to absolute temperature.
- V₁/T₁ = V₂/T₂
Avogadro's Law
- At constant temperature and pressure, gas volume is directly proportional to the number of moles.
- V₁/n₁ = V₂/n₂
Standard Conditions of Temperature and Pressure (STP)
- Standard temperature: 0°C = 273 K.
- Standard pressure: 1 atm = 760 mmHg.
- One mole of gas occupies 22.4 L at STP (molar volume).
Ideal Gas Equation
- PV = nRT
- P = pressure, V = volume, n = moles, R = ideal gas constant, T = temperature.
- R has various values depending on the units used for pressure, volume, and temperature such as: L-atm /mol-K, J/mol-K, etc.
Dalton's Law of Partial Pressures
- The total pressure of a mixture of non-reacting gases is the sum of the partial pressures of each gas.
- Ptotal = P1 + P2 + P3 + ...
Mole Fraction
- Mole fraction (Xᵢ) is the ratio of moles of a component to the total moles in a mixture.
- X₁ = n₁/ntotal
- Partial pressure of a gas (P₁) is given by P₁ = X₁Ptotal
Non-ideal (Real) Gases
- Real gases deviate from ideal gas behavior at high pressures or low temperatures.
- Compressibility factor(Z) quantifies this deviation: Z = PV/nRT. For ideal gases, Z =1
- Intermolecular forces and molecular volume are important for real gases.
The van der Waals Equation
- (P + a(n/V)²)(V – nb) = nRT
- a and b are van der Waals constants which correct for intermolecular forces and the finite volume of the gas molecules respectively.
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