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Questions and Answers
Which statement accurately describes the particle behavior in gases?
Which statement accurately describes the particle behavior in gases?
- Particles are arranged in a fixed lattice structure.
- Particles are closely packed and have strong interparticle forces.
- Particles have a definite volume but no definite shape.
- Particles are loosely packed, exhibiting negligible interparticle forces. (correct)
According to the kinetic molecular theory, collisions between gas particles are considered perfectly inelastic.
According to the kinetic molecular theory, collisions between gas particles are considered perfectly inelastic.
False (B)
What is the relationship between Kelvin temperature and the average kinetic energy of gas molecules?
What is the relationship between Kelvin temperature and the average kinetic energy of gas molecules?
directly proportional
Boyle's Law states that at constant temperature, the pressure of a gas is __________ proportional to its volume.
Boyle's Law states that at constant temperature, the pressure of a gas is __________ proportional to its volume.
Match each gas law with its correct formula:
Match each gas law with its correct formula:
A container holds 2 moles of hydrogen gas, 3 moles of oxygen gas, and 1 mole of nitrogen gas. If the total pressure is 12 atm, what is the partial pressure of oxygen?
A container holds 2 moles of hydrogen gas, 3 moles of oxygen gas, and 1 mole of nitrogen gas. If the total pressure is 12 atm, what is the partial pressure of oxygen?
The rate of diffusion of a gas is directly proportional to the square root of its molar mass.
The rate of diffusion of a gas is directly proportional to the square root of its molar mass.
What measurable property of a gas is defined as the amount of space it occupies?
What measurable property of a gas is defined as the amount of space it occupies?
The combined gas law relates pressure, volume, and temperature when the amount of gas (moles) remains __________.
The combined gas law relates pressure, volume, and temperature when the amount of gas (moles) remains __________.
A gas occupies 10 L at standard temperature and pressure (STP). If the amount of gas is doubled, what is the new volume, assuming temperature and pressure remain constant?
A gas occupies 10 L at standard temperature and pressure (STP). If the amount of gas is doubled, what is the new volume, assuming temperature and pressure remain constant?
Flashcards
Gases Properties
Gases Properties
Atoms are farthest apart & move randomly. They mix easily with other gases and have lower densities.
Kinetic Molecular Theory
Kinetic Molecular Theory
Gas molecules are in constant, random motion. They collide with container walls in perfectly elastic collisions, resulting in pressure.
Gas Volume (V)
Gas Volume (V)
Amount of space a gas occupies, expanding to fill containers; measured in mL, L, or cubic meters.
Moles of Gas (n)
Moles of Gas (n)
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Temperature (T)
Temperature (T)
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Pressure (P)
Pressure (P)
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Boyle's Law
Boyle's Law
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Charles' Law
Charles' Law
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Gay-Lussac's Law
Gay-Lussac's Law
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Avogadro's Law
Avogadro's Law
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Study Notes
- Gases consist of atoms that are far apart and move randomly
- Gases exhibit diffusion, readily mixing with other gases, and have low densities
Properties of Matter
- Solids have a definite mass and shape, are not compressible, and have high rigidity
- Liquids have a definite mass but adapt to the container shape and are not very compressible
- Gases have a definite mass, indefinite shape and are highly compressible
- Solids have slow diffusion and are closely packed
- Liquids have fast diffusion and are less closely packed
- Gases have very fast diffusion and are loosely packed
- Interparticle forces are strongest in solids, slightly weaker in liquids, and negligible in gases
- Solids are densest, liquids are less dense, and gases are least dense
- Kinetic energy is lowest in solids, low in liquids, and high in gases
Kinetic Molecular Theory
- Gas molecules are in constant, random, straight-line motion, colliding with container walls
- Collisions are perfectly elastic, causing molecules to bounce back
Gas Properties
- Collisions result in pressure, and molecules have mass
- Gases lack attraction or repulsion forces
- Gases possess the same average kinetic energy directly proportional to absolute Kelvin temperature
Measurable Properties of Gases
- Volume (V) is the amount of space, gas molecules expand to fill containers, measured in milliliters (mL), liters (L), and cubic meters (m³)
- Moles of Gas (n) denotes the amount of gas, measured in moles or mol
- Temperature (T) refers to average kinetic energy, measured in Fahrenheit (°F), Celsius (°C), or Kelvin (K)
- Pressure (P) is the force exerted by all gases due to collisions, measured in atmosphere (atm), Pascal (Pa), Torr, and millimeter of Mercury (mmHg)
Gas Laws
- Gas laws originated in the late 18th century, relating pressure, volume, temperature, and moles of gas
Boyle's Law
- Discovered by Robert Boyle, under constant temperature, pressure and volume are inversely proportional
- Higher temperature corresponds to lesser volume
- Formula: P1V1 = P2V2
Charles' Law
- Discovered by Jacques Charles, under constant pressure and mass, temperature and volume are directly proportional
- Higher temperature corresponds to higher volume
- Formula: V1/T1 = V2/T2
Gay-Lussac's Law
- Discovered by Joseph Louis Gay-Lussac, temperature and pressure are directly proportional
- Higher temperature corresponds to higher pressure
- Formula: P1/T1 = P2/T2
Avogadro's Law
- Discovered by Amadeo Avogadro, volume and moles of gas are directly proportional
- Higher volume corresponds to more moles of gas
- Formula: V1/n1 = V2/n2
Combined Gas Law
- Combination of Boyle's, Charles', and Gay-Lussac's Laws, relating pressure, volume, and temperature
- Formula: P1V1/T1 = P2V2/T2
Ideal Gas Law
- Approximates real gas behavior and relates pressure, volume, temperature, and moles of gas
- Formula: PV = nRT
Dalton's Law on Partial Pressure
- Partial pressure refers to pressure of 1 gas in a mixture, establishing the relationship between pressure and moles of gas, gas molecules behave independently
- Formulas: Ptotal = P1 + P2, P1 = XA * Ptotal, XA = nA / ntotal
Graham's Law on Effusion and Diffusion
- Diffusion is the readily mixing of gases
- Effusion is the movement of particles through a hole
- Formula: RA/RB = sqrt(MB) / sqrt(MA)
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