Chapter 4: States Of Matter Flashcards
(17 cards)
Describe the gaseous state in terms of particles moving randomly and rapidly.
Gas particles are far apart and move freely in random directions at high speeds with negligible forces between them.
This describes the behavior and arrangement of particles in the gaseous state.
What is Boyle’s Law?
p ∝ 1/V (at constant temperature)
Boyle’s Law states that when the volume decreases, the pressure increases due to more frequent collisions.
What does Charles’ Law state?
V ∝ T (in kelvin) (at constant pressure)
In Charles’ Law, heating a gas increases the average kinetic energy, leading to volume expansion.
What is the Pressure Law?
p ∝ T (in kelvin) (at constant volume)
According to the Pressure Law, higher temperature causes faster particle motion, increasing pressure.
What is the ideal gas equation?
pV = nRT
Where p = pressure in Pascals (Pa), V = volume in cubic metres (m³), n = number of moles, R = gas constant = 8.31 J mol⁻¹ K⁻¹, T = temperature in Kelvin (K).
How do you calculate the number of moles using the ideal gas equation?
n = pV / RT
This rearrangement of the ideal gas equation allows for the calculation of the amount of gas.
How do you convert cm³ to m³?
÷ 1,000,000
This conversion is necessary when using the ideal gas equation.
How do you convert °C to K?
+ 273
This conversion is important for temperature when applying gas laws.
Describe the liquid state in terms of particle arrangement and motion.
Particles are close together with some movement. They can slide over one another, allowing the liquid to flow.
This outlines the characteristics of particles in the liquid state.
What are the properties of liquids in terms of intermolecular forces?
- Nearly incompressible due to small spaces between particles
- Intermolecular forces are weaker than in solids but stronger than in gases
These properties explain the behavior of liquids compared to solids and gases.
Describe the solid state in terms of particle arrangement and motion.
Particles are tightly packed in a fixed, orderly arrangement. They vibrate but do not move freely.
This defines the structure and behavior of particles in the solid state.
Explain melting in terms of intermolecular forces.
Energy is used to overcome the attractive forces holding particles in place.
This process describes what happens to particles during melting.
Describe melting using the kinetic theory.
Particles gain energy, vibrate more, and eventually overcome fixed positions.
This explains the transition from solid to liquid.
Describe boiling using the kinetic theory.
Particles gain enough energy to escape into the gas phase.
This explains the transition from liquid to gas.
What is sublimation?
Solids transition directly to gas when particles gain enough energy to overcome all forces without becoming liquid.
This describes a phase change that skips the liquid state.
Interpret heating/cooling curves: What do flat sections represent?
Phase changes (temperature constant while energy breaks bonds).
This indicates that during phase changes, temperature does not change despite energy input.
Interpret heating/cooling curves: What do sloped sections represent?
Temperature changes (kinetic energy increases).
This indicates that during temperature changes, kinetic energy of particles is increasing.
