Thermal Physics Flashcards
Flashcard 1
Q: What are the distinguishing properties of solids?
A: Solids have a fixed shape and volume, with particles closely packed in a regular arrangement.
Flashcard 2
Q: What are the distinguishing properties of liquids?
A: Liquids have a fixed volume but can change shape to fit their container, with particles loosely arranged and able to flow.
Flashcard 3
Q: What are the distinguishing properties of gases?
A: Gases have neither a fixed shape nor volume, with particles widely spaced and moving freely.
Flashcard 4
Q: What are the terms for the changes in state between solids, liquids, and gases?
A: Melting (solid to liquid), freezing (liquid to solid), evaporation (liquid to gas), and condensation (gas to liquid).
Flashcard 4
Q: What are the terms for the changes in state between solids, liquids, and gases?
A: Melting (solid to liquid), freezing (liquid to solid), evaporation (liquid to gas), and condensation (gas to liquid).
Flashcard 5
Q: How are particles arranged and separated in solids?
A: Particles in solids are closely packed in a fixed, regular structure.
Flashcard 6
Q: How are particles arranged and separated in liquids?
A: Particles in liquids are close together but can move around, allowing the liquid to flow.
Flashcard 7
Q: How are particles arranged and separated in gases?
A: Particles in gases are far apart and move freely in all directions.
Flashcard 8
Q: What is the relationship between particle motion and temperature?
A: Higher temperatures increase particle motion, while at absolute zero (-273°C), particles have minimal kinetic energy.
Flashcard 9
Q: How does particle collision create pressure in gases?
A: Pressure is created by particles colliding with surfaces, exerting force per unit area.
Flashcard 10
Q: What evidence supports the kinetic particle model of matter?
A: The random motion of microscopic particles in a suspension, known as Brownian motion, supports the kinetic model.
Flashcard 11
Q: How do forces and distances between particles affect the properties of solids, liquids, and gases?
A: Strong forces and close distances result in solid structures, while weaker forces and greater distances characterize liquids and gases.
Flashcard 12
Q: What happens to gas pressure when temperature increases at constant volume?
A: Gas pressure increases as particles move faster and collide more frequently with surfaces.
Flashcard 13
Q: What happens to gas pressure when the volume increases at constant temperature?
A: Gas pressure decreases as particles have more space and collide less frequently with surfaces.
Flashcard 14
Q: How do you convert Celsius to Kelvin?
A: T (K) = θ (°C) + 273.
Flashcard 15
Q: What is the equation for a fixed mass of gas at constant temperature?
A: pV = constant.
Flashcard 16
Q: Describe thermal expansion in solids, liquids, and gases.
A: Solids, liquids, and gases expand when heated, with gases expanding the most and solids the least.
Flashcard 17
Q: What are some everyday applications of thermal expansion?
A: Gaps in bridges, thermometer function, and bimetallic strips in thermostats.
Flashcard 18
Q: What is specific heat capacity?
A: The energy required per unit mass to increase the temperature of a substance by one degree Celsius.
Flashcard 19
Q: What is the equation for specific heat capacity?
A: c = ∆E / (m∆θ).
Flashcard 20
Q: What occurs during melting and boiling in terms of energy?
A: Energy is added to overcome attractive forces between particles, causing a change of state without a temperature increase.
Flashcard 21
Q: What are the melting and boiling points of water at standard atmospheric pressure?
A: Melting point: 0°C, Boiling point: 100°C.
Flashcard 22
Q: What is evaporation?
A: Evaporation is the escape of higher-energy particles from the surface of a liquid, causing cooling.
Flashcard 23
Q: How does evaporation cause cooling?
A: As higher-energy particles escape, the average kinetic energy of remaining particles decreases, cooling the liquid.
Flashcard 24
Q: What is thermal conduction?
A: Thermal conduction is the transfer of heat through a material by atomic vibrations or, in metals, by free electron movement.
Flashcard 25
Q: Why is thermal conduction poor in gases?
A: In gases, particles are far apart, reducing the frequency of particle collisions, which makes heat transfer inefficient.
Flashcard 26
Q: What is convection?
A: Convection is the transfer of heat in fluids (liquids and gases) due to density changes when the fluid is heated and moves.
Flashcard 27
Q: What is thermal radiation?
A: Thermal radiation is infrared radiation, which is emitted by all objects and does not require a medium to transfer heat.
Flashcard 28
Q: How do surface color and texture affect thermal radiation?
A: Black, dull surfaces are good emitters and absorbers of radiation, while shiny, white surfaces reflect radiation well.
Flashcard 29
Q: What factors affect the rate of evaporation?
A: Temperature, surface area, and air movement increase the rate of evaporation.
Flashcard 30
Q: What are some applications of conduction, convection, and radiation in everyday life?
A: Heating water in a kettle (conduction), cooking on a stove (conduction and radiation), and room heaters (convection).
Flashcard 31
Q: Describe the particle structure of a solid in terms of arrangement, separation, and motion.
A: Particles in solids are closely packed in a regular, fixed arrangement with very limited motion, primarily vibrating in place.
Flashcard 32
Q: Describe the particle structure of a liquid in terms of arrangement, separation, and motion.
A: Particles in liquids are close together but randomly arranged, with more freedom to move around and slide past each other.
Flashcard 33
Q: Describe the particle structure of a gas in terms of arrangement, separation, and motion.
A: Particles in gases are far apart, randomly arranged, and move freely and rapidly in all directions.
Flashcard 34
Q: What is absolute zero, and why is it significant?
A: Absolute zero (-273°C or 0 K) is the lowest possible temperature, where particles have minimal kinetic energy and virtually no movement.
Flashcard 35
Q: What is Brownian motion, and how does it provide evidence for the kinetic model of matter?
A: Brownian motion is the random movement of microscopic particles in a fluid, caused by collisions with fast-moving molecules, demonstrating particle movement in gases and liquids.
Flashcard 36
Q: How does particle motion relate to the pressure of a gas?
A: Increased particle motion leads to more frequent and forceful collisions with container walls, raising the gas pressure.
Flashcard 37
Q: What factors increase the rate of thermal expansion in materials?
A: Higher temperature increases particle motion, causing solids, liquids, and gases to expand, with gases expanding the most due to weaker intermolecular forces.
Flashcard 38
Q: How does temperature affect the motion of particles in a substance?
A: As temperature rises, particles gain kinetic energy and move faster, leading to expansion and increased pressure in gases.
Flashcard 39
Q: Explain the term “specific heat capacity.”
A: Specific heat capacity is the energy required to raise the temperature of 1 kg of a substance by 1°C, measured in J/(kg°C).
Flashcard 40
Q: What experiment could be used to measure the specific heat capacity of a solid?
*A:** Heat the solid and measure its temperature rise over time, using known values for mass, energy supplied, and the temperature change to calculate specific heat capacity.
Flashcard 41
Q: How does the kinetic energy of particles relate to the temperature of an object?
A: Higher temperature means higher average kinetic energy of the particles in an object.
Flashcard 42
Q: Describe boiling in terms of energy input.
A: During boiling, energy is added to overcome intermolecular forces without increasing temperature until the entire substance has changed to gas.
Flashcard 43
Q: What is the main difference between boiling and evaporation?
A: Boiling occurs throughout the liquid at a specific temperature, while evaporation only occurs at the surface of the liquid at any temperature.
Flashcard 44
Q: How does surface area affect the rate of evaporation?
A: A larger surface area allows more particles to escape, increasing the rate of evaporation.
Flashcard 45
Q: Explain why objects cool down when in contact with an evaporating liquid.
A: As more energetic particles leave the liquid, the average energy (and temperature) of the remaining particles decreases, cooling the liquid.
Flashcard 46
Q: What is conduction and why does it occur more easily in metals?
A: Conduction is the transfer of thermal energy through direct particle contact; metals conduct better due to free-moving electrons that transfer energy quickly.
Flashcard 46
Q: What is conduction and why does it occur more easily in metals?
A: Conduction is the transfer of thermal energy through direct particle contact; metals conduct better due to free-moving electrons that transfer energy quickly.
Flashcard 47
Q: Why is convection an important method of heat transfer in fluids?
A: Convection occurs as warmer, less dense fluid rises, while cooler, denser fluid sinks, creating a cycle that efficiently transfers heat through the fluid.
Flashcard 48
Q: What factors influence thermal radiation emission and absorption in objects?
A: Surface color (black absorbs/emits more, white reflects) and texture (dull surfaces absorb more than shiny ones) affect an object’s thermal radiation properties.
Flashcard 49
Q: What is the role of infrared radiation in thermal energy transfer?
A: Infrared radiation transfers heat between objects without needing a medium, allowing heat to travel through a vacuum (like sunlight reaching Earth).
Flashcard 50
Q: How does a car radiator use conduction, convection, and radiation to keep an engine cool?
A: The radiator absorbs engine heat (conduction), transfers it to the coolant (convection), and releases heat into the air via radiation and convection.
Flashcard 51
Q: State Boyle’s Law.
A: Boyle’s Law states that for a fixed mass of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. Mathematically, ( p \times V = \text{constant} ).
Flashcard 52
Q: Describe a practical example of Boyle’s Law.
A: When a syringe is compressed, the gas inside decreases in volume, causing the pressure to increase if temperature remains constant.
Flashcard 53
Q: State Charles’ Law.
A: Charles’ Law states that for a fixed mass of gas at constant pressure, the volume of the gas is directly proportional to its absolute temperature (measured in Kelvin). Mathematically, ( V \propto T ) or ( \frac{V}{T} = \text{constant} ).
Flashcard 53
Q: State Charles’ Law.
A: Charles’ Law states that for a fixed mass of gas at constant pressure, the volume of the gas is directly proportional to its absolute temperature (measured in Kelvin). Mathematically, ( V \propto T ) or ( \frac{V}{T} = \text{constant} ).
Flashcard 54
Q: How does Charles’ Law explain why a balloon expands when heated?
A: As temperature increases, the volume of gas in the balloon increases at constant pressure, causing it to expand.
Flashcard 55
Q: What is the relationship between Celsius and Kelvin temperatures?
A: To convert from Celsius to Kelvin, add 273: ( T(\text{K}) = \theta (\text{°C}) + 273 ).
Flashcard 56
Q: Explain the pressure-temperature relationship in a gas at constant volume.
A: When temperature increases, the particles move faster, increasing the pressure due to more frequent and forceful collisions with container walls (Gay-Lussac’s Law).
Flashcard 57
Q: What is the equation ( pV = \text{constant} ) used for?
A: This equation is used to calculate the relationship between pressure and volume in a fixed amount of gas at a constant temperature (Boyle’s Law).
Flashcard 58
Q: What happens to gas pressure if the volume of a container is halved at constant temperature?
A: The gas pressure doubles, as pressure and volume are inversely related according to Boyle’s Law.
Flashcard 59
Q: Describe the absolute zero temperature in terms of particle motion.
A: At absolute zero (-273°C or 0 K), particles have minimum kinetic energy and virtually no motion.
