Thermal Physics

Question 1

Flashcard 1
Q: What are the distinguishing properties of solids?

Answer 1

A: Solids have a fixed shape and volume, with particles closely packed in a regular arrangement.

Question 2

Flashcard 2
Q: What are the distinguishing properties of liquids?

Answer 2

A: Liquids have a fixed volume but can change shape to fit their container, with particles loosely arranged and able to flow.

Question 3

Flashcard 3
Q: What are the distinguishing properties of gases?

Answer 3

A: Gases have neither a fixed shape nor volume, with particles widely spaced and moving freely.

Question 4

Flashcard 4
Q: What are the terms for the changes in state between solids, liquids, and gases?

Answer 4

A: Melting (solid to liquid), freezing (liquid to solid), evaporation (liquid to gas), and condensation (gas to liquid).

Question 5

Flashcard 4
Q: What are the terms for the changes in state between solids, liquids, and gases?

Answer 5

A: Melting (solid to liquid), freezing (liquid to solid), evaporation (liquid to gas), and condensation (gas to liquid).

Question 6

Flashcard 5
Q: How are particles arranged and separated in solids?

Answer 6

A: Particles in solids are closely packed in a fixed, regular structure.

Question 7

Flashcard 6
Q: How are particles arranged and separated in liquids?

Answer 7

A: Particles in liquids are close together but can move around, allowing the liquid to flow.

Question 8

Flashcard 7
Q: How are particles arranged and separated in gases?

Answer 8

A: Particles in gases are far apart and move freely in all directions.

Question 9

Flashcard 8
Q: What is the relationship between particle motion and temperature?

Answer 9

A: Higher temperatures increase particle motion, while at absolute zero (-273°C), particles have minimal kinetic energy.

Question 10

Flashcard 9
Q: How does particle collision create pressure in gases?

Answer 10

A: Pressure is created by particles colliding with surfaces, exerting force per unit area.

Question 11

Flashcard 10
Q: What evidence supports the kinetic particle model of matter?

Answer 11

A: The random motion of microscopic particles in a suspension, known as Brownian motion, supports the kinetic model.

Question 12

Flashcard 11
Q: How do forces and distances between particles affect the properties of solids, liquids, and gases?

Answer 12

A: Strong forces and close distances result in solid structures, while weaker forces and greater distances characterize liquids and gases.

Question 13

Flashcard 12
Q: What happens to gas pressure when temperature increases at constant volume?

Answer 13

A: Gas pressure increases as particles move faster and collide more frequently with surfaces.

Question 14

Flashcard 13
Q: What happens to gas pressure when the volume increases at constant temperature?

Answer 14

A: Gas pressure decreases as particles have more space and collide less frequently with surfaces.

Question 15

Flashcard 14
Q: How do you convert Celsius to Kelvin?

Answer 15

A: T (K) = θ (°C) + 273.

Question 16

Flashcard 15
Q: What is the equation for a fixed mass of gas at constant temperature?

Answer 16

A: pV = constant.

Question 17

Flashcard 16
Q: Describe thermal expansion in solids, liquids, and gases.

Answer 17

A: Solids, liquids, and gases expand when heated, with gases expanding the most and solids the least.

Question 18

Flashcard 17
Q: What are some everyday applications of thermal expansion?

Answer 18

A: Gaps in bridges, thermometer function, and bimetallic strips in thermostats.

Question 19

Flashcard 18
Q: What is specific heat capacity?

Answer 19

A: The energy required per unit mass to increase the temperature of a substance by one degree Celsius.

Question 20

Flashcard 19
Q: What is the equation for specific heat capacity?

Answer 20

A: c = ∆E / (m∆θ).

Question 21

Flashcard 20
Q: What occurs during melting and boiling in terms of energy?

Answer 21

A: Energy is added to overcome attractive forces between particles, causing a change of state without a temperature increase.

Question 22

Flashcard 21
Q: What are the melting and boiling points of water at standard atmospheric pressure?

Answer 22

A: Melting point: 0°C, Boiling point: 100°C.

Question 23

Flashcard 22
Q: What is evaporation?

Answer 23

A: Evaporation is the escape of higher-energy particles from the surface of a liquid, causing cooling.

Question 24

Flashcard 23
Q: How does evaporation cause cooling?

Answer 24

A: As higher-energy particles escape, the average kinetic energy of remaining particles decreases, cooling the liquid.

Question 25

**Flashcard 24** **Q:** What is thermal conduction?

Answer 25

**A:** Thermal conduction is the transfer of heat through a material by atomic vibrations or, in metals, by free electron movement. ---

Question 26

**Flashcard 25** **Q:** Why is thermal conduction poor in gases?

Answer 26

**A:** In gases, particles are far apart, reducing the frequency of particle collisions, which makes heat transfer inefficient. ---

Question 27

**Flashcard 26** **Q:** What is convection?

Answer 27

**A:** Convection is the transfer of heat in fluids (liquids and gases) due to density changes when the fluid is heated and moves. ---

Question 28

**Flashcard 27** **Q:** What is thermal radiation?

Answer 28

**A:** Thermal radiation is infrared radiation, which is emitted by all objects and does not require a medium to transfer heat. ---

Question 29

**Flashcard 28** **Q:** How do surface color and texture affect thermal radiation?

Answer 29

**A:** Black, dull surfaces are good emitters and absorbers of radiation, while shiny, white surfaces reflect radiation well. ---

Question 30

**Flashcard 29** **Q:** What factors affect the rate of evaporation?

Answer 30

**A:** Temperature, surface area, and air movement increase the rate of evaporation. ---

Question 31

**Flashcard 30** **Q:** What are some applications of conduction, convection, and radiation in everyday life?

Answer 31

**A:** Heating water in a kettle (conduction), cooking on a stove (conduction and radiation), and room heaters (convection).

Question 32

**Flashcard 31** **Q:** Describe the particle structure of a solid in terms of arrangement, separation, and motion.

Answer 32

**A:** Particles in solids are closely packed in a regular, fixed arrangement with very limited motion, primarily vibrating in place. ---

Question 33

**Flashcard 32** **Q:** Describe the particle structure of a liquid in terms of arrangement, separation, and motion.

Answer 33

**A:** Particles in liquids are close together but randomly arranged, with more freedom to move around and slide past each other. ---

Question 34

**Flashcard 33** **Q:** Describe the particle structure of a gas in terms of arrangement, separation, and motion.

Answer 34

**A:** Particles in gases are far apart, randomly arranged, and move freely and rapidly in all directions. ---

Question 35

**Flashcard 34** **Q:** What is absolute zero, and why is it significant?

Answer 35

**A:** Absolute zero (-273°C or 0 K) is the lowest possible temperature, where particles have minimal kinetic energy and virtually no movement. ---

Question 36

**Flashcard 35** **Q:** What is Brownian motion, and how does it provide evidence for the kinetic model of matter?

Answer 36

**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. ---

Question 37

**Flashcard 36** **Q:** How does particle motion relate to the pressure of a gas?

Answer 37

**A:** Increased particle motion leads to more frequent and forceful collisions with container walls, raising the gas pressure. ---

Question 38

**Flashcard 37** **Q:** What factors increase the rate of thermal expansion in materials?

Answer 38

**A:** Higher temperature increases particle motion, causing solids, liquids, and gases to expand, with gases expanding the most due to weaker intermolecular forces. ---

Question 39

**Flashcard 38** **Q:** How does temperature affect the motion of particles in a substance?

Answer 39

**A:** As temperature rises, particles gain kinetic energy and move faster, leading to expansion and increased pressure in gases. ---

Question 40

**Flashcard 39** **Q:** Explain the term "specific heat capacity."

Answer 40

**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). ---

Question 41

**Flashcard 40** **Q:** What experiment could be used to measure the specific heat capacity of a solid?

Answer 41

*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. ---

Question 42

**Flashcard 41** **Q:** How does the kinetic energy of particles relate to the temperature of an object?

Answer 42

**A:** Higher temperature means higher average kinetic energy of the particles in an object. ---

Question 43

**Flashcard 42** **Q:** Describe boiling in terms of energy input.

Answer 43

**A:** During boiling, energy is added to overcome intermolecular forces without increasing temperature until the entire substance has changed to gas. ---

Question 44

**Flashcard 43** **Q:** What is the main difference between boiling and evaporation?

Answer 44

**A:** Boiling occurs throughout the liquid at a specific temperature, while evaporation only occurs at the surface of the liquid at any temperature. ---

Question 45

**Flashcard 44** **Q:** How does surface area affect the rate of evaporation?

Answer 45

**A:** A larger surface area allows more particles to escape, increasing the rate of evaporation. ---

Question 46

**Flashcard 45** **Q:** Explain why objects cool down when in contact with an evaporating liquid.

Answer 46

**A:** As more energetic particles leave the liquid, the average energy (and temperature) of the remaining particles decreases, cooling the liquid. ---

Question 47

**Flashcard 46** **Q:** What is conduction and why does it occur more easily in metals?

Answer 47

**A:** Conduction is the transfer of thermal energy through direct particle contact; metals conduct better due to free-moving electrons that transfer energy quickly. ---

Question 48

**Flashcard 46** **Q:** What is conduction and why does it occur more easily in metals?

Answer 48

**A:** Conduction is the transfer of thermal energy through direct particle contact; metals conduct better due to free-moving electrons that transfer energy quickly. ---

Question 49

**Flashcard 47** **Q:** Why is convection an important method of heat transfer in fluids?

Answer 49

**A:** Convection occurs as warmer, less dense fluid rises, while cooler, denser fluid sinks, creating a cycle that efficiently transfers heat through the fluid. ---

Question 50

**Flashcard 48** **Q:** What factors influence thermal radiation emission and absorption in objects?

Answer 50

**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. ---

Question 51

**Flashcard 49** **Q:** What is the role of infrared radiation in thermal energy transfer?

Answer 51

**A:** Infrared radiation transfers heat between objects without needing a medium, allowing heat to travel through a vacuum (like sunlight reaching Earth). ---

Question 52

**Flashcard 50** **Q:** How does a car radiator use conduction, convection, and radiation to keep an engine cool?

Answer 52

**A:** The radiator absorbs engine heat (conduction), transfers it to the coolant (convection), and releases heat into the air via radiation and convection.

Question 53

**Flashcard 51** **Q:** State Boyle's Law.

Answer 53

**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, \( p \times V = \text{constant} \). ---

Question 54

**Flashcard 52** **Q:** Describe a practical example of Boyle's Law.

Answer 54

**A:** When a syringe is compressed, the gas inside decreases in volume, causing the pressure to increase if temperature remains constant. ---

Question 55

**Flashcard 53** **Q:** State Charles' Law.

Answer 55

**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 \( \frac{V}{T} = \text{constant} \). ---

Question 56

**Flashcard 53** **Q:** State Charles' Law.

Answer 56

**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 \( \frac{V}{T} = \text{constant} \). ---

Question 57

**Flashcard 54** **Q:** How does Charles' Law explain why a balloon expands when heated?

Answer 57

**A:** As temperature increases, the volume of gas in the balloon increases at constant pressure, causing it to expand. ---

Question 58

**Flashcard 55** **Q:** What is the relationship between Celsius and Kelvin temperatures?

Answer 58

**A:** To convert from Celsius to Kelvin, add 273: \( T(\text{K}) = \theta (\text{°C}) + 273 \). ---

Question 59

**Flashcard 56** **Q:** Explain the pressure-temperature relationship in a gas at constant volume.

Answer 59

**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). ---

Question 60

**Flashcard 57** **Q:** What is the equation \( pV = \text{constant} \) used for?

Answer 60

**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). ---

Question 61

**Flashcard 58** **Q:** What happens to gas pressure if the volume of a container is halved at constant temperature?

Answer 61

**A:** The gas pressure doubles, as pressure and volume are inversely related according to Boyle’s Law. ---

Question 62

**Flashcard 59** **Q:** Describe the absolute zero temperature in terms of particle motion.

Answer 62

**A:** At absolute zero (-273°C or 0 K), particles have minimum kinetic energy and virtually no motion. ---