2B1 Temperature, Heating, and Thermal Energy Flashcards

Describe the differences, functions, and applications of temperature, heating, and thermal energy. (50 cards)

1
Q

Define:

Heat

A

Energy transferred due to a temperature difference.

Heat is energy in transit from a body of higher temperature to a body of lower temperature.

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2
Q

Fill in the blank:

Temperature is a measure of the average ______ energy of particles in a substance.

A

kinetic

Temperature is a way to describe warmth and coldness using quantitative descriptors.

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3
Q

True or False:

Heat and temperature are the same physical quantity.

A

False

Temperature measures average kinetic energy, while heat refers to energy transferred due to temperature difference.

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4
Q

Fill in the blank:

A ______ is an instrument used to measure temperature.

A

thermometer

Thermometers can be analog (mercury or alcohol-based) or digital, depending on the application.

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5
Q

How does temperature affect the speed of particles in a substance?”

A

Higher temperature corresponds to faster particle motion.

The motion includes translational, rotational, and vibrational movements.

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6
Q

Define:

Absolute zero

A

The lowest possible temperature (0 K) where there is no kinetic energy or motion in a system of particles.

In Celsius, absolute zero is -273.15 degrees. In Fahrenheit, -459.67 degrees.

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7
Q

Relate temperature and the state of matter.

A

Higher temperatures increase particle motion, which can cause changes in state (e.g., solid to liquid).

Phase changes occur when the average kinetic energy overcomes intermolecular forces. Examples include melting (solid to liquid) and evaporation (liquid to gas).

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8
Q

Define:

Thermal expansion

A

Increase in material size as temperature rises.

It occurs because particles move faster and spread apart as they gain energy. Examples include thermometers, where a higher temperature causes the liquid inside to rise, indicating a fever.

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9
Q

True or false:

All materials expand at the same rate when heated.

A

False

The rate of expansion depends on the material’s thermal expansion coefficient. For example, metals expand more than ceramics.

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10
Q

What factors affect the heat needed to change a substance’s temperature?

A
  • Temperature difference
  • Mass of the substance
  • Nature of the substance

These factors determine the heat capacity and specific heat capacity of a substance. Water has high specific heat, meaning it heats up & cools down slowly.

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11
Q

Define:

Thermal energy

A

The total internal energy associated with the motion of the particles (atoms and molecules) in an object or substance.

An example is using thermal energy from a steam engine to move a piston.

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12
Q

Why does a swimming pool at the same temperature as a cup of coffee have more thermal energy?

A

The pool has more thermal energy because it contains a larger number of particles.

Thermal energy depends on both temperature and particle count.

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13
Q

Fill in the blank:

Thermal energy is the total energy of particles, while temperature measures their ______ energy.

A

average kinetic

Thermal energy accounts for both kinetic and potential energy, but temperature only measures average kinetic energy.

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14
Q

True or false:

Adding heat always increases a substance’s temperature.

A

False

Heat can also cause a phase change without increasing temperature (e.g., melting ice). For example, Ice at 0°C absorbs heat but stays at 0°C until fully melted.

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15
Q

Define:

Phase transition

A

The process by which a substance changes from one state of matter (solid, liquid, gas) to another due to energy transfer.

Examples include melting, freezing, vaporization, and condensation, often occurring at specific temperatures and pressures.

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16
Q

Explain how heating is related to temperature and thermal energy.

A

Heating transfers energy to increase a substance’s thermal energy, which may raise its temperature or cause a phase change.

Heating occurs via conduction, convection, or radiation.

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17
Q

How are thermal energy, temperature, and particle count related?

A

Thermal energy increases with higher temperature and more particles.

Larger objects can have more thermal energy even at the same temperature.

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18
Q

What does the kinetic molecular theory state about the motion of particles in matter?

A

All particles of matter are in constant motion and their speed increases with temperature.

This motion explains energy transfer during heating and cooling.

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19
Q

Explain how temperature is related to the kinetic energy of particles.

A

Temperature is directly proportional to the average kinetic energy of the particles in a substance.

Higher temperatures mean faster-moving particles with more kinetic energy, causing more collisions and greater expansion.

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20
Q

True or false:

A gas at the same temperature as a solid has particles with the same average kinetic energy.

A

True

State of matter doesn’t affect average kinetic energy. Temperature determines the average motion of particles.

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21
Q

Define:

Specific heat

A

The amount of thermal energy per unit mass required to increase the temperature by one degree Celsius.

Different substances have different specific heats based on their physical properties.

22
Q

True or false:

Latent heat changes a substance’s temperature during phase transitions.

A

False

Latent heat is the thermal energy released or absorbed during a phase change at constant temperature.

23
Q

What is the formula for calculating latent heat?

A

L = Q/m

Where L is latent heat (J/g), Q is heat added or removed (J), and m is mass (g).

24
Q

What is the latent heat of fusion?

A

It is the energy required to change a substance from a solid to a liquid at constant temperature.

This energy breaks the bonds between particles, enabling the phase transition at occurs at the melting point of a substance.

25
How does latent heat help in **ice pack injury treatment**?
The latent heat of fusion allows ice packs to **absorb heat** as the ice melts, reducing swelling by **extracting heat** from the injured area. ## Footnote The phase change from solid to liquid absorbs heat without increasing the temperature of the ice pack.
26
What is the **unit** of **latent heat**?
Joules per gram (**J/g**) or kilojoules per kilogram (**kJ/kg**). ## Footnote Other units include calories per gram and British thermal units.
27
Explain the difference between **specific heat** and **latent heat**.
Specific heat involves **temperature change**, while latent heat involves **phase changes** without temperature change. ## Footnote Both are measures of heat energy.
28
How does specific heat affect a **material’s ability to retain heat**?
Materials with high specific heat **retain heat longer** and resist temperature change. ## Footnote **Water is an example with high specific heat**, making it useful for thermal regulation.
29
# Define: Heat capacity
The **amount of heat energy required** to raise the temperature of a substance by one unit. ## Footnote It depends on the substance's mass and specific heat.
30
# Fill in the blank: **Heat capacity** is directly proportional to \_\_\_\_\_\_ and inversely proportional to \_\_\_\_\_\_.
mass; temperature change ## Footnote A larger mass requires more energy for the same temperature change, while a greater temperature change lowers heat capacity for a fixed energy input.
31
Which common substance has the **highest specific heat capacity**?
**Water** (4184 J/kg-K) ## Footnote Water's high specific heat capacity allows it to absorb a significant amount of heat, making it useful in various applications.
32
What is the **SI unit** of **heat capacity**?
Joules per Kelvin (J/K). ## Footnote This unit represents the ratio of heat supplied to the corresponding temperature change. The equation is C = Q / ΔT, or, heat divided by the temperature change.
33
Why is **water** used as a **coolant** in car engines?
Because of its **high specific heat capacity**, water can absorb and store large amounts of heat without a significant rise in temperature. ## Footnote This helps regulate engine temperature and prevent overheating.
34
# Fill in the blank: **Thermal energy storage** systems use materials with high \_\_\_\_\_\_ to store and release heat efficiently.
specific heat or latent heat ## Footnote Materials like molten salts or phase change materials (PCMs) are used in solar power plants and building insulation.
35
What are the three modes of **heat transfer**?
1. Conduction 2. Convection 3. Radiation ## Footnote Each mode describes a different mechanism by which heat can move through or out of a system.
36
# Define: Conduction
Mode of **energy transfer** that occurs by **direct contact** between particles. ## Footnote It occurs in solids, where particles vibrate to transfer energy. For instance, when you are walking on hot sand, the heat energy is conducted through direct contact with your feet.
37
# Fill in the blank: **Convection** transfers heat through the movement of particles within a \_\_\_\_\_\_.
fluid ## Footnote Warm fluid rises while cooler fluid sinks, creating convection currents.
38
How does **convection** work in boiling water?
**Hot** water **rises** while **cold** water **sinks**, creating a **cycle** that transfers heat throughout the pot. ## Footnote This process is known as thermal expansion.
39
# True or false: **Radiation** requires a medium to transfer heat.
False ## Footnote Radiation transfers heat through electromagnetic waves, even in a vacuum. An example is the sun's radiation warming the Earth.
40
How does radiation help **solar panels** generate electricity?
Solar panels absorb radiant energy from the sun and convert it into electrical energy using **photovoltaic cells**. ## Footnote Radiation is the transfer of energy through electromagnetic waves, which solar panels efficiently harness.
41
What are everyday examples of **conduction**, **convection**, and **radiation**?
* Conduction: Touching a hot pan. * Convection: Boiling water. * Radiation: Feeling warmth from sunlight. ## Footnote All three mechanisms transfer thermal energy but differ in process and medium.
42
What is the **difference** between *conduction* and *convection*?
* **Conduction** transfers heat through contact. * **Convection** uses the movement of fluids. ## Footnote Conduction is more common in solids and liquids.
43
What **units** are commonly used to **measure temperature**?
* Celsius * Fahrenheit * Kelvin ## Footnote Kelvin is used in scientific contexts, Celsius is common worldwide, and Fahrenheit is primarily used in the United States.
44
# Define: **Kelvin** temperature scale
Kelvin measures temperature starting from **absolute zero**, where particle motion stops. ## Footnote It is commonly used in scientific calculations.
45
What is the lowest temperature possible on the **Kelvin** scale?
0 K ## Footnote This temperature is known as absolute zero, where there is no molecular movement.
46
# Fill in the blank: 0°C corresponds to \_\_\_\_\_\_ **Kelvin**.
273.15 ## Footnote Kelvin = Celsius + 273.15
47
# True or false: The **Fahrenheit** scale is widely used in scientific contexts.
False ## Footnote Fahrenheit is used mainly in the U.S., while Celsius and Kelvin dominate in science.
48
Explain the **difference** between the *Celsius* and *Fahrenheit* scales.
* The **Celsius** scale is based on water’s freezing point (0°C) and boiling point (100°C). * The **Fahrenheit** scale uses 32°F and 212°F for the same. ## Footnote They are both relative scales, unlike Kelvin.
49
What are the **freezing and boiling points** of water in Celsius?
* Water's freezing point: 0°C * Water's boiling point: 100°C ## Footnote These values are standard measurements at normal atmospheric pressure.
50
Relate the **temperature scales** to real-world applications.
* Celsius: Meteorology. * Fahrenheit: U.S. weather reports. * Kelvin: Scientific research. ## Footnote Each scale suits specific contexts and practices.