Advanced Thermal Physics: Concepts and Principles

Physics

IB HL

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| By Thames

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1. 3.1.1 State that temperature determines the direction of thermal energy transfer between two objects.

The weight of the objects determines the direction of thermal energy transfer.

Temperature determines the direction of thermal energy transfer between two objects. Direction: hot->cold

The size of the objects determines the direction of thermal energy transfer.

The color of the objects determines the direction of thermal energy transfer.

Temperature is the determining factor for the direction of thermal energy transfer between two objects. Heat always flows from a hotter object to a colder object due to the difference in temperature.

Explanation

Temperature is the determining factor for the direction of thermal energy transfer between two objects. Heat always flows from a hotter object to a colder object due to the difference in temperature.

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About This Quiz

Explore key concepts of Thermal Physics as outlined in the 2009 IB Physics Higher Level curriculum. This assessment focuses on understanding heat transfer, thermodynamics, and related physical principles, essential for students aiming to excel in advanced physics studies.

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2. State the relation between the Kelvin and Celsius scales of temperature.

TK = TC +273.16

TK = TC / 100

TK = TC * 2

TK = TC - 273.16

The correct relation between the Kelvin and Celsius scales of temperature is TK = TC + 273.15. This is because the Kelvin scale starts at absolute zero (0K = -273.15°C), so to convert from Celsius to Kelvin, you add 273.15.

Explanation

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3. State the definition of internal energy of a substance.

Internal Energy is the total potential energy of the molecules of a substance.

Internal Energy is the total kinetic energy of the molecules of a substance.

Internal Energy is the energy required to change the state of a substance from solid to liquid.

Internal Energy is the potential energy and random kinetic energy of the molecule of a substanceInternal Energy = PE +... Internal Energy is the potential energy and random kinetic energy of the molecule of a substanceInternal Energy = PE + KE

The internal energy of a substance is the sum of potential energy and kinetic energy of its molecules, not just one or the other. This definition helps in understanding the concept of internal energy in thermodynamics.

Explanation

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4. 3.1.4 Explain and distinguish between macroscopic concepts of temperature internal energy and thermal energy (heat).

Temperature: rate of changeInternal Energy: rotational motion of moleculesThermal Energy: light energy transfer.

Temperature: measure of pressureInternal Energy: electromagnetic energyThermal Energy: flow of electricity.

Temperature: degree of hot/coldInternal Energy: PE + KE (molecules move)Thermal Energy: transfer of energy

Temperature: amount of energyInternal Energy: heat generatedThermal Energy: state of matter.

The correct answer distinguishes between temperature as the degree of hot/cold, internal energy as the sum of potential and kinetic energy of molecules in motion, and thermal energy as the transfer of energy. The incorrect answers provide inaccurate definitions and relationships between the concepts, leading to confusion or incorrect understanding.

Explanation

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5. Define the Avogadro constant.

Avogadro constant is the number of atoms or molecules in one mole of a substanceOR6.02 X 1023 particles

Avogadro constant is the speed of light in a vacuum.

Avogadro constant is the measure of acidity or basicity of a solution.

Avogadro constant is the gravitational constant in physics.

The Avogadro constant specifically refers to the number of atoms or molecules in one mole of a substance, which is 6.02 X 10^23 particles. It is a fundamental constant in chemistry and physics.

Explanation

The Avogadro constant specifically refers to the number of atoms or molecules in one mole of a substance, which is 6.02 X 10^23 particles. It is a fundamental constant in chemistry and physics.

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6. 3.2.3 Explain the physical differences between the solid, liquid, and gaseous phases in terms of molecular structure and particle motion.

Particle motion is the same in all three phases; only molecular structure differs.

Refer to the picture for details

The physical differences between solid, liquid, and gaseous phases are solely due to the size of the molecules involved.

Solid, liquid, and gaseous phases have identical molecular structures, with differences only in external appearance.

This question assesses understanding of the physical differences between solid, liquid, and gaseous phases in relation to molecular structure and particle motion. The correct answer emphasizes the need for visual reference to explain these concepts effectively, while the incorrect answers misinterpret or oversimplify the concept, leading to confusion or inaccuracy.

Explanation

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7. 3.2.4Explain the process of phase changes in terms of molecular behavior.

Phase changes occur randomly without any relation to energy inputs or molecular behavior.

(melting point)- When the solid is heated the particles of the solid vibrate at an increasing rate as the temperature... (melting point)- When the solid is heated the particles of the solid vibrate at an increasing rate as the temperature is increased- The vibrational KE of the particles increases- At melting point, the PE of the system increases as the particles move apart(boiling point)- Temperature between melting point and boiling point -> increases- At boiling point, particles gain energy to overcome intermolecular forces- PE increases- Heating continues until every particles change phase to gas

During the process of evaporation, particles lose energy instead of gaining energy to transition to a gaseous state.

In phase changes, the temperature always decreases as the state of matter changes.

The correct answer explains the process of phase changes in terms of molecular behavior focusing on the increasing energy input to overcome intermolecular forces. The incorrect answers provided do not align with the principles of phase changes and molecular behavior.

Explanation

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8. Explain why temperature does not change during a phase change in terms of molecular behavior.

Temperature decreases during a phase change due to the loss of energy between particles.

Temperature remains constant during a phase change because the heat is absorbed by the surroundings.

Temperature increases during a phase change as molecules speed up and collide more frequently.

During phase change, energy is continuously provided, but temperature does not increase because energy is used to break intermolecular forces... During phase change, energy is continuously provided, but temperature does not increase because energy is used to break intermolecular forces between particles. Instead of increasing average kinetic energy, the heat added transfers to increase in potential energy

During a phase change, the energy added is absorbed for breaking intermolecular forces and changing potential energy, rather than increasing kinetic energy which would result in a temperature change.

Explanation

During a phase change, the energy added is absorbed for breaking intermolecular forces and changing potential energy, rather than increasing kinetic energy which would result in a temperature change.

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9. Distinguish between evaporation and boiling.

Evaporation involves a decrease in temperature, while boiling involves an increase in temperature.

Water boils at 100? but evaporates at all temperatures. Evaporation happens when faster moving molecules escape of change from liquid... Water boils at 100? but evaporates at all temperatures. Evaporation happens when faster moving molecules escape of change from liquid to gas at the surface, so the average kinetic energy declines, and so temperature declines

Evaporation only occurs in hot temperatures, while boiling can happen at any temperature.

Boiling and evaporation are interchangeable terms referring to the same process of liquid turning into gas.

Evaporation and boiling are distinct processes in which molecules transition from liquid to gas, but they occur under different conditions and with different temperature changes.

Explanation

Evaporation and boiling are distinct processes in which molecules transition from liquid to gas, but they occur under different conditions and with different temperature changes.

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10. Define pressure.

Force per unit areaUnit: Nm-21atm = 1.013 X 105 Pa or 101.3kPa

The force per unit volume.

The temperature at which a substance changes from a liquid to a gas.

The amount of water vapor in the air.

Pressure is defined as the force per unit area exerted on a surface. It is typically measured in pascals (Pa) or kilopascals (kPa).

Explanation

Pressure is defined as the force per unit area exerted on a surface. It is typically measured in pascals (Pa) or kilopascals (kPa).

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11. State that temperature is a measure of the average random kinetic energy of the molecules of an ideal gas.

Temperature is a measure of the total energy of the molecules of an ideal gas.

Temperature is a measure of the pressure exerted by the molecules of an ideal gas.

Temperature is a measure of the volume occupied by the molecules of an ideal gas.

Temperature is a measure of the average kinetic energy per particles of an ideal gas

Temperature is a measure of the average kinetic energy per particle, not the total energy, volume, or pressure of the molecules in an ideal gas. Kinetic energy refers to the energy of motion possessed by particles.

Explanation

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12. 3.2.12 Explain the macroscopic behavior of an ideal gas in terms of a molecular model.

Ideal gases exhibit strong intermolecular forces

Refer to the picture for details

An ideal gas behaves like a solid at high temperatures

The molecular model of an ideal gas relates to its color

The macroscopic behavior of an ideal gas can be accurately predicted using a molecular model

The correct answer emphasizes the importance of referring to a specific picture or diagram to understand the macroscopic behavior of an ideal gas based on a molecular model. The incorrect answers provide common misconceptions or inaccurate statements related to ideal gases and molecular models.

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