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Questions and Answers
What term describes the sum of kinetic and potential energy of a substance?
What term describes the sum of kinetic and potential energy of a substance?
Which principle describes that two bodies in thermal equilibrium with a third body are also in equilibrium with each other?
Which principle describes that two bodies in thermal equilibrium with a third body are also in equilibrium with each other?
What is the correct unit of measurement for temperature in thermodynamics?
What is the correct unit of measurement for temperature in thermodynamics?
According to the equipartition theorem, how is energy distributed among the degrees of freedom of a system?
According to the equipartition theorem, how is energy distributed among the degrees of freedom of a system?
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What does the first law of thermodynamics express in equation form?
What does the first law of thermodynamics express in equation form?
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In the context of kinetic theory, what is assumed about the motion of gas molecules?
In the context of kinetic theory, what is assumed about the motion of gas molecules?
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What characterizes an ideal gas according to thermodynamics?
What characterizes an ideal gas according to thermodynamics?
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Which type of thermometer uses gas to measure temperature?
Which type of thermometer uses gas to measure temperature?
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Study Notes
Thermal Physics/Heat and Thermodynamics
- This is a course on thermal physics, heat, and thermodynamics.
- It's part of Engineering Physics (PHY 101).
Thermodynamic Concepts
- Thermodynamic System: A portion of the material universe isolated for study of changes, often composed of smaller systems.
- Surroundings: The rest of the universe outside the system.
-
Boundary: The "wall" separating the system from its surroundings. The boundary may or may not allow heat and matter to exchange.
- Open System: Allows exchange of both heat and matter. Example: human digestive system.
- Closed System: Allows exchange of heat only with surroundings, no matter exchange. Example: refrigerator, enclosed gas.
- Isolated System: Thermally insulated. No heat exchange with surroundings. Example: thermos flask.
- Adiabatic Changes: Changes in an isolated system.
- Diathermal Wall: Allows heat exchange between system and surroundings. Example: metallic walls.
- Adiabatic/Adiathermal Wall: Does not allow heat exchange. Example: vacuum flask walls.
Internal Energy
- Defined as the total kinetic energy and potential energy of particles in a substance.
- Dependent on temperature.
Heat
- Transfer of energy due to temperature difference.
- Usually involves energy transfer from higher to lower temperatures.
Ideal Gas
- Theoretical gas of point particles with no interparticle interactions.
- Described by the Ideal Gas Law: PV = nRT
- P = Pressure
- V = Volume
- n = Number of moles
- R = Gas constant (8.314 JK⁻¹mol⁻¹)
- T = Temperature
Temperature
- Degree of hotness or coldness.
- Measured in Kelvin (K).
- Measured using thermometers.
- Types of Thermometers:
- Constant-volume gas thermometers
- Resistance thermometers
- Mercury-in-glass thermometers
- Electric thermometers
- Thermocouples
- Types of Thermometers:
Zeroth Law of Thermodynamics
- If two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.
- Based on temperature measurement.
First Law of Thermodynamics
- Change in internal energy (∆U) equals heat added (Q) minus work done (W) by the system.
- ∆U = Q - W
- dQ = dU + dW, where dW = P dV (pressure-volume work)
Thermodynamic Processes
- Isothermal: Constant temperature. ( a -> b )
- Isobaric: Constant pressure. ( d -> b )
- Isochoric: Constant volume. ( a -> d )
- Adiabatic: No heat exchange.
Work done in various processes
- Isothermal: Work calculated using PV = nRT and W = nRT ln(V2/V1)
- Isochoric: No work done as volume remains constant ( dV = 0).
- Isobaric: Work done is calculated as W = P ∆V.
Kinetic Theory of Gases
- Explains gas behavior in terms of molecular motion.
- Assumptions: molecules are points and occupy negligible volume; no intermolecular forces except during collision; collisions are perfectly elastic; and duration of collision is negligible compared to time between collisions.
Equipartition Theorem
- Energy shared equally among all accessible degrees of freedom.
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Description
Test your understanding of thermal physics and thermodynamics concepts covered in Engineering Physics (PHY 101). This quiz will challenge your knowledge on thermodynamic systems, surroundings, and boundaries. Prepare to explore open, closed, and isolated systems, as well as adiabatic changes and heat exchange methods.
