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Questions and Answers
What is internal energy in the context of thermodynamics?
What is internal energy in the context of thermodynamics?
Internal energy is the sum of kinetic and potential energy of a substance, resulting from the motion of its particles.
Define temperature in thermodynamics.
Define temperature in thermodynamics.
Temperature is the degree of hotness or coldness of a body, measured on a scale such as Kelvin.
What does the Zeroth Law of Thermodynamics state?
What does the Zeroth Law of Thermodynamics state?
The Zeroth Law states that if body A is in thermal equilibrium with body B, and body A is also in thermal equilibrium with body C, then B and C are in thermal equilibrium with each other.
What is the equation representing the First Law of Thermodynamics?
What is the equation representing the First Law of Thermodynamics?
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How is work done by an ideal gas during expansion expressed mathematically?
How is work done by an ideal gas during expansion expressed mathematically?
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What does the equipartition theorem state?
What does the equipartition theorem state?
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Explain the kinetic theory of gases briefly.
Explain the kinetic theory of gases briefly.
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Name two types of thermometers and describe one.
Name two types of thermometers and describe one.
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Study Notes
Thermal Physics/Heat and Thermodynamics
- This subject covers heat and thermodynamics.
- It's part of Engineering Physics (PHY 101).
Thermodynamic Concepts
- Thermodynamic System: A portion of the material universe, isolated for study, to see how conditions change. Systems can be made up of smaller systems.
- Surroundings: The rest of the universe outside the system.
- Boundary: The "wall" separating the system from its surroundings.
- Open Systems: Exchange both heat and matter across the boundary (e.g., digestive system).
- Closed Systems: Only heat exchange across the boundary, no matter exchange (e.g., refrigerator).
- Isolated Systems: Thermally insulated, no heat communication with surroundings, but work can be done (e.g., thermos flask); adiabatic changes.
Isolated Systems
- A system that is thermally insulated and has no communication of heat; work can be done.
- Examples are thermos flasks. These exhibit adiabatic changes.
- The boundary separates the system from its surroundings, and its nature affects heat and matter exchange.
- A rigid boundary prevents changes in volume or shape, so no mechanical work occurs
Surroundings
- Refers to all of the universe outside the system being considered.
Diathermal Wall
- Allows heat exchange between the system and surroundings.
- Examples include metal walls.
- Two systems that are separated by a diathermal wall are said to be in thermal contact; heating one affects the other.
Adiabatic/Adiathermal Wall
- Does not allow heat exchange between the system and surroundings.
- Examples: walls of a vacuum flask.
- An isolated system is enclosed by an adiabatic wall.
Internal Energy
- Defined as the sum of kinetic and potential energy of a substance.
- Result of particle motion and interactions within the substance.
- Heat is the transfer of energy between objects with different temperatures.
Ideal Gas
- Theoretical gas comprised of many randomly moving point particles.
- Particles do not interact.
Equation of State for Ideal Gas
- Pressure (P) multiplied by Volume (V) equals moles (n) multiplied by the Ideal Gas Constant (R) and absolute Temperature (T).
- Note: the relationship is PV=nRT.
Temperature
- The degree of hotness or coldness of a body, measured using a scale.
- Measured in Kelvin (K).
Thermometers
- Devices for measuring temperature.
- Types include constant-volume gas, resistance, mercury-in-glass, electric, and thermocouple thermometers.
Zeroth Law
- If two systems are each in thermal equilibrium with a third, then they are in thermal equilibrium with each other.
- Based on temperature measurement.
First Law of Thermodynamics
- Change in internal energy equals heat added minus work done by the system.
- ΔU = Q - W.
Thermodynamic Processes
- Main processes like Isothermal, Isobaric, Isochoric, and Adiabatic.
Isothermal Process
- Occurs at a constant temperature (dT=0).
- Ideal gas law can be used to express the relationship.
Isobaric Process
- Occurs at a constant pressure (dP=0).
- Work done = P * (V2-V1).
Isochoric Process
- Occurs with constant volume (dV = 0).
- No work is done.
Adiabatic Process
- No heat exchange (dQ = 0).
- Internal energy change is equal to the negative of the work done.
Kinetic Theory of Gases
- Explains gas behavior in terms of molecular motion.
- Gases consist of numerous molecules, moving randomly at high speeds, interacting with container walls.
- Theory based on specific assumptions: negligible molecular volume, no intermolecular forces during collisions, perfectly elastic collisions, and negligible collision duration.
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Description
Test your knowledge on thermal physics concepts, specifically heat and thermodynamics as covered in Engineering Physics (PHY 101). This quiz will delve into thermodynamic systems, their boundaries, and the differences between open, closed, and isolated systems.
