Podcast
Questions and Answers
What occurs in an adiabatic expansion?
What occurs in an adiabatic expansion?
- Volume remains constant
- Internal energy decreases (correct)
- Temperature increases
- Internal energy increases
The Clausius statement of the second law of thermodynamics asserts that heat can spontaneously flow from a colder body to a hotter body.
The Clausius statement of the second law of thermodynamics asserts that heat can spontaneously flow from a colder body to a hotter body.
False (B)
What is a characteristic of a reversible process?
What is a characteristic of a reversible process?
It can be retraced in the opposite direction without dissipating energy.
In an adiabatic process, the change in internal energy ($
abla U$) is equal to the negative of the work done ($
abla W$). Thus, ΔU = -Δ______.
In an adiabatic process, the change in internal energy ($ abla U$) is equal to the negative of the work done ($ abla W$). Thus, ΔU = -Δ______.
Match the following processes with their characteristics:
Match the following processes with their characteristics:
What type of system allows for the exchange of both energy and matter?
What type of system allows for the exchange of both energy and matter?
An isolated system allows for the exchange of energy only.
An isolated system allows for the exchange of energy only.
What is defined as any part of the universe that is not a system?
What is defined as any part of the universe that is not a system?
In thermal equilibrium, the temperature of the two systems are __________.
In thermal equilibrium, the temperature of the two systems are __________.
Match the following types of systems with their definitions:
Match the following types of systems with their definitions:
Which of the following best describes an adiabatic wall?
Which of the following best describes an adiabatic wall?
The mean kinetic energy per molecule of a substance is directly proportional to its absolute temperature.
The mean kinetic energy per molecule of a substance is directly proportional to its absolute temperature.
Give an example of a closed system.
Give an example of a closed system.
What does the Zeroth Law of Thermodynamics state?
What does the Zeroth Law of Thermodynamics state?
Thermodynamic state variables include pressure, volume, and temperature.
Thermodynamic state variables include pressure, volume, and temperature.
What is defined as the sum of kinetic and potential energies of the molecules in a system?
What is defined as the sum of kinetic and potential energies of the molecules in a system?
In thermodynamic work, force is calculated using the formula F = P x ______.
In thermodynamic work, force is calculated using the formula F = P x ______.
Match the following thermodynamic concepts with their definitions:
Match the following thermodynamic concepts with their definitions:
Which of the following is NOT a thermodynamic state variable?
Which of the following is NOT a thermodynamic state variable?
Heat flow can occur through adiabatic walls.
Heat flow can occur through adiabatic walls.
What is the formula to calculate work done (dW) when pressure exerted is P?
What is the formula to calculate work done (dW) when pressure exerted is P?
What does the area under the indicator diagram in a thermodynamic process represent?
What does the area under the indicator diagram in a thermodynamic process represent?
In an isothermal process, the temperature of the system remains constant.
In an isothermal process, the temperature of the system remains constant.
What is the equation used to express the First Law of Thermodynamics?
What is the equation used to express the First Law of Thermodynamics?
In an adiabatic process, there is no heat flow between the system and the ______.
In an adiabatic process, there is no heat flow between the system and the ______.
Which of the following statements is true for an adiabatic process?
Which of the following statements is true for an adiabatic process?
Match the thermodynamic processes with their characteristics:
Match the thermodynamic processes with their characteristics:
The walls of the container in an isothermal process must be perfectly conducting.
The walls of the container in an isothermal process must be perfectly conducting.
What must the specific heat ratio (γ) represent in the equation for adiabatic processes?
What must the specific heat ratio (γ) represent in the equation for adiabatic processes?
Flashcards
System (Thermodynamics)
System (Thermodynamics)
The portion of the universe enclosed by a boundary through which heat or energy can be exchanged.
Surroundings (Thermodynamics)
Surroundings (Thermodynamics)
Any part of the universe that is not considered the 'system'.
Thermal Equilibrium
Thermal Equilibrium
The state where a system's macroscopic variables (pressure, volume, etc.) remain constant over time. This means the system's temperature is uniform.
Open System
Open System
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Closed System
Closed System
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Isolated System
Isolated System
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Adiabatic Wall
Adiabatic Wall
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Thermodynamics
Thermodynamics
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Diathermic Wall
Diathermic Wall
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Zeroth Law of Thermodynamics
Zeroth Law of Thermodynamics
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Thermodynamic State Variable
Thermodynamic State Variable
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Internal Energy
Internal Energy
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Indicator Diagram
Indicator Diagram
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Work (in Thermodynamics)
Work (in Thermodynamics)
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Isothermal Process
Isothermal Process
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Adiabatic Process
Adiabatic Process
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First Law of Thermodynamics
First Law of Thermodynamics
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Specific Heat Ratio (γ)
Specific Heat Ratio (γ)
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Molar Heat Capacity at Constant Volume (Cv)
Molar Heat Capacity at Constant Volume (Cv)
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Molar Heat Capacity at Constant Pressure (Cp)
Molar Heat Capacity at Constant Pressure (Cp)
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Difference between Cp and Cv
Difference between Cp and Cv
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Adiabatic Expansion
Adiabatic Expansion
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Reversible Process
Reversible Process
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Irreversible Process
Irreversible Process
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Kelvin-Planck Statement (Second Law of Thermodynamics)
Kelvin-Planck Statement (Second Law of Thermodynamics)
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Clausius Statement (Second Law of Thermodynamics)
Clausius Statement (Second Law of Thermodynamics)
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Study Notes
Thermodynamics
- Heat is a form of energy. Molecular kinetic energy is proportional to absolute temperature.
- Thermodynamics studies heat and temperature in relation to energy and work.
- System: A defined part of the universe enclosed by a boundary.
- Surroundings: The universe outside the system.
- Thermal equilibrium: Macroscopic system properties (pressure, volume, etc.) remain constant over time.
- System types
- Open system: Energy and matter exchange occurs. Example - water boiling in a pan without a lid
- Closed system: Only energy exchange occurs. Example – water boiling in a pan with a lid
- Isolated system: No energy or matter exchange occurs. Example – thermos flask
- Adiabatic wall: Insulating wall, preventing heat flow.
- Diathermic wall: Allows heat flow between systems.
- Zeroth Law of Thermodynamics: If two systems are each in thermal equilibrium with a third system, then the first two systems are in thermal equilibrium with each other.
- Thermodynamic state variables: Macroscopic quantities determining thermodynamic equilibrium. Examples include pressure, volume, temperature, mass, internal energy (U). These determine state of a system at a particular time.
Work
- Work is done when a body moves a certain distance in the direction of an applied force.
- Internal energy (U) is the sum of kinetic and potential energies of all molecules within a system.
First Law Of Thermodynamics
- Conservation of energy in thermodynamic systems. Heat energy supplied = change in internal energy + work done.
- Equation : ΔQ = ΔU + ΔW
- Symbols
- ΔQ: Change in heat supplied to the system
- ΔU:Change in internal energy of the system
- ΔW: Change in work done by/on the system
Isothermal Processes
- Thermodynamic processes where temperature remains constant throughout.
- Condition: System walls perfectly conducting, allowing heat exchange; Process is slow.
- Equation: PV = constant
Adiabatic Processes
- Processes where no heat exchange occurs between system and surroundings.
- Condition: System enclosed in perfectly non-conducting walls; Process is rapid.
- Equation: PV^γ = constant, where γ = Cp/Cv (ratio of specific heat capacities).
Reversible Processes
- Thermodynamic processes that can be reversed without causing any changes in surroundings.
- Conditions: Slow, no dissipative forces; System and surroundings maintain similar characteristics
- Examples: melting, boiling
Irreversible Processes
- Processes that cannot be reversed.
- Conditions: Fast, accompanied by dissipative forces (friction, turbulence)
- Examples: plastic deformation, combustion, diffusion.
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