Thermodynamics Concepts Quiz
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Questions and Answers

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.

    False (B)

    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______.

    <p>W</p> Signup and view all the answers

    Match the following processes with their characteristics:

    <p>Reversible Process = Can be retraced in the opposite direction Irreversible Process = Cannot be retraced Adiabatic Process = Occurs without heat exchange Dissipative Forces = Cause energy to be lost in a system</p> Signup and view all the answers

    What type of system allows for the exchange of both energy and matter?

    <p>Open System (D)</p> Signup and view all the answers

    An isolated system allows for the exchange of energy only.

    <p>False (B)</p> Signup and view all the answers

    What is defined as any part of the universe that is not a system?

    <p>surroundings</p> Signup and view all the answers

    In thermal equilibrium, the temperature of the two systems are __________.

    <p>equal</p> Signup and view all the answers

    Match the following types of systems with their definitions:

    <p>Open System = Exchange of energy and matter exists Closed System = Exchange of energy occurs, but not matter Isolated System = No exchange of energy or matter takes place Adiabatic System = Insulating wall that prevents heat transfer</p> Signup and view all the answers

    Which of the following best describes an adiabatic wall?

    <p>Does not allow heat to flow between systems. (C)</p> Signup and view all the answers

    The mean kinetic energy per molecule of a substance is directly proportional to its absolute temperature.

    <p>True (A)</p> Signup and view all the answers

    Give an example of a closed system.

    <p>A sealed container of gas.</p> Signup and view all the answers

    What does the Zeroth Law of Thermodynamics state?

    <p>Two systems are in thermal equilibrium through a third system if they are equal in temperature. (C)</p> Signup and view all the answers

    Thermodynamic state variables include pressure, volume, and temperature.

    <p>True (A)</p> Signup and view all the answers

    What is defined as the sum of kinetic and potential energies of the molecules in a system?

    <p>Internal energy</p> Signup and view all the answers

    In thermodynamic work, force is calculated using the formula F = P x ______.

    <p>A</p> Signup and view all the answers

    Match the following thermodynamic concepts with their definitions:

    <p>Thermal Equilibrium = Temperature is equal in systems. Adiabatic Wall = No heat flow between systems. Diathermic Wall = Allows heat flow between systems. Indicator Diagram = Graph representing thermodynamic process.</p> Signup and view all the answers

    Which of the following is NOT a thermodynamic state variable?

    <p>Distance (D)</p> Signup and view all the answers

    Heat flow can occur through adiabatic walls.

    <p>False (B)</p> Signup and view all the answers

    What is the formula to calculate work done (dW) when pressure exerted is P?

    <p>dW = P x dV</p> Signup and view all the answers

    What does the area under the indicator diagram in a thermodynamic process represent?

    <p>Work done during the process (B)</p> Signup and view all the answers

    In an isothermal process, the temperature of the system remains constant.

    <p>True (A)</p> Signup and view all the answers

    What is the equation used to express the First Law of Thermodynamics?

    <p>ΔQ = ΔU + ΔW</p> Signup and view all the answers

    In an adiabatic process, there is no heat flow between the system and the ______.

    <p>surroundings</p> Signup and view all the answers

    Which of the following statements is true for an adiabatic process?

    <p>Heat remains constant. (A)</p> Signup and view all the answers

    Match the thermodynamic processes with their characteristics:

    <p>Isothermal = Temperature remains constant throughout. Adiabatic = No heat exchange occurs. First Law of Thermodynamics = Conservation of energy principle. Indicator Diagram = Represents work done during a process.</p> Signup and view all the answers

    The walls of the container in an isothermal process must be perfectly conducting.

    <p>True (A)</p> Signup and view all the answers

    What must the specific heat ratio (γ) represent in the equation for adiabatic processes?

    <p>Cp/Cv</p> Signup and view all the answers

    Flashcards

    System (Thermodynamics)

    The portion of the universe enclosed by a boundary through which heat or energy can be exchanged.

    Surroundings (Thermodynamics)

    Any part of the universe that is not considered the 'system'.

    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

    A system that exchanges both heat and matter with its surroundings. Think of a pot of boiling water without a lid.

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    Closed System

    A system that allows only heat exchange, not matter.

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    Isolated System

    A system that doesn't exchange either heat or matter with its surroundings. Think of a sealed thermos flask.

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    Adiabatic Wall

    A wall that prevents heat from passing through, ensuring constant temperatures in both systems it separates.

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    Thermodynamics

    The branch of physics that studies the relationship between heat, temperature, work, and energy.

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    Diathermic Wall

    A wall that allows heat to flow between two systems.

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    Zeroth Law of Thermodynamics

    Two systems are in thermal equilibrium with each other if they are in thermal equilibrium with a third system individually.

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    Thermodynamic State Variable

    A macroscopic quantity that describes the thermodynamic state of a system, such as pressure, volume, temperature, or internal energy.

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    Internal Energy

    The total energy contained within a system due to the motion and interactions of its molecules.

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    Indicator Diagram

    A graph that represents a thermodynamic process by plotting pressure on the Y-axis and volume on the X-axis.

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    Work (in Thermodynamics)

    The work done on or by a system when it expands or contracts against an external pressure.

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    Isothermal Process

    A thermodynamic process where the temperature remains constant throughout. This means the system can exchange heat with the surroundings.

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    Adiabatic Process

    A thermodynamic process where there is no heat exchange between the system and its surroundings. This can happen if the process is fast or the container is well insulated.

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    First Law of Thermodynamics

    The change in internal energy of a system is equal to the heat supplied minus the work done by the system.

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    Specific Heat Ratio (γ)

    The ratio of the specific heat at constant pressure (Cp) to the specific heat at constant volume (Cv). It represents the relationship between heat capacity under different conditions.

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    Molar Heat Capacity at Constant Volume (Cv)

    The amount of energy required to raise the temperature of one mole of a substance by one degree Celsius at constant volume.

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    Molar Heat Capacity at Constant Pressure (Cp)

    The amount of energy required to raise the temperature of one mole of a substance by one degree Celsius at constant pressure.

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    Difference between Cp and Cv

    The difference between the molar heat capacity at constant pressure (Cp) and the molar heat capacity at constant volume (Cv). It's related to the work done during expansion.

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    Adiabatic Expansion

    The internal energy of a system decreases during an adiabatic expansion, leading to a drop in temperature.

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    Reversible Process

    A process that can be reversed in reverse, returning the system and surroundings to their original states.

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    Irreversible Process

    A process that cannot be fully reversed, leaving the system or surroundings in a different state.

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    Kelvin-Planck Statement (Second Law of Thermodynamics)

    It's impossible to continuously extract work from a system by cooling it below its surroundings' temperature.

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    Clausius Statement (Second Law of Thermodynamics)

    It's impossible for a machine to transfer heat from a colder body to a hotter body without external work.

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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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    Thermodynamics Past Paper PDF MES Indian School, Doha, Qatar 2023-2024

    Description

    Test your understanding of key thermodynamic principles including adiabatic processes, system types, and the laws governing energy transfer. This quiz covers fundamental concepts and definitions necessary for mastering thermodynamics. Get ready to challenge your knowledge with a range of questions on these crucial topics.

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