Thermodynamics Study Questions
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Questions and Answers

What are the three components of thermodynamical systems?

System, Surrounding, and Universe.

What are the three types of thermodynamical systems?

Open, Closed, and Isolated.

What two types of energy are involved in thermodynamics?

Internal energy and external energy.

What are the two fundamental concepts in thermodynamics?

<p>Heat and Work.</p> Signup and view all the answers

What is the first law of thermodynamics?

<p>Energy can neither be created nor destroyed, only transformed from one form to another.</p> Signup and view all the answers

What is heat capacity?

<p>The amount of heat required to raise the temperature of a substance by a specific amount.</p> Signup and view all the answers

What are the two forms of heat capacity?

<p>Molar heat capacity and specific heat capacity.</p> Signup and view all the answers

What are the two types of thermodynamic variables?

<p>Extensive and intensive.</p> Signup and view all the answers

What is a quasi-static process?

<p>A process that occurs slowly enough to be considered in equilibrium at all times.</p> Signup and view all the answers

What are the four types of thermodynamic processes?

<p>Isothermal, isobaric, isochoric, and adiabatic.</p> Signup and view all the answers

How does the work done in a thermodynamical system change depending on the process type?

<p>Work done in thermodynamical systems can vary depending on the process used. The work done is different for isothermal, isobaric, isochoric, and adiabatic processes.</p> Signup and view all the answers

What are the two types of thermodynamical processes?

<p>Reversible and irreversible.</p> Signup and view all the answers

Flashcards

System

The part of the universe that is being studied. It can be anything from a single atom to an entire galaxy.

Surrounding

Everything outside of the system that can interact with it. It can be the air around a balloon, the water in a beaker, or even the walls of a room.

Universe

The combination of the system and its surroundings. It represents everything that exists.

Open System

A system that can exchange both energy and matter with its surroundings.

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Closed System

A system that can exchange only energy with its surroundings.

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Isolated System

A system that cannot exchange either energy or matter with its surroundings. It is completely isolated from its surroundings.

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Internal Energy

The total energy of all the molecules within a system. It includes kinetic energy (motion) and potential energy (position) of the molecules.

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External Energy

The energy that a system possesses due to its interaction with its surroundings. Examples include gravitational potential energy, mechanical energy, and electrical energy.

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Heat

The transfer of thermal energy between objects at different temperatures. It flows from a hotter object to a colder object until they reach thermal equilibrium.

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Work

Energy transfer that occurs when a force acts over a distance. It can be done by a system or on a system.

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1st Law of Thermodynamics

The total energy of a closed system remains constant; energy can be transferred but cannot be created or destroyed.

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Heat Capacity

The amount of heat energy required to raise the temperature of a substance by one degree.

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Molar Heat Capacity

The amount of heat energy required to raise the temperature of one mole of a substance by one degree.

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Specific Heat Capacity

The amount of heat energy required to raise the temperature of one gram of a substance by one degree.

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Extensive Variables

Variables that depend on the size or amount of the system. Examples include volume, mass, and energy.

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Intensive Variables

Variables that are independent of the size or amount of the system. Examples include temperature, pressure, and density.

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Quasi-Static Process

A thermodynamic process that happens slowly enough that the system is always in equilibrium.

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Isothermal Process

A thermodynamic process that occurs at constant temperature.

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Isobaric Process

A thermodynamic process that occurs at constant pressure.

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Isochoric Process

A thermodynamic process that occurs at constant volume.

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Adiabatic Process

A thermodynamic process that occurs without any exchange of heat with the surroundings.

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Reversible Process

A thermodynamic process that can be reversed without leaving any change in the system or surroundings.

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Irreversible Process

A thermodynamic process that cannot be reversed completely. It always results in a net increase in entropy in the universe.

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Study Notes

Thermodynamics Study Questions

  • Q.01: Define system, surroundings, and the universe.
  • Q.02: Differentiate between open, closed, and isolated systems.
  • Q.03: Explain internal energy and external energy.
  • Q.04: Define heat and work.
  • Q.05: State the first law of thermodynamics.
  • Q.06: Define heat capacity.
  • Q.07: Distinguish between molar heat capacity and specific heat capacity.
  • Q.08: Explain intensive and extensive variables.
  • Q.09: Define a quasi-static process.
  • Q.10: Define isothermal, isobaric, isochoric, and adiabatic processes.
  • Q.11: Write equations for work done in isothermal, isobaric, isochoric, and adiabatic processes.
  • Q.12: Differentiate between reversible and irreversible processes.

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Test your understanding of thermodynamics concepts with these study questions. This quiz covers key definitions, laws, and processes in thermodynamics, including different types of systems and thermodynamic properties. Enhance your grasp on the subject as you prepare for exams or deeper studies.

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