Thermodynamics Chapter 12

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Questions and Answers

What is the branch of physics that deals with the concepts of heat and temperature, and the inter-conversion of heat and other forms of energy?

Thermodynamics

Thermodynamics is a microscopic science.

False (B)

What is the unit of molar specific heat capacity of a substance?

J mol-1 K-1

What are the two modes of energy transfer to a system?

<p>Heat and work</p> Signup and view all the answers

The term "equilibrium" in thermodynamics appears in what context?

<p>State of a system where the macroscopic variables don't change in time.</p> Signup and view all the answers

What is the difference between mechanics and thermodynamics?

<p>Mechanics is concerned with the motion of the system as a whole, while thermodynamics focuses on the internal macroscopic state of the body. (B)</p> Signup and view all the answers

The internal energy of a system depends on how that state was achieved.

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

Which of the following is NOT a thermodynamic state variable?

<p>Heat (C)</p> Signup and view all the answers

What is the first law of thermodynamics?

<p>The general law of conservation of energy applied to any system where energy transfer from or to the surroundings is taken into account.</p> Signup and view all the answers

What is the difference between specific heat capacity and molar specific heat capacity?

<p>Specific heat capacity is defined per unit mass, while molar specific heat capacity is defined per mole.</p> Signup and view all the answers

What are the two conditions under which specific heats are defined for gases?

<p>Constant volume and constant pressure.</p> Signup and view all the answers

What is the relationship between Cp and Cv for an ideal gas?

<p>Cp - Cv = R, where R is the universal gas constant.</p> Signup and view all the answers

A quasi-static process is an infinitely slow process such that the system remains in thermal and mechanical equilibrium with its surroundings.

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

What is the work done by an ideal gas in an isothermal expansion from volume V₁ to V₂ at temperature T?

<p>W = μRT ln(V₂/V₁)</p> Signup and view all the answers

The internal energy of an ideal gas depends only on its temperature.

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

Why are reversible processes important in thermodynamics?

<p>They achieve the highest possible efficiency for heat engines and refrigerators.</p> Signup and view all the answers

What is a Carnot cycle?

<p>A theoretical thermodynamic cycle that operates between two temperatures and achieves the maximum possible efficiency for a heat engine or refrigerator.</p> Signup and view all the answers

What is the efficiency of a Carnot engine operating between temperatures T₁ and T₂?

<p>η = 1 - T₂/T₁</p> Signup and view all the answers

The efficiency of a Carnot engine is independent of the nature of the working substance.

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

What is a refrigerator?

<p>A device that extracts heat from a cold reservoir, does work on the system, and releases heat to a hot reservoir.</p> Signup and view all the answers

What is the coefficient of performance (α) of a refrigerator?

<p>α = Q₂/W, where Q₂ is the heat extracted from the cold reservoir, and W is the work done on the system.</p> Signup and view all the answers

The spontaneous processes of nature are irreversible.

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

A process that is reversible is an idealised notion.

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

What are the two main causes of irreversibility in thermodynamic processes?

<p>Non-equilibrium states and dissipative effects.</p> Signup and view all the answers

Flashcards

Thermodynamics

The branch of physics that deals with heat, temperature, and the conversion of heat and other forms of energy.

Thermal Equilibrium

A state where macroscopic variables like pressure, volume, temperature, mass, and composition of a system remain constant over time.

Zeroth Law of Thermodynamics

If two systems are in thermal equilibrium with a third system, they are also in thermal equilibrium with each other.

Heat

A form of energy transfer from a hotter object to a colder object due to a temperature difference.

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Internal Energy

The total energy of a system due to the random motion of its particles.

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Work

Energy transfer associated with a force acting over a distance.

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First Law of Thermodynamics

The change in a system's internal energy is equal to the heat added to the system minus the work done by the system.

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Specific Heat Capacity

The amount of heat required to raise the temperature of one unit of mass of a substance by one degree Celsius.

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Thermodynamic State Variables

Macroscopic properties like temperature, pressure, and volume that describe the thermodynamic state of a system.

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Equation of State

Mathematical relationship between thermodynamic state variables of a system.

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Thermodynamic Processes

Changes in the state of a thermodynamic system, including changes in pressure, temperature, volume or internal energy.

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Heat Engines

Devices which use thermal energy to do mechanical work, converting heat to work.

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Refrigerators and Heat Pumps

Devices that transfer thermal energy from a cold reservoir to a hot reservoir (refrigerator) or the opposite (heat pump).

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Second Law of Thermodynamics

Heat does not spontaneously flow from a cold object to a hot object.

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Reversible process

A process that can return to its original state without leaving any noticeable change to its surroundings.

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Irreversible process

A process that cannot be reversed to its original state without some noticeable effect on its surroundings, such as heat.

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Study Notes

Chapter Twelve: Thermodynamics

  • Thermodynamics is the branch of physics that deals with concepts of heat and temperature, and the conversion of energy.
  • It's a macroscopic science, focusing on bulk systems rather than molecular structures.
  • Concepts like heat, temperature, work, and internal energy are more precisely defined.

12.1 Introduction

  • Thermal energy is converted to work (e.g., rubbing hands together) and vice-versa (e.g., a steam engine).
  • Historically, heat was thought of as a fluid, but now understood as a form of energy.
  • Rumford's experiment (1798) demonstrated heat as energy, not a fluid. The amount of heat produced relied on the work done, not the sharpness of the drill.

12.2 Thermal Equilibrium

  • Thermal equilibrium: a system's macroscopic variables remain constant over time.
  • This means properties like pressure, volume, temperature, mass, and composition aren't changing.

12.3 Zeroth Law of Thermodynamics

  • Two systems in thermal equilibrium with a third system are in thermal equilibrium with each other.
  • This implies a shared variable: temperature (T). If Tₐ = Tₓ and Tₓ = Tᵧ, then Tₐ = Tᵧ

12.4 Heat, Internal Energy, and Work

  • Internal energy (U) is the sum of molecular kinetic and potential energies within a system.
  • It's a state function (value depends only on the current state, not the path to get there).
  • Heat (Q) is energy transfer due to temperature difference.
  • Work (W) is energy transfer not involving a temperature difference (e.g., pushing a piston).
  • First Law of Thermodynamics: ΔQ = ΔU + ΔW (Change in heat equals change in internal energy plus change in work).

12.5 First Law of Thermodynamics

  • Internal energy can change through heat flow and work done on or by the system.
  • ΔQ = ΔU + ΔW
  • ΔQ: heat supplied to the system by the surroundings
  • ΔW: work done by the system on the surroundings
  • ΔU: change in internal energy of the system

12.6 Specific Heat Capacity

  • Specific heat (s): Amount of heat needed to raise the temperature of 1 kg of a substance by 1 K.
  • Molar specific heat (C): Amount of heat needed to raise the temperature of 1 mole of a substance by 1 K.

12.7 Thermodynamic State Variables and Equations of State

  • State variables: variables that describe a system's state (e.g., pressure, volume, temperature, mass).
  • Equations of state: relationships between state variables (e.g., the ideal gas law: PV = nRT).
  • Extensive variables: depend on the size of the system (e.g., volume, internal energy, mass).
  • Intensive variables: do not depend on the size of the system (e.g., temperature, pressure, density).

12.8 Thermodynamic Processes

  • Quasi-static process: a process that happens infinitely slowly, allowing the system to remain in equilibrium at each step.
  • Isothermal process: constant temperature.
  • Isobaric process: constant pressure.
  • Isochoric process: constant volume.
  • Adiabatic process: no heat transfer.

12.9 Heat Engines

  • Heat Engine: converts heat to work in a cyclic process.
  • A working substance undergoes a cycle of processes absorbing heat at a high temperature and rejecting heat at a low temperature, while performing work.
  • Efficiency η = (work done) / (heat input) = 1 - (heat rejected) / (heat input).

12.10 Refrigerators and Heat Pumps

  • Refrigerators are heat pumps operating in reverse.
  • They absorb heat from a cold reservoir, and reject heat to a hot reservoir, requiring work input.
  • Coefficient of Performance (COP) = (heat removed) / (work input).

12.11 Second Law of Thermodynamics

  • The Second Law of Thermodynamics limits the efficiency of a heat engine.
  • Kelvin-Planck statement: It's impossible to construct a cyclic process that absorbs heat from one reservoir and delivers an equal amount of work.

12.12 Reversible and Irreversible Processes

  • Reversible process: one in which both the system and surroundings can return to their initial states without any net change elsewhere in the universe.
  • Irreversible process: a process that cannot be exactly reversed.

12.13 Carnot Engine

  • A theoretical heat engine that operates on a cyclic process involving reversible steps.
  • It sets an upper limit on the efficiency of any heat engine between two temperatures.

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