Thermodynamics Flashcards

1
Q

What is a System?

A

A collection of material objects, enclosed from the surrounding area

Types of systems include isolated, closed, and open systems.

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2
Q

What is an Isolated System?

A

A system with no exchange of matter or energy with the surroundings

Example: A thermos flask with a sealed lid.

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3
Q

What is a Closed System?

A

A system that exchanges energy but not matter with the surroundings

Example: A sealed container that can be heated.

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4
Q

What is an Open System?

A

A system that exchanges both matter and energy with the surroundings

Example: A boiling pot of water.

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5
Q

What is Energy?

A

The measure of matter movement during transformation from one form to another

Types of energy include mechanical, thermal, chemical, and electrical energy.

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6
Q

What is Mechanical Energy?

A

Energy associated with motion or position

Includes kinetic energy (due to motion) and potential energy (due to position).

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7
Q

What is Thermal Energy?

A

Energy from the random motion of atoms and molecules

Example: Heat in a warm cup of tea.

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8
Q

What is Chemical Energy?

A

Energy stored in chemical bonds

Example: Energy released during digestion or combustion.

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9
Q

What is Electrical Energy?

A

Energy due to the motion of charged particles

Example: Electricity powering a bulb.

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10
Q

What is Work?

A

The measure of energy conversion from one form to another

Types of work include mechanical, chemical, osmotic, and electrical work.

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11
Q

What is Mechanical Work?

A

Energy used to move body components against mechanical forces

Example: Lifting a weight.

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12
Q

What is Chemical Work?

A

Energy used in chemical reactions

Example: Protein synthesis.

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13
Q

What is Osmotic Work?

A

Energy used to transport substances against a concentration gradient

Example: Active transport in cells.

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14
Q

What is Electrical Work?

A

Energy used to move charged particles

Example: Generation of nerve impulses.

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15
Q

What is the First Law of Thermodynamics?

A

Total energy in a system remains constant; it can only change through energy exchange with the surroundings

Mathematical formulation involves change in internal energy, heat added, and work done.

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16
Q

What is Primary Heat?

A

Heat produced from metabolic processes

Example: Friction of blood flow in vessels produces heat.

17
Q

What is Secondary Heat?

A

Heat produced due to electrical resistance

Example: Muscle contractions producing heat.

18
Q

What is the Second Law of Thermodynamics?

A

All energy conversions are accompanied by energy dissipation in the form of heat, which cannot be fully converted back into other forms of energy.

19
Q

What is a Reversible Process?

A

A process where the system can return to its initial state without external energy

Example: Idealized gas compression/expansion.

20
Q

What is an Irreversible Process?

A

A process that cannot return to the initial state without external energy

Example: Friction, real-world chemical reactions.

21
Q

What is Entropy?

A

A measure of the amount of energy unavailable to do work

Involves heat produced and absolute temperature.

22
Q

How does Entropy behave in Reversible Processes?

A

Entropy remains constant or changes predictably.

23
Q

How does Entropy behave in Irreversible Processes?

A

Entropy increases due to heat dissipation.

24
Q

What is Thermodynamic Equilibrium?

A

A state with no energy or matter exchange; free energy = 0, entropy = maximum.

25
What is a Steady State?
A state where energy and matter exchange occur, but system parameters remain constant ## Footnote Example: Blood flow in the human body.
26
What is a similarity between Thermodynamic Equilibrium and Steady State?
Both involve constant system parameters.
27
What is the Coefficient of Effectiveness?
The effectiveness of a system’s ability to convert free energy into work. ## Footnote In irreversible processes, part of the free energy dissipates as heat, reducing the work performed.
28
What is the Coefficient of Efficiency for reversible processes?
100% efficiency ## Footnote This indicates that all free energy is converted into work without any loss.
29
What is the implication of Prigogine’s Theorem?
In a steady state, the speed of entropy production caused by irreversible processes is positive and at its minimum among all possible values. ## Footnote This shows how systems minimize entropy production while maintaining efficiency.
30
How do living systems self-regulate?
By maintaining homeostasis (steady state) and minimizing entropy production. ## Footnote An example is body temperature regulation.
31
What happens to free energy and entropy at life?
Free Energy: High, Entropy: Low ## Footnote Cells perform work actively, keeping the system organized.
32
What changes occur in free energy and entropy at death?
Free Energy: Decreases, Entropy: Increases ## Footnote The system loses organization and moves toward equilibrium.
33
What characterizes a steady state in living systems?
Free Energy: Maintained at a constant level, Entropy: Increases but remains minimized. ## Footnote This allows continuous work through active regulation.
34
What occurs in stationary conditions (thermodynamic equilibrium)?
Free Energy: Reaches zero, Entropy: Maximum ## Footnote The system has lost organization and is at equilibrium.
35
Define Internal Energy.
Total energy in the system, combining usable and unusable energy. ## Footnote It includes free energy, temperature, and entropy.
36
What is Free Energy?
Usable energy for work (e.g., ATP in biological systems). ## Footnote This energy is available for performing biological processes.
37
What is Bound Energy?
Useless energy dissipated as heat and unavailable for work. ## Footnote It represents energy that cannot be harnessed for useful tasks.