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PMP 102 > Concepts Of Thermodynamics > Flashcards

Concepts Of Thermodynamics Flashcards

1
Q

What are the two forms of energy?

A

Potential energy
Kinetic energy

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2
Q

What is potential energy?

A

Any form of stored energy

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3
Q

What is kinetic energy?

A

Energy of moving objects

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4
Q

What are examples of potential energy?

A

Gravitational
Elastic
Chemical
Electrical

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5
Q

What are examples of kinetic energy?

A

Radiant
Thermal
Sound
Mechanical

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6
Q

What are the three types of systems?

A

Open
Closed
Isolated

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7
Q

What happens in an open system?

A

Mass transfer
Heat transfer

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8
Q

What happens in a closed system?

A

No mass transfer
Heat transfer

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9
Q

What happens in an isolated system?

A

No mass transfer
No heat transfer

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10
Q

What is the Zeroth Law of Thermodynamics?

A

If two systems are in thermal equilibrium with a third system, the two original systems are in thermal equilibrium with each other.

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11
Q

What is the first Law of Thermodynamics?

A

Energy cannot be created or destroyed, it can only be transferred from one form to another.

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12
Q

What is the Law of Conservation of Energy?

A

The change in internal energy of a closed system will be equal to the heat added or released by the system on its surrounding or work done on the system by its surroundings.

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13
Q

What does each figure mean in this equation?
🔺U=Q+W

A

🔺U= change in internal energy
Q= heat added to the system
W = work done by the system (mass transfer)

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14
Q

If Q is positive what does this mean?

A

Heat has been added to the system.
Endothermic process

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15
Q

If Q is negative what does this mean?

A

Heat released from the system.
Exothermic process

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16
Q

What does isovolumetric mean?

A

Constant volume
🔺U=Q
No work is done on it by the system

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17
Q

What does isothermal mean?

A

Constant temperature.
Q=W
No change in internal energy

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18
Q

What does adiabatic mean?

A

🔺U= W
Internal energy changes only for work done or received by the system

19
Q

What does one calorie do?

A

The heat needed to raise the temperature of one gram of water one degree under standard pressure.

20
Q

What is one calorie in joules?

A

4.184J

21
Q

What is heat capacity (C)?

A

Amount of heat required to raise a substance temperature by 1 kelvin

22
Q

What is specific heat capacity (Cs) ?

A

Amount of heat required to raise one gram of a substance by 1 kelvin

23
Q

What is enthalpy?

A

Measurement if energy in a thermodynamic system (joules)

24
Q

What is the equation for enthalpy?

A

🔺H=🔺U+🔺(PV)
P= pressure
V= volume

25
Q

Why does 🔺H = Q in biological system?

A

Biological systems are under constant pressure and volume rarely changes.
🔺H=🔺U
🔺U=Q
Therefore 🔺H=Q

26
Q

What is 🔺H in an endothermic process?

A

Positive

27
Q

What is 🔺H in an exothermic process?

A

Negative

28
Q

What is the second law of thermodynamics?

A

The universe is always moving towards maximum disorder.

29
Q

What is entropy?

A

Measure of disorder

30
Q

What are the symbols in this equation mean?
S= KB Ln W

A

KB= Boltzmann constant
Ln= natural logarithm
W= microstates

31
Q

What is the third law of thermodynamics?

A

At absolute zero (0Kelvin) the entropy of a perfect crystalline substance is zero.

32
Q

What is the equation for Gibbs free energy?

A

G=H-TS

33
Q

What are the symbols in the Gibbs free energy equation?

A

G=Gibbs free energy
H=enthalpy
S=Entropy
T=temperature

34
Q

What does the number for 🔺G indicate?

A

Negative= spontaneous in forward direction only
Zero= reaction at equilibrium
Positive= non-spontaneous

35
Q

Why is T always positive in Gibbs free energy equation?

A

Temperature is in Kelvin

36
Q

What is free energy of formation?

A

The free energy change which result from 1mol of substance prepared from its elements at standard pressure (1atm) and a given temperature (usually 298K)

37
Q

What is the free energy formation of chemical elements?

A

0

38
Q

What is oxidative metabolism?

A

A process by which nutrients from our diet are converted to energy.

39
Q

What is thermochemistry?

A

The study of heat changes that occur during a chemical reaction.

40
Q

What is the standard enthalpy change of a reaction?

A

The heat transferred by a chemical reaction under standard conditions

41
Q

What is the standard enthalpy change of formation?

A

The enthalpy change when 1mol of a compound is formed under standard conditions for it’s constituent elements in their standard states

42
Q

What is the bond dissociation enthalpy?

A

The enthalpy change, per mol, in the gas phase, when a bond is broken of compound A-B through the reaction: AB—> A+B

43
Q

What is the standard entropy change of a reaction?

A

The difference in standard entropy between products and reactants of a system under standard conditions.

PMP 102 (29 decks)

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