Thermodynamics Flashcards

1
Q

What is thermodynamic describe?

A

Processes that involve changes in temperature, transformation of energy, and the relationship between heat and work

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2
Q

What does the system boundary separate?

A

The system from the surroundings

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3
Q

What is the law of conservation of energy?

A

Energy can neither be created nor destroyed; it can only change form. The internal energy of the universe does not change. The energy lost by one must equal the energy gained by the other.

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4
Q

What is internal energy (U)?

A

Energies associated with the structure and motion of molecules within the system

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5
Q

What is internal energy as a state function?

A

(a state function) Change in internal energy depends only on the initial and final states and not on the path connecting these states. U system= U final-U inital

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6
Q

What can the internal energy of a closed system be changed by?

A

Transfer of work (w) and heat (q) between the system and its surrounding

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7
Q

What is the first law?

A

The change in internal energy of a closed system equals: U sys = q + w

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8
Q

What must happen when heat is lost by the system?

A

It must be complemented by an input of work to make up for the loss of heat (and conversely)

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9
Q

What is used to measure changes in energies at constant pressure?

A

The change in enthalpy

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10
Q

What does enthalpy as a state function mean?

A

Change in internal energy depends only on the initial and final states and not on the path connecting these states.
H system=. H final- H inital

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11
Q

What are the standard conditions for the standard enthalpy reactions?

A

289K

P= 1 bar

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12
Q

What is the standard enthalpy of formation?

A

Enthalpy associated with the formation of 1 mole of a substance from its element in their most stable form

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13
Q

What can the standard enthalpy of a reaction be determined from?

A

Standard enthalpy of formation

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14
Q

What does it mean if enthalpy change is less than 0 (

A

Reaction is exothermic

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15
Q

What does it mean if enthalpy change is more than 0 (>0)?

A

Reaction is endothermic

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16
Q

What happens if reaction losses heat?

A

Transfer of thermal energy from the system to the surroundings

17
Q

What happens if the reaction gains heat?

A

Transfer of thermal energy from the surroundings to the system

18
Q

What does the first law of thermodynamics not predict?

A

Which of several possible processes will occur (i.e. which one is natural or spontaneous)

19
Q

What is the second law of thermodynamics state?

A

That the total entropy of a system and its surrounding always increases for a spontaneous process

20
Q

What is entropy?

A

It is related to energy dispersal, measures the microscopic disorder of a system. Units J.K-1

21
Q

What is the reaction if G

A

It is spontaneous

22
Q

What is the reaction if G=0?

A

The reaction is at equilibrium

23
Q

What is the reaction if G>0?

A

It is non spontaneous

24
Q

What does it mean if the K»1?

A

Mixture will mainly consist of the products at equilibrium

25
Q

What does heterogeneous systems do?

A

Omit terms for pure solids and liquids

26
Q

What is Kd?

A

The dissociation constant

27
Q

What is Kp?

A

The thermodynamic equilibrium constant