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Chemistry 3321 > Exam 1 > Flashcards

Exam 1 Flashcards

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1
Q

First law of thermodynamics

A

energy can be converted from one form to another with the interaction of heat, work, and internal energy, but cannot be created or destroyed

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2
Q

Second law of thermodynamics

A

total entropy in spontaneous processes increases irreversibly

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3
Q

Third law of thermodynamics

A

entropy of perfectly crystalline substance at 0 K is 0

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4
Q

What did Clausius say about the second law of thermodynamics?

A

no process is possible whose sole result is the transfer of heat from a cold body to a hot body

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5
Q

What is the critical point? (2)

A

the point on a phase diagram at which the liquid and gas phases have the same density and are therefore indistinguishable; in the P-V plot, the critical point is an inflection point in the constant temperature line write out partial derivatives

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6
Q

What is a supercritical fluid?

A

A phase of matter that forms at a temperature/pressure above the critical point that effuses like a gas and dissolves substances like a liquid

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7
Q

Define extensive quantity.

A

Quantity that depends on the size of a system

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8
Q

Give three examples of extensive quantities.

A

volume, mass, energy

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9
Q

Define intensive quantity.

A

Quantity that doesn’t depend on the size of a system

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10
Q

Give three examples of intensive quantities.

A

pressure, temperature, density

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11
Q

Write out the equation for pressure.

A

write out - Chapter 16: Textbook Notes

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12
Q

Write out the equation for the compressibility factor.

A

write out - Chapter 16: Textbook Notes

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13
Q

Write out the van der Waals equation.

A

write out

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14
Q

What do the variables a and b in the van der Waals equation correspond to?

A

a - corresponds to intermolecular attractions; b - corresponds to the size of the molecules

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15
Q

When does Z = 1?

A

Z = 1 under all conditions for ideal gases

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16
Q

When does Z not equal 1?

A

Z does not equal 1 as pressure increases (deviations from ideal gas behavior)

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17
Q

Write out the van der Waals equation in cubic form.

A

write out - Chapter 16: Textbook Notes

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18
Q

Define heat.

A

manner of energy transfer that results from a temperature difference between the system and its surroundings.

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19
Q

Heat input is a

A

positive quantity

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20
Q

Heat evolved is a

A

negative quantity

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21
Q

Define work.

A

the transfer of energy between the system of interest and its surroundings as a result of the existence of unbalanced forces between the two

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22
Q

Work done on the system is a (sketch figure)

A

sketch - Dineli’s Exam 4 Notes, page 6; positive quantity - compression

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23
Q

Work done by the system is a (sketch figure)

A

sketch - Dineli’s Exam 4 Notes, page 6; negative quantity - expansion

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24
Q

What is the equation for pressure-volume work at constant pressure?

A

write out - Chapter 19: Textbook Notes

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25
Q

What is the equation for pressure-volume work at not-constant pressure?

A

write out - Chapter 19: Textbook Notes

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26
Q

Define state function.

A

a property that depends only upon the state of the system, and not upon how the system was brought to that state.

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27
Q

(T/F) Energy is a state function.

A

True - write out - Chapter 19: Textbook Notes

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28
Q

Isothermal compression requires what work?

A

the minimum amount of work

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29
Q

Isothermal expansion requires what work?

A

the maximum amount of work

30
Q

Write out the equation for isothermal/reversible work.

A

write out - Chapter 19: Textbook Notes (page 2)

31
Q

(T/F) Work is a state function.

A

False, it is a path function.

32
Q

What is the relationship between work, heat, and energy?

A

∆U = q + w

33
Q

What is the second statement of the first law of thermodynamics?

A

the sum of work and heat, which are both inexact differentials, is a state function and an exact differential

34
Q

Define adiabatic process.

A

process in which no energy as heat is transferred (q = 0)

35
Q

Write out the three derivation equations for constant-volume heat capacity.

A

write out - Chapter 19: Textbook Notes (page 2)

36
Q

What is the value of C(V) for one mole of a monatomic ideal gas?

A

3/2*R

37
Q

What is the value of C(V) for one mole of a nonlinear polyatomic ideal gas?

A

3R

38
Q

Under what conditions is enthalpy relevant?

A

constant-pressure situations

39
Q

What are the relationships between q, ∆H, ∆U, P, and ∆V?

A

(1) qp = ∆H; (2) ∆H = ∆U + P∆V

40
Q

What is the law of corresponding states?

A

all fluids, when evaluated at the same reduced temperature + pressure, have roughly the same Z value and thus deviate from ideal gas behavior to the same degree

41
Q

For an ideal gas, internal energy (U) only depends on

A

temperature

42
Q

What is the Joule-Thomson coefficient?

A

mu(sub)JT and is equivalent to (di-T/di-P) at constant H

43
Q

Nonzero values of the Joule-Thomson coefficient reflect

A

intermolecular interactions

44
Q

How did Clausius sum up the first two laws of thermodynamics?

A

The energy of the universe is constant, the entropy tending to a maximum

45
Q

Convert 1 atm-L into joules

A

1 atm-L = 101.33 J

46
Q

Define a state function.

A

Independent of the path taken, to establish a property or value

47
Q

Give four examples of a state function.

A

S, G, H, T

48
Q

Give two examples of a path function.

A

w, q

49
Q

Write out the van der Waals equation of state in the PV=nRT form.

A

write out - Dineli’s Exam 4 Review, page 1

50
Q

Calculate dP/dV using explicit differentiation.

A

calculate - Dineli’s Exam 4 Review, page 1

51
Q

Calculate dP/dV using implicit differentiation.

A

calculate - Dineli’s Exam 4 Review, page 2

52
Q

What is the Zeroth Law of Thermodynamics?

A

if 2 thermodynamic systems are in equilibrium with a third, then the first two are in equilibrium with each other (A=C, B=C, then A=B)

53
Q

What is Dalton’s Law of Partial Pressure?

A

if we have a mixture of ideal gases, the total pressure of the mixture is equal to the sum of the partial pressures of the component gasses

54
Q

What is the Equipartition Theorem?

A

At thermal equilibrium, each microscopic degree of freedom of a molecule has an average energy 1/2kbT

55
Q

What is the internal energy of a monatomic ideal gas containing N particles?

A

U = 3/2 * N * kb * T; U(bar) = 3/2 * R * T; because R = kb * NA

56
Q

Define reversible process.

A

When Pext and P differ only infinitesimally, the process is called reversible because the process could be reversed by decreasing the external pressure infinitesimally

57
Q

Define irreversible process.

A

When Pext is controlled to be constant and the final pressure; expansion/compression is allowed to continue until the gas re-equilibrates at the final pressure and volume

58
Q

Sketch a pressure-volume plot for isothermal reversible compression.

A

sketch - Dineli’s Exam 4 Review, page 8

59
Q

Sketch a pressure-volume plot for isothermal reversible expansion.

A

sketch - Dineli’s Exam 4 Review, page 8

60
Q

What happens to pressure and temperature in adiabatic compression?

A

pressure and temperature both increase without any gain or loss of heat

61
Q

What happens to pressure and temperature in adiabatic expansion?

A

pressure and temperature both decrease without any gain or loss of heat

62
Q

What is the difference between state and path functions in terms of differentials?

A

state functions are exact differentials, whereas path functions are inexact differentials

63
Q

What did the Joule-Thomson experiment try to do?

A

tried to measure the temperature change when a gas expanded in a vacuum

64
Q

In the microscopic entropy equation, what does W represent?

A

the number of microstates

65
Q

Sketch out the microscopic representation of entropy and the associated table.

A

sketch/write out Dineli’s Exam 4 Review, page 15

66
Q

Define microstate.

A

number of different possible arrangements of molecular position at a particular thermodynamic state

67
Q

What is the relationship between microstates and entropy?

A

more microstates mean more entropy

68
Q

Write out the two formulas associated with the Clausius inequality.

A

write out Dineli’s Exam 4 Review, page 17

69
Q

In the Clausius Inequality, when does the equality sign apply and when does the inequality sign apply?

A

equality sign applies if change is carried out reversibly (i.e. system is in equilibrium during process); inequality is applied if change is carried out irreversibly at any stage

70
Q

The Clausius Inequality as a statement is equivalent to

A

the Second Law of Thermodynamics

71
Q

Write out the formula for the entropy of a gaseous mixture.

A

write out - Formulas to Memorize, page 1

Chemistry 3321 (3 decks)

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