Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHM 201 > CHM Exam 2 Flashcards (Chapter 9 and Chapter 10) > Flashcards

CHM Exam 2 Flashcards (Chapter 9 and Chapter 10)

1
Q

Energy

A

the capacity to do work or produce heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

First Law of Thermodynamics

A

energy is conserved and can be converted from one form to another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Energy is/isn’t a statement function

A

is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

the internal energy for a system is the

A

sum of its potential and kinetic energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

the internal energy of a system can be changed by

A

work and heat

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Internal energy formula

A

△E = q + w

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

work

A

force applied over a distance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Work is/isn’t a state function

A

isn’t

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Heat

A

energy flow due to temperature difference

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

exothermic

A

energy as heat flows out of a system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

endothermic

A

energy as heat flows into a system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Heat is/isn’t a state function

A

isn’t

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Enthalpy forumla

A

H = E + PV

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Formula for heat

A

q = mC△T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Enthalpy is/isn’t a state function

A

is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Hess’s Law

A

the change in enthalpy in going from a given set of reactants to a given set of products is the same whether the process takes place in one step or a series of steps

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

△H of reaction formula

A

△H(reaction) = sum of △H of products - sum of △H reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Heating an ideal gas at constant volume

A
  • no PV work done
  • all energy used to increase the translational energies of the gas molecules
  • bomb calorimeter
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Heating an ideal gas at constant pressure

A
  • PV work done
  • energy is used to increase the translational energies of gas molecules and do work
  • coffee cup calorimeter
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

State function

A

refers to a property of a system that depends only on its present state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

energy gained by the surroundings must be…

A

equal to the energy lost by the surroundings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

work done by a gas

A

expansion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

work done to a gas

A

compression

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

1 Latm = x J

A

101.325 J

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

small font = flow = ?

A

work (w) and heat (q)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

capital font = state function = ?

A

Energy (E) and Enthalpy (H)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

q of system = ?

A
  • q of surroundings
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

An open system can exchange ____ with its surroundings

A

energy and matter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

A closed system can exchange ____ with its surroundings

A

only energy

30
Q

A isolated system can exchange ____ with its surroundings

A

neither energy or matter

31
Q

Water has a high heat capacity because

A

of its hydrogen bonds

32
Q

exothermic = ?
endothermic = ?

A

exothermic = negative
endothermic = positive

33
Q

formula for pressure

A

P = (w)/(-△V)

34
Q

What are the 5 applications of thermochemistry?

A
  1. phase changes
  2. dissolution of solids into liquids
  3. enthalpy of chemical reactions
  4. redox chemistry
  5. combustion of hydrocarbons
35
Q

Energy in the universe is constant

A

1st law of thermodynamics

36
Q

Second Law of Thermodynamics

A

states that for any spontaneous process there is always an increase with the entropy of the universe

37
Q

Entropy

A

the thermodynamic function that describes the number of arrangements (positions and/or energy levels) available to a system existing in a given state

38
Q

Nature spontaneously proceeds toward states that have the _____

A

highest probability of occurring

39
Q

Using entropy, thermodynamics can ____

A

predict the direction in which a process will occur spontaneously

40
Q

Entropy of universe formula

A

△S (universe) = △S (system) + △S (surroundings)

41
Q

For a spontaneous process, △S (universe) must be

A

positive

42
Q

△S (system) is dominated by

A

positional entropy

43
Q

For a chemical reaction, △S (system) is dominated by changes in

A

the number of gas molecules

44
Q

△S (surroundings) is determined by heat (formula?)

A

△S (surroundings) = (-△H)/(T)

45
Q

△S (surroundings) is positive for exothermic processes because

A

△H is negative

46
Q

Because △S (surroundings) depends inversely on T, exothermicity becomes more of an important driving force at

A

low temperature

47
Q

Thermodynamics can/can’t predict the rate at which a system will spontaneously change

A

can’t

48
Q

Third Law of Thermodynamics

A

states entropy of a perfect crystal at 0K is zero

49
Q

Free energy is/isn’t a state function

A

is

50
Q

Free Energy

A

a process ocurring at constant temperature and pressure is spontaneous in the direction in which its free energy decreases

51
Q

Standard state is at

A

25 C, and 1 atm

52
Q

△G = 0

A

K = 1

53
Q

△G < 0

A

K > 1, G products < G reactants

54
Q

△G > 0

A

K < 1, G products > G reactants

55
Q

positional microstates _____ as you go from a solid to a liquid to a gas

A

increase

56
Q

Change in entropy formula

A

△S = nCln[T(final)/T(initial)]

57
Q

Standard free energy change formula

A

△G = △H - T△S

58
Q

the number of micro states ____ with the temperature _____

A

increases, increases

59
Q

△G depends on _____ and _____

A

concentration and temperature

60
Q

What are the three ways to find △G of a reaction?

A
  1. △G = △H - T△S
  2. △G = sum of △G(products) - sum of △G(reactants)
  3. △G = -RTlnK
61
Q

The thermodynamic quantity that expresses the degree of disorder in a system is

A

entropy

62
Q

Which one is always positive when a spontaneous process occurs?

A

△S univ

63
Q

What can be said about a chemical system that has reached a minimum in free energy?

A

The system has achieved equilibrium

64
Q

A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if △H is _____ and △S is ______

A

+, +

65
Q

For a reaction to be spontaneous under standard conditions at all temperatures, the signs of △H and △S must be _____ and ____ respectively

A

-, +T

66
Q

The greater the dispersal of matter and/or energy in a system, the _____ the entropy

A

larger

67
Q

The entropy of a substance always _____ as it changes from solid to liquid to gas

A

increases

68
Q

When a pure solid or liquid dissolves in a solvent, the entropy of the substance _______

A

increases

69
Q

When a gas molecule escapes from a solvent, the entropy _____

A

increases

70
Q

Entropy generally increases with ______ molecular complexity since there are more moving electrons

A

increasing

71
Q

Reactions increasing the number of moles of particles often ______ entropy

A

increase

CHM 201 (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions