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Review Flashcards

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1
Q

What is energy placed in?

A
  1. PE

2. KE

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2
Q

What is KE?

A

Energy of motion or anything moving

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3
Q

What is potential energy?

A

Stored energy of an object is to varied such as stress or electric charges

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4
Q

What are KE types?

A
  1. V(ery) - vibrational
  2. T(ough) - transitional
  3. R(oad) - rotational
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5
Q

What is chemical energy?

A

Energy required or released when bonds break

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6
Q

What is a system?

A

Any sample under observation

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7
Q

What is an open system?

A

Exchange of Eng and matter with surroundings

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8
Q

What is a closed system?

A

No exchange of eng with surroundings

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9
Q

What is an isolated system?

A

No exchange of Eng and matter with surroundings

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10
Q

What is specific heat capacity?

A

Amt of eng to raise 1 g of a temp by 1c

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11
Q

What is thermal energy?

A

Sum of KE of particles of a matter sample

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12
Q

What is temp?

A

Avge KE of molecules

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13
Q

What is heat?

A

Sum of KE of a system

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14
Q

What does heat measure?

A

Measure transfer between sys and surrounding

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15
Q

What’s the 1st law of thermodynamics?

A

Law of conservation of eng
Nrg not created or destroyed, just turned into different forms of end
Nrg in universe is constant
E surrounding = E system

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16
Q

What is the second law of conservation?

A

If thermal contact, heat from hotter obj will transfer to heat of lower obj until equal

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17
Q

What is an endothermic rxn?

A

When energy enters system or airs surrounded from surroundings

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18
Q

What is an exothermic reaction?

A

When heat leaves the system or released into surroundings

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19
Q

What is enthalpy?

A

Total nrg in a sys
Nrg of sys + PV
Nrg needed to move temp from abs 0 to certain temp

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20
Q

What is an enthalpy diff?

A

Change in PE of reactants and products?

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21
Q

Why is enthalpy diff used?

A

Unable to measure H of a system

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22
Q

Under what conditions does the enthalpy change of system equal the heat exchanged between system and surroundings

A

Constant pressure and volume

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23
Q

What is enthalpy also referred as?

A

Hear content

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24
Q

What does the enthalpy change of a system depend on?

A
  1. The initial state

2. The final state

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25
Q

Why are the enthalpy changes at 1 pressure different from those at different pressures?

A

The initial and final states are at different pressures

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26
Q

What pressure is chosen with enthalpy and why?

A

Atmospheric

  1. Easy to achieve
  2. SHC is reports in that
27
Q

When is an enthalpy change positive?

A

When heat enters (endothermic)

28
Q

When is an enthalpy change negative?

A

When heat leaves (exothermic)

29
Q

What 3 steps must occur for a solute to dissolve in a solvent?

A
  1. Bonds between molecules or ions of a solute must be broken to make room for solvent molecules
  2. Bonds between solvent molecules must be broken to make room for solute molecules
  3. Bonds must form between solute and solvent molecules. Can be bonds such as intermolecular bonds
30
Q

What is the enthalpy of a solution?

A

The enthalpy change associate ls with a solute dissolving in a solvent

31
Q

When is the enthalpy associate with something positive?

A

Separating solute and sober molecules

32
Q

When is the associated enthalpy negative?

A

Mixing solute and solvent particles

33
Q

What is the enthalpy of melting?

A

Energy needed to change a solid into a liquid

34
Q

What is the enthalpy of vaporization?

A

Energy required to change a liquid into a gas

35
Q

What is the enthalpy of condensation?

A

Energy released when gas becomes a liquid

36
Q

What is the enthalpy of freezing?

A

Energy released when liquid turns into a solid

37
Q

What are the 4 main calorimetry assumptions?

A
  1. System is isolated (any thermal energy linked with surroundings outside of colorimeter is small enough to be ignored)
  2. Thermal energy exchanged with polystyrene cups, thermometer, lid and stirring rod is small enough to be ignored
  3. If something dissolves or reacts with water, resulting solution retains properties of water
  4. The process takes place under constant pressure
38
Q

In a thermochemical equation, when is the number negative?

A

On product side of equation

39
Q

When, in a thermochemical equation, is the nrg positive?

A

In the reactant side

40
Q

In an enthalpy diagram, when goes the arrow point down?

A

When rxn is exothermic or negative

41
Q

When does the arrow point up in an enthalpy diagram?

A

When it’s endothermic or positive

42
Q

What is bond energy?

A

Energy required to break a bond

43
Q

What does a large bond energy mean?

A

More stable bond

44
Q

What are negative enthalpy values?

A

Energy lost from a system or transferred into surroundings

45
Q

What are positive enthalpy value?

A

Energy gained from surroundings

46
Q

What is a physical enthalpy change?

A

A change in phase or when something dissolves

Intermolecular forces holding molecules together, broken or formed

47
Q

What is an enthalpy chem change??

A

Input and cosiest bonds break and form new ones

Products have different amts of pe when compared with reactants

48
Q

What is entropy?

A

The measure of randomness or disorder

49
Q

What does a large entropy mean?

A

Large energy disorder meaning that atoms are not ordered and are free to move anywhere

50
Q

What does a low entropy mean?

A

Low disorder meaning that atoms are highly disordered and are free to move anywhere

51
Q

Why do large molecules have a large entropy?

A

They have several atoms placed in a specific order

52
Q

What do small molecules have a high entropy?

A

They have few atoms placed in a specific order

53
Q

What is the entropy of universe increasing or remaining constant?

A

Universal processes get more disordered

54
Q

When does the entropy decrease? (3 reasons)

A
  1. More moles of products than reactants
  2. Complex molecules broken down into smaller molecules
  3. Substance changes from more ordered state to less ordered state
55
Q

What is Gibbs free energy?

A

Energy available to work in a chem system

56
Q

What are exergonic reactions?

A

Release energy and are spontaneous

57
Q

What are endergonic rescuing?

A

Absorb energy and are non-spontaneous

58
Q

What is thermal stability?

A

Ability of a substance to resist decomposition when heat

59
Q

What is an effective collision? (2 reasons)

A
  1. Correct orientation of reactants

2. Sufficient activation energy

60
Q

What is the activation energy?

A

Min amt of energy required to initiate a chem rxn

61
Q

How does nature of reactants affect reaction rate?
2 ions
1 acid and base
1 molecular

A
  1. Ions in solution have rapid rate bc:
  2. No bonds to be broken for new ones to form
    • and - charges attract each other
  4. Same for acids and bases
  5. Molecular rxns are slower bc:
  6. Bonds must be broken for new ones to form
62
Q

How does the concentration affect rate of rxn?

A

Increase in [] of reactants will increase tie number of collisions per unit time

63
Q

Why Increase in [] of reactants increase rate of rxn?

A
  1. More particles in the same volume

2. Greater number of effective collisions

64
Q

Why does as the [] of products increase, the rate of rxn decrease?

A

Remaining products are more likely to collide wiry a product than reactant

chemistry (3 decks)

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