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Gen Chem > Lesson 1-5 > Flashcards

Lesson 1-5 Flashcards

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1
Q

Change in Entropy: Positive or Negative

Solid sugar is added to water to form a solution.

A

Positive

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2
Q

Change in Entropy: Positive or Negative

Iodine vapor condenses on a cold surface to form crystals.

A

Negative

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3
Q

Change in Entropy: Positive or Negative

Water freezez

A

Negative

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4
Q

Change in Entropy: Positive or Negative

Student breaks a pyrex beaker

A

Positive

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5
Q

Change in Entropy: Positive or Negative

A gas expands

A

Positive

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6
Q

(Entropy) change measures the dispersal of energy: how much energy is spread out in a particular process

A

True

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7
Q

Entropy, S, is a measure of randomness of disorder. The natural tendency of things is to tend toward (lesser) disorder.

A

Greater

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8
Q

Spontaneity is independent of the (speed or rate of a reaction)

A

True

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9
Q

A (spontaneous process) is one that occurs without outside intervention

A

True

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10
Q

Thermodynamics studies how changes in energy, (enthalpy) and temperature affect spontaneity of a process or chemical reaction

A

Entropy

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11
Q

3 factors to predict spontaneity

A

Energy change, temperature and entropy change

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12
Q

Driving force for a spontaneous process

A

An increase in the entropy of the universe

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13
Q

Determination of the degree of disorderliness

A

A. Number of arrangement of molecules can have in a system
B. Number of types of molecules as well as number of molecules

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14
Q

A reaction will never spontaneously move away from equilibrium

A

And will always move spontaneously towards equilibrium

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15
Q

Spontaneity is a process can be determined from

A

change in entropy and change in free energy of a system

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16
Q

Gibbs free energy formula

A

△G = △H - T△S

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17
Q

Study of the rates of chemical reactions

A

Chemical Kinetics

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18
Q

The rate of a chemical reaction is proportional to the number of collisions between reactant molecules.

A

Collision Theory

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19
Q

Energy required for collisions to be sufficiently energetic to break chemical bonds

A

Activation Energy

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20
Q

Collisions that results in a chemical reactions and form a new product.

A

Effective Collision

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21
Q

No product was formed when collision happens.

A

Ineffective Collision

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22
Q

Substances that help speed up the rate of chemical reactions

A

Catalysts

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23
Q

Process of speeding up a reaction by using catalysts

A

Catalysis

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24
Q

Catalysts and reactants are in the same phase

A

Homogenous Catalysis

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25
Q

Catalysts and reactants are in different phases

A

Heterogeneous Catalysis

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26
Q

Proteins that function as catalyst in all living systems

A

Enzymes

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27
Q

Enzyme lowers the activation energy of a reaction

A

True

28
Q

Energy level that the reactant molecules must overcome before a reaction can occur

A

Activation energy

29
Q

Entropy phases

A

Gasses > Liquids > Solids

30
Q

Entropy Change Formula

A

△S°rxn = ΣS°(products) - Σ°(reactants)

31
Q

Increase in entropy when

A

Gas is formed from the reactants

32
Q

Decrease in entropy when

A

Gaseous reactants are converted to solids or liquids

33
Q

Reduction in disorder during

A

Synthesis reactions

34
Q

Increase in disorder during

A

Decomposition reactions

35
Q

Reaction that occurs under a given set of condition

A

Spontaneous reactions

36
Q

Reaction that does not occur under a given set of conditions

A

Nonspontaneous reactions

37
Q

△H - △S +

A

Always negative, Spontaneous

38
Q

△H + △S -

A

Always Positive, Nonspontaneous

39
Q

△H - △S -

A

Negative at Low T, Spontaneous

40
Q

△H + △S +

A

Positive at Low T, Nonspontaneous

41
Q

A reaction is at _______ state if the rate of the forward reaction equals the backward reaction

A

Equilibrium

42
Q

Double arrow

A

Reversible reaction, at Equilibrium

43
Q

Reaction Quotient

mA + nB -> xC + yD

A

Qc = (C^x)(D^y)/(A^m)(B^n)

44
Q

Conditions that needs to be met for a chemical reaction to occur

A

Particles in the substance must collide and have enough energy.

45
Q

Why does a candle burn more rapidly when place in an open jar than in air?

A

Higher oxygen concentration

46
Q

Greater number of reactant are more _____ at higher temperatures

A

Energetic

47
Q

Second Law of Thermodynamics

A

For any spontaneous process, the entropy of the universe increases.

48
Q

When hear is added to a pure liquid, the temperature

A

Increases and the entropy increases

49
Q

Conditions for a reaction to be spontaneous at all temperatures

A

△H < 0 and △S >=0

50
Q

For a spontaneous reaction

A

△G = △H - T△S must be negative

51
Q

△S = Products - Reactants

A

True

52
Q

Entropy Change Formula

A

△Ssys = (Mass)(Molar Mass)(△Fusion: Negative)(1000j/Kj)/(°C+273.15)

53
Q

Hg Mercury 113 g

A

-5.51 J/K

54
Q

Cu Copper 125 g

A

-19.1 J/K

55
Q

Au Gold 97 g

A

-4.86 J/K

56
Q

Hg Mercury 89 g

A

-4.34 J/K

57
Q

Au Gold 69 g

A

-3.47 J/K

58
Q

Hg Mercury 67 g

A

-3.26 J/K

59
Q

Cu Copper 69 g

A

-10.6 J/K

60
Q

First Law of Thermodynamics

A

Energy cannot be created or destroyed. Total energy of the universe is constant. Energy can only be converted.

61
Q

When heat is added to a system, the amount of heat added can

A

increase the temperature, increase internal energy, and do external work.

62
Q

The lowest possible temperature is absolute zero, at

A

0 on the Kelvin scale and -273 degrees on the Celsius scale.

63
Q

When you breathe on your hand, the temperature of the exhaled air reaching your hand

A

Depends on how you blow

64
Q

The second law of thermodynamics tells us that heat cannot flow from

A

cold to hot without external energy.

65
Q

Heat engines such as jet engines are more efficient when run at

A

High temperatures

Gen Chem (4 decks)

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