Brainscape's Knowledge GenomeTM

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


See full index

IMAT Chem > Chapter 6: Equilibrium > Flashcards

Chapter 6: Equilibrium Flashcards

1
Q

What is a homogeneous mixture?

A

A mixture with uniform composition and properties throughout.

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

What is a heterogeneous mixture?

A

A mixture with non-uniform composition and varying properties.

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

What type of mixture is air?

A

Homogeneous mixture of gases.

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

How much oxygen does inhaled air typically contain?

A

About 20% by volume.

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

How much oxygen does exhaled air typically contain?

A

About 16% by volume.

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

What separation technique is used for homogeneous mixtures?

A

Fractional distillation.

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

What separation technique is used for heterogeneous mixtures?

A

Filtration.

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

What is a reversible reaction?

A

A reaction where products can reform reactants under certain conditions.

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

What is an equilibrium mixture?

A

A mixture where concentrations of reactants and products remain constant over time.

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

What happens to hydrated copper(II) sulfate when heated?

A

It loses water and becomes white

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

What is dynamic equilibrium?

A

A state where forward and reverse reaction rates are equal.

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

What condition is necessary for equilibrium?

A

A closed system.

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

What does the equilibrium constant (Kc) indicate?

A

How far a reaction proceeds in the forward direction at a given temperature.

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

Does Kc provide information about reaction speed?

A

No

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

What is the position of equilibrium?

A

The relative amounts of reactants and products at equilibrium.

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

What happens when equilibrium shifts to the right?

A

More products are formed.

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

What happens when equilibrium shifts to the left?

A

More reactants are formed.

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

What principle predicts equilibrium shifts when a system is disturbed?

A

Le Chatelier’s principle.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What happens when concentration of a reactant increases?

A

Equilibrium shifts to oppose the change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What happens in an open system during equilibrium?

A

The reaction may go to completion as products escape.

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

How does an increase in pressure affect equilibrium?

A

It favors the side with fewer gas molecules.

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

When does pressure affect equilibrium?

A

Only when gases are involved.

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

What happens to equilibrium in an exothermic reaction when temperature increases?

A

Shifts to the left (reverse reaction).

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

What happens to equilibrium in an endothermic reaction when temperature increases?

A

Shifts to the right (forward reaction).

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

How does temperature affect Kc?

A

Kc changes; increased Kc favors the forward reaction.

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

Do catalysts affect the position of equilibrium?

A

No

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

Why don’t catalysts affect equilibrium position?

A

They increase forward and reverse reaction rates equally.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What type of reaction has ∆H < 0?

A

Exothermic reaction.

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

What type of reaction has ∆H > 0?

A

Endothermic reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the role of a catalyst in equilibrium reactions?

A

It reduces the time needed to reach equilibrium.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

How is equilibrium affected by removing a product?

A

Shifts to the right to produce more of the removed product.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

How is equilibrium affected by adding a reactant?

A

Shifts to the right to form more products.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How is equilibrium affected by adding a product?

A

Shifts to the left to produce more reactants.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What happens when CO2 is removed from a calcium carbonate equilibrium system?

A

The reaction moves forward

35
Q

What is the effect of decreasing temperature on an exothermic reaction?

A

Equilibrium shifts to the right.

36
Q

What is the effect of decreasing temperature on an endothermic reaction?

A

Equilibrium shifts to the left.

37
Q

What determines the extent of equilibrium shift with temperature changes?

A

Whether the reaction is exothermic or endothermic.

38
Q

What does a large Kc value mean?

A

The reaction strongly favors products.

39
Q

What does a small Kc value mean?

A

The reaction strongly favors reactants.

40
Q

In which direction does equilibrium shift when pressure decreases?

A

Toward the side with more gas molecules.

41
Q

What is the equilibrium constant expression for a reaction?

A

A ratio of product concentrations to reactant concentrations

42
Q

What does a change in Kc signify?

A

A change in temperature.

43
Q

Why must equilibrium reactions occur in a closed system?

A

To prevent reactants or products from escaping.

44
Q

What is the effect of pressure on a reaction with equal gas molecules on both sides?

A

No effect on equilibrium.

45
Q

How does temperature affect reaction rates?

A

Higher temperatures increase reaction rates.

46
Q

What is the definition of a reversible reaction?

A

A reaction that can proceed in both forward and reverse directions.

47
Q

What happens to equilibrium when temperature increases in an exothermic reaction?

A

Kc decreases

48
Q

What happens to equilibrium when temperature decreases in an endothermic reaction?

A

Kc decreases

49
Q

Why do equilibrium constants only change with temperature?

A

Because temperature affects reaction rates differently for forward and reverse reactions.

50
Q

How does equilibrium respond to changes in gas volume?

A

It shifts to the side with fewer or more gas molecules depending on the volume change.

51
Q

Why does Le Chatelier’s principle predict equilibrium shifts?

A

To minimize changes imposed on a system.

52
Q

What is the importance of maintaining equilibrium in industrial processes?

A

It ensures optimal yield of products.

53
Q

What is the relationship between Kc and reaction direction?

A

Larger Kc favors forward; smaller Kc favors reverse.

54
Q

How is equilibrium related to chemical stability?

A

It reflects a balance between product and reactant stability.

55
Q

What are the units of Kc?

A

Varies depending on the reaction stoichiometry.

56
Q

How is equilibrium achieved in a closed system?

A

When forward and reverse reaction rates are equal.

57
Q

What is the key characteristic of an equilibrium state?

A

Concentrations of reactants and products remain constant.

58
Q

How does pressure affect equilibrium involving solids and liquids?

A

It has no effect.

59
Q

Why is equilibrium dynamic?

A

Reactions continue in both directions at the same rate.

60
Q

Why do industrial reactions often use catalysts?

A

To speed up the attainment of equilibrium.

61
Q

How does equilibrium affect reaction reversibility?

A

It allows both forward and reverse reactions to occur simultaneously.

62
Q

What does it mean if Kc is temperature-dependent?

A

Reaction yield varies with temperature.

63
Q

What happens to equilibrium if a gaseous reactant is added?

A

Shifts toward the product side.

64
Q

Why do open systems prevent equilibrium?

A

Products or reactants escape

65
Q

What determines the direction of equilibrium shift with pressure changes?

A

Number of gas molecules on each side.

66
Q

How does adding a catalyst affect reaction equilibrium?

A

No change in equilibrium position.

67
Q

How does removing a catalyst affect equilibrium?

A

No change in position; reaction may slow down.

68
Q

Why is equilibrium independent of reaction pathway?

A

Pathway affects speed

69
Q

What is a practical example of equilibrium in nature?

A

Carbon dioxide exchange in water and atmosphere.

70
Q

What happens to equilibrium when product concentration decreases?

A

Shifts toward products.

71
Q

Why does equilibrium oppose concentration changes?

A

To restore balance.

72
Q

How is equilibrium modeled mathematically?

A

Using the equilibrium constant expression.

73
Q

What happens if a reactant concentration is halved?

A

Equilibrium shifts to produce more reactant.

74
Q

What is required to measure Kc?

A

Concentrations of reactants and products at equilibrium.

75
Q

Why are pressure changes critical in gas-phase reactions?

A

They can significantly alter reaction yield.

76
Q

What is the equilibrium constant for N₂ + 3H₂ ↔ 2NH₃?

A

Kc = [NH₃]² / ([N₂][H₂]³).

77
Q

How does increasing pressure affect NH₃ production in the Haber process?

A

Favors NH₃ formation due to fewer gas molecules.

78
Q

What is Le Chatelier’s principle’s main application?

A

Predicting shifts in industrial chemical processes.

79
Q

What is equilibrium’s role in biochemical reactions?

A

Maintains stability in metabolic pathways.

80
Q

What is a common industrial example of equilibrium?

A

Ammonia synthesis in the Haber process.

81
Q

What defines a system in equilibrium?

A

Forward and reverse reactions occur at the same rate.

82
Q

What happens when equilibrium is disturbed?

A

The system adjusts to minimize the disturbance.

83
Q

Why does equilibrium require constant conditions?

A

To maintain balance between reactants and products.

IMAT Chem (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions