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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.

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2
Q

What is a heterogeneous mixture?

A

A mixture with non-uniform composition and varying properties.

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3
Q

What type of mixture is air?

A

Homogeneous mixture of gases.

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4
Q

How much oxygen does inhaled air typically contain?

A

About 20% by volume.

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5
Q

How much oxygen does exhaled air typically contain?

A

About 16% by volume.

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6
Q

What separation technique is used for homogeneous mixtures?

A

Fractional distillation.

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7
Q

What separation technique is used for heterogeneous mixtures?

A

Filtration.

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8
Q

What is a reversible reaction?

A

A reaction where products can reform reactants under certain conditions.

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9
Q

What is an equilibrium mixture?

A

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

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10
Q

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

A

It loses water and becomes white

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11
Q

What is dynamic equilibrium?

A

A state where forward and reverse reaction rates are equal.

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12
Q

What condition is necessary for equilibrium?

A

A closed system.

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13
Q

What does the equilibrium constant (Kc) indicate?

A

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

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14
Q

Does Kc provide information about reaction speed?

A

No

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15
Q

What is the position of equilibrium?

A

The relative amounts of reactants and products at equilibrium.

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16
Q

What happens when equilibrium shifts to the right?

A

More products are formed.

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17
Q

What happens when equilibrium shifts to the left?

A

More reactants are formed.

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18
Q

What principle predicts equilibrium shifts when a system is disturbed?

A

Le Chatelier’s principle.

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19
Q

What happens when concentration of a reactant increases?

A

Equilibrium shifts to oppose the change

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20
Q

What happens in an open system during equilibrium?

A

The reaction may go to completion as products escape.

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21
Q

How does an increase in pressure affect equilibrium?

A

It favors the side with fewer gas molecules.

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22
Q

When does pressure affect equilibrium?

A

Only when gases are involved.

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23
Q

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

A

Shifts to the left (reverse reaction).

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24
Q

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

A

Shifts to the right (forward reaction).

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25
How does temperature affect Kc?
Kc changes; increased Kc favors the forward reaction.
26
Do catalysts affect the position of equilibrium?
No
27
Why don’t catalysts affect equilibrium position?
They increase forward and reverse reaction rates equally.
28
What type of reaction has ∆H < 0?
Exothermic reaction.
29
What type of reaction has ∆H > 0?
Endothermic reaction.
30
What is the role of a catalyst in equilibrium reactions?
It reduces the time needed to reach equilibrium.
31
How is equilibrium affected by removing a product?
Shifts to the right to produce more of the removed product.
32
How is equilibrium affected by adding a reactant?
Shifts to the right to form more products.
33
How is equilibrium affected by adding a product?
Shifts to the left to produce more reactants.
34
What happens when CO2 is removed from a calcium carbonate equilibrium system?
The reaction moves forward
35
What is the effect of decreasing temperature on an exothermic reaction?
Equilibrium shifts to the right.
36
What is the effect of decreasing temperature on an endothermic reaction?
Equilibrium shifts to the left.
37
What determines the extent of equilibrium shift with temperature changes?
Whether the reaction is exothermic or endothermic.
38
What does a large Kc value mean?
The reaction strongly favors products.
39
What does a small Kc value mean?
The reaction strongly favors reactants.
40
In which direction does equilibrium shift when pressure decreases?
Toward the side with more gas molecules.
41
What is the equilibrium constant expression for a reaction?
A ratio of product concentrations to reactant concentrations
42
What does a change in Kc signify?
A change in temperature.
43
Why must equilibrium reactions occur in a closed system?
To prevent reactants or products from escaping.
44
What is the effect of pressure on a reaction with equal gas molecules on both sides?
No effect on equilibrium.
45
How does temperature affect reaction rates?
Higher temperatures increase reaction rates.
46
What is the definition of a reversible reaction?
A reaction that can proceed in both forward and reverse directions.
47
What happens to equilibrium when temperature increases in an exothermic reaction?
Kc decreases
48
What happens to equilibrium when temperature decreases in an endothermic reaction?
Kc decreases
49
Why do equilibrium constants only change with temperature?
Because temperature affects reaction rates differently for forward and reverse reactions.
50
How does equilibrium respond to changes in gas volume?
It shifts to the side with fewer or more gas molecules depending on the volume change.
51
Why does Le Chatelier's principle predict equilibrium shifts?
To minimize changes imposed on a system.
52
What is the importance of maintaining equilibrium in industrial processes?
It ensures optimal yield of products.
53
What is the relationship between Kc and reaction direction?
Larger Kc favors forward; smaller Kc favors reverse.
54
How is equilibrium related to chemical stability?
It reflects a balance between product and reactant stability.
55
What are the units of Kc?
Varies depending on the reaction stoichiometry.
56
How is equilibrium achieved in a closed system?
When forward and reverse reaction rates are equal.
57
What is the key characteristic of an equilibrium state?
Concentrations of reactants and products remain constant.
58
How does pressure affect equilibrium involving solids and liquids?
It has no effect.
59
Why is equilibrium dynamic?
Reactions continue in both directions at the same rate.
60
Why do industrial reactions often use catalysts?
To speed up the attainment of equilibrium.
61
How does equilibrium affect reaction reversibility?
It allows both forward and reverse reactions to occur simultaneously.
62
What does it mean if Kc is temperature-dependent?
Reaction yield varies with temperature.
63
What happens to equilibrium if a gaseous reactant is added?
Shifts toward the product side.
64
Why do open systems prevent equilibrium?
Products or reactants escape
65
What determines the direction of equilibrium shift with pressure changes?
Number of gas molecules on each side.
66
How does adding a catalyst affect reaction equilibrium?
No change in equilibrium position.
67
How does removing a catalyst affect equilibrium?
No change in position; reaction may slow down.
68
Why is equilibrium independent of reaction pathway?
Pathway affects speed
69
What is a practical example of equilibrium in nature?
Carbon dioxide exchange in water and atmosphere.
70
What happens to equilibrium when product concentration decreases?
Shifts toward products.
71
Why does equilibrium oppose concentration changes?
To restore balance.
72
How is equilibrium modeled mathematically?
Using the equilibrium constant expression.
73
What happens if a reactant concentration is halved?
Equilibrium shifts to produce more reactant.
74
What is required to measure Kc?
Concentrations of reactants and products at equilibrium.
75
Why are pressure changes critical in gas-phase reactions?
They can significantly alter reaction yield.
76
What is the equilibrium constant for N₂ + 3H₂ ↔ 2NH₃?
Kc = [NH₃]² / ([N₂][H₂]³).
77
How does increasing pressure affect NH₃ production in the Haber process?
Favors NH₃ formation due to fewer gas molecules.
78
What is Le Chatelier's principle's main application?
Predicting shifts in industrial chemical processes.
79
What is equilibrium's role in biochemical reactions?
Maintains stability in metabolic pathways.
80
What is a common industrial example of equilibrium?
Ammonia synthesis in the Haber process.
81
What defines a system in equilibrium?
Forward and reverse reactions occur at the same rate.
82
What happens when equilibrium is disturbed?
The system adjusts to minimize the disturbance.
83
Why does equilibrium require constant conditions?
To maintain balance between reactants and products.

IMAT Chem (9 decks)

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