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dYEEEE > Unit 5 - Chemical Equilibrium > Flashcards

Unit 5 - Chemical Equilibrium Flashcards

1
Q

T/F
Most chemical reactions are irreversible. Only few reactions proceed to completion.

A

F

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2
Q

It exists when two opposing reactions occur simultaneously at the same rate.

A

Chemical equlibrium

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3
Q

It is a dynamic process.

A

Chemical equilibrium

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4
Q

T/F
Once equilibrium is achieved, the amount of each reactant and product remains constant.

A

T

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5
Q

T/F
As a system approaches equilibrium, both the forward and reverse reactions are occuring.

A

T

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6
Q

All reactants and products are in same phase and cannot be separated.

A

Homogenous equilibrium

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7
Q

Reactants and products are not in homogenous phase and can be separated.

A

Heterogenous equilibrium

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8
Q

T/F
The forward rate will be the reactant side.

A

T

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9
Q

T/F
The reverse rate will be the product side.

A

T

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10
Q

States that the rate of any chemical reaction is proportional to the product of the masses of the reacting substances, with each mass raised to a power equal to the coefficient that occurs in the chemical equation.

A

Law of mass action

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11
Q

It relates the concentrations of reactants and products at equilibrium.

A

Equilibrium constant

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12
Q

T/F
It is the product of the concentrations of PRODUCTS of a chemical equilibrium divided by the concentrations of REACTANTS, each raised to the power equal to its coefficient in the balanced chemical equation.

A

T

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13
Q

T/F
In writing equilibrium constant expression, a pure solid or a pure liquid in the reaction is omitted from the expression.

A

T

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14
Q

T/F
The concentration of a pure solid or a pure liquid is always the same.

A

T

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15
Q

The activity of liquid or solid is defined as _____.

A

1

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16
Q

T/F
H2O(l) has activity of 1 while H2O(g) is considered in the expression.

A

T

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17
Q

This results from a reversible reaction involving reactants and products that are in different phases.

A

Heterogeneous equilibrium

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18
Q

T/F
In heterogeneous equilibrium, neither density nor molar mass is a variable, the concentrations of solids and pure liquids are constant.

A

T

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19
Q

T/F
The concentrations of pure liquids and pure solids are not included in equilibrium constant expressions.

A

T

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20
Q

The larger K the more _____ are present at equilibrium.

A. Reactants
B. Products

A

B

21
Q

The smaller K the more _____ are present at equilibrium.

A. Reactants
B. Products

A

A

22
Q

If K > 1, then products dominate at equilibrium and equilibrium lies to the _____.

A. Left
B. Right

A

B

23
Q

If K < 1, then products dominate at equilibrium and equilibrium lies to the _____.

A. Left
B. Right

A

A

24
Q

If K > 1, the reaction is _____.

A. Product-favored; product predominates at equilibrium.
B. Reactant-favored; reactant predominates at equilibrium

A

A

25
Q

If K < 1, the reaction is _____.

A. Product-favored; product predominates at equilibrium.
B. Reactant-favored; reactant predominates at equilibrium

A

B

26
Q

T/F
In the magnitude of equilibrium constants, an equilibrium can be approached from any direction.

A

T

27
Q

The ___ for a reaction in one direction is the reciprocal of the equilibrium constant of the reaction in the opposite direction.

A

Kc

28
Q

It is the equilibrium constant for a net reaction made up of two or more steps is the product of the equilibrium constants for the individual steps.

A

Multiple equilibria

29
Q

T/F
In predicting the direction of the reaction, the reaction quotient, Q, for a reaction at conditions NOT at equilibrium.

A

T

30
Q

T/F
Q = K only at equilibrium.

A

T

31
Q

If K = Q the _____.

A. System is at equilibrium.
B. Forward reaction is favored.
C. Reverse reaction is favored.

A

A

32
Q

If K > Q the _____.

A. System is at equilibrium.
B. Forward reaction is favored.
C. Reverse reaction is favored.

A

B

33
Q

If K < Q the _____.

A. System is at equilibrium.
B. Forward reaction is favored.
C. Reverse reaction is favored.

A

C

34
Q

T/F
Changes in experimental conditions may disturb the balance and shift the equilibrium.

A

T

35
Q

Factors that affect equilibrium.

A

Concentration
Catalyst
Temperature
Volume and Pressure

36
Q

A principle wherein if stress is applied to a system that is in equilibrium, the system will adjust in such a way that the stress is partially offset as the system reaches a new equilibrium position.

A

Le Chatelier’s Principle

37
Q

A + B ⇋ C + D

Increasing the amount of A or B.

A. Forward
B. Reverse
C. No shift

A

A

38
Q

A + B ⇋ C + D

Increasing the amount of C or D.

A. Forward
B. Reverse
C. No shift

A

B

39
Q

A + B ⇋ C + D

Decreasing the amount of A or B.

A. Forward
B. Reverse
C. No shift

A

B

40
Q

A + B ⇋ C + D

Decreasing the amount of C or D.

A. Forward
B. Reverse
C. No shift

A

A

41
Q

A + B ⇋ C + D

Reacting A with compound E.

A. Forward
B. Reverse
C. No shift

A

B

42
Q

A + B ⇋ C + D

Removing C as the reaction proceeds.

A. Forward
B. Reverse
C. No shift

A

A

43
Q

A system that RELEASES heat to the surroundings, has a negative ΔH (-ΔH) by convention, because the enthalpy of the products is LOWER than the enthalpy of the reactants of the system.

A

Exothermic reaction

44
Q

A system of reactants that ABSORBS heat from the surroundings in a reaction has a positive ΔH (+ ΔH), because the HIGHER of the products is HIGHER than the enthalpy of the reactants of the system.

A

Endothermic reaction

45
Q

Changes in volume and pressure affect only systems involving _____.

A. Solid
B. Liquid
C. Gases

A

C

46
Q

T/F
Changes in volume and pressure increase in pressure or decrease in volume favors the reaction where there is less total number of moles of gases.

A

T

47
Q

T/F
Changes in volume and pressure decrease in pressure or increase in volume favors the reaction where there is higher total number of moles of gases.

A

T

48
Q

T/F
Presence of catalyst does not affect the state of equilibrium.

A

T

49
Q

T/F
Presence of catalyst allows the system to reach equilibrium faster.

A

T

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