Chapter 15 Chemical Equilibrium

Chapter 15 Chemical Equilibrium

Presentation

•

Chemistry

•

University

•

Medium

•

NGSS

HS-PS1-6, HS-PS1-5

Standards-aligned

Created by

Luis Bello

Used 6+ times

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63 Slides • 19 Questions

1

Chapter 15 Chemical Equilibrium

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Previous Chapter 14 Acids and Bases

14.2 Acids: Properties and Examples

14.3 Bases: Properties and Examples

14.4 Molecular Definitions of Acids and Bases

14.5 Reactions of Acids and Bases

14.6 Acid-Base Titration: A Way to Quantify the Amount of Acid or Base in a Solution

14.7 Strong and Weak Acids and Bases

14.8 Water: Acid and Base in One

14.9 The pH and pOH Scales: Ways to Express Acidity and Basicity

14.10 Buffers: Solutions That Resist pH Change

3

Multiple Choice

What is the pH of water?

1

0

2

4

3

7

4

14

4

Multiple Choice

Which of the following is true about acids and bases?

1

The lower the pH, the stronger the acid

2

the higher the pH, the stronger the acid

3

The lower the pH, the more neutral the acid

4

The higher the pH, the weaker the base

5

Multiple Choice

Explain what happens when a strong acid and a strong base are poured into the same container.

1

they form separate layers

2

they mix physically but not chemically

3

they break apart into separate elements

4

they react chemically to form a salt

6

Multiple Choice

Ammonia has a pH of 12. Ammonia is __________.

1

an acid

2

a base

3

an element

4

a metal

7

Multiple Choice

Which of these pH values represent an acid?

1

4

2

8

3

10

4

12

8

Multiple Choice

If the pH of a solution is 8 the [H₃O⁺] is

1

1.0 x 10⁶M

2

8.0 x 10¹M

3

1.0 x 10⁸M

4

1.0 x 10^-8M

9

Multiple Choice

If the pH of a solution is 4.0, what is the pOH?

1

4.0

2

10.0

3

1.0 x 10 ^-4

4

cannot be determined from the information

10

Multiple Choice

If the pH of a solution is 4.0, what is the pOH?

1

4.0

2

10.0

3

1.0 x 10 ^-4

4

cannot be determined from the information

11

Today: Chapter 15 Chemical Equilibrium

15.2 The Rate of a Chemical Reaction

15.3 The Idea of Dynamic Chemical Equilibrium

15.4 The Equilibrium Constant: A Measure of How Far a Reaction Goes

15.5 Heterogeneous Equilibria: The Equilibrium Expression for Reactions Involving a Solid or a Liquid

15.6 Calculating and Using Equilibrium Constants

15.7 Disturbing a Reaction at Equilibrium: Le Châtelier’s Principle

15.8 The Effect of a Concentration Change on Equilibrium

15.9 The Effect of a Volume Change on Equilibrium

15.10 The Effect of a Temperature Change on Equilibrium

15.11 The Solubility-Product Constant

15.12 The Path of a Reaction and the Effect of a Catalyst

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Multiple Choice

For the following reaction: H₂(g) + Cl₂ (g) ↔ 2HCl(g), calculate the concentration of HCl when K_eq= 2.3x10^-5, [H₂]= 0.0056mol, [Cl₂]= 0.0048mol.

1

6.2 x 10^-10M

2

2.5 x 10^-5 M

3

1.1 M

4

1.2 M

73

Multiple Choice

2SO₂(g)+O₂(g)⇌2SO₃(g)
Decreasing volume of container will

1

shift equilibrium right

2

shift equilibrium left

3

change K

4

have no change

74

Multiple Choice

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This symbol indicates that a reaction is ____________

1

reversible

2

irreversible

75

Multiple Choice

What is the equilibrium-constant expression for
CO₂(g) + H₂(g) ↔ CO(g) + H₂O(l)

1

K_c= [CO][H₂O] / [CO₂][H₂]

2

K_c= [CO₂][H₂] / [CO]

3

K_c= [CO₂][H₂] / [CO][H₂O]

4

K_c= [CO] / [CO₂][H₂]

76

Multiple Choice

Changes in pressure will only affect substances that are in the __________ state.

1

gaseous

2

liquid

3

solid

4

plasma

77

Multiple Choice

2SO₂(g)+O₂(g)⇌2SO₃(g)
Adding SO₂(g) will

1

shift equilibrium right

2

shift equilibrium left

3

increase rate of reaction

4

have no change

78

Multiple Choice

A complete reaction is in which:

1

All the reactants convert into products

2

All the reactants do not convert into products

3

Half reactants convert into products

4

only 10% reactants convert into products

79

Multiple Choice

A complete reaction is in which:

1

All the reactants convert into products

2

All the reactants do not convert into products

3

Half reactants convert into products

4

only 10% reactants convert into products

80

Multiple Choice

Such reactions which continue in both directions are called:

1

Irreversible reactions

2

Reversible reactions

3

Non-reactive reactions

4

dynamic reactions

81

Multiple Choice

The general rule for writing an equilibrum expression is K_eq= __________

1

[Products]^p / [Reactants]^r

2

[Reactants]^r / [Products]^p

3

[A][B] / [C]

82

Multiple Choice

The general rule for writing an equilibrum expression is K_eq= __________

1

[Products]^p / [Reactants]^r

2

[Reactants]^r / [Products]^p

3

[A][B] / [C]

Chapter 15 Chemical Equilibrium

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