Chapter 15 Chemical Equilibrium

Chapter 15 Chemical Equilibrium

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 

Multiple Choice

What is the pH of water?

• 0

• 4

• 7

• 14

Multiple Choice

Which of the following is true about acids and bases?

• The lower the pH, the stronger the acid

• the higher the pH, the stronger the acid

• The lower the pH, the more neutral the acid

• The higher the pH, the weaker the base

Multiple Choice

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

• they form separate layers
• they mix physically but not chemically
• they break apart into separate elements
• they react chemically to form a salt

Multiple Choice

Ammonia has a pH of 12.  Ammonia is __________.

• an acid
• a base
• an element
• a metal

Multiple Choice

Which of these pH values represent an acid?

• 4

• 8

• 10

• 12

Multiple Choice

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

• 1.0 x 10⁶ M

• 8.0 x 10¹ M

• 1.0 x 10⁸ M

• 1.0 x 10^-8 M

Multiple Choice

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

• 4.0

• 10.0

• 1.0 x 10 ^-4

• cannot be determined from the information

Multiple Choice

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

• 4.0

• 10.0

• 1.0 x 10 ^-4

• cannot be determined from the information

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 

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.

• 6.2 x 10^-10 M

• 2.5 x 10^-5 M

• 1.1 M

• 1.2 M

Multiple Choice

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

• shift equilibrium right
• shift equilibrium left
• change K
• have no change

Multiple Choice

This symbol indicates that a reaction is ____________

• reversible
• irreversible

Multiple Choice

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

• K_c= [CO][H₂O] / [CO₂][H₂]  
• K_c= [CO₂][H₂] / [CO]
• K_c= [CO₂][H₂] / [CO][H₂O]
• K_c= [CO] / [CO₂][H₂]  

Multiple Choice

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

• gaseous
• liquid
• solid
• plasma

Multiple Choice

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

• shift equilibrium right
• shift equilibrium left
• increase rate of reaction
• have no change

Multiple Choice

A complete reaction is in which:

• All the reactants convert into products

• All the reactants do not convert into products

• Half reactants convert into products

• only 10% reactants convert into products

Multiple Choice

A complete reaction is in which:

• All the reactants convert into products

• All the reactants do not convert into products

• Half reactants convert into products

• only 10% reactants convert into products

Multiple Choice

Such reactions which continue in both directions are called:

• Irreversible reactions

• Reversible reactions

• Non-reactive reactions

• dynamic reactions

Multiple Choice

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

• [Products]^p / [Reactants]^r

• [Reactants]^r / [Products]^p

• [A][B] / [C]

Multiple Choice

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

• [Products]^p / [Reactants]^r

• [Reactants]^r / [Products]^p

• [A][B] / [C]