slide 1 of 39 chemistry 18.2. © copyright pearson prentice hall slide 2 of 39 reversible reactions...
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Chemistry 18.2
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Reversible Reactions and Equilibrium
In the early 1900s, German chemists refined the process of making ammonia from elemental nitrogen and hydrogen.This process allows the manufacture of nitrogen fertilizers. You will learn how reaction conditions can influence the yield of a chemical reaction.
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Reversible Reactions and Equilibrium
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Reversible Reactions
Reversible Reactions
How do the amounts of reactants and products change in a chemical system at equilibrium?
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Reversible Reactions and Equilibrium
> Reversible Reactions
At chemical equilibrium, no net change occurs in the actual amounts of the components of the system.
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Reversible Reactions
If the rate of the shoppers going up the escalator is equal to the rate of the shoppers going down, then the number of shoppers on each floor remains constant, and there is an equilibrium.
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Reversible Reactions
A reversible reaction is one in which the conversion of reactants to products and the conversion of products to reactants occur simultaneously.
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Reversible Reactions and Equilibrium
> Reversible Reactions18.2
At equilibrium, all three types of molecules are present.
SO2 and O2 react to give
SO3
SO3 decomposes to SO2 and O2
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Reversible Reactions
When the rates of the forward and reverse reactions are equal, the reaction has reached a state of balance called chemical equilibrium.
The relative concentrations of the reactants and products at equilibrium constitute the equilibrium position of a reaction.
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Reversible Reactions18.2
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Reversible Reactions and Equilibrium
> Reversible Reactions
Animation 23
Take a close look at a generalized reversible reaction.
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Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Factors Affecting Equilibrium: Le Châtelier’s Principle
What three stresses can cause a change in the equilibrium position of a chemical system?
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Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Stresses that upset the equilibrium of a chemical system include changes in the concentration of reactants or products, changes in temperature, and changes in pressure.
18.2
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
The French chemist Le Châtelier proposed what has come to be called Le Châtelier’s principle: If a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress.
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Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Simulation 24
Simulate Le Châtelier’s principle for the synthesis of ammonia.
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Concentration
Rapid breathing during and after vigorous exercise helps reestablish the body’s correct CO2:H2CO3 equilibrium, keeping the acid concentration in the blood within a safe range.
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Temperature
Dinitrogen tetroxide is a colorless gas; nitrogen dioxide is a brown gas. The flask on the left is in a dish of hot water; the flask on the right is in ice.
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Reversible Reactions and Equilibrium
> Factors Affecting Equilibrium: Le Châtelier’s Principle
Pressure
Pressure affects a mixture of nitrogen, hydrogen, and ammonia at equilibrium
18.2
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Conceptual Problem 18.1
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Conceptual Problem 18.1
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Conceptual Problem 18.1
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Practice Problems for Conceptual Problem 18.1
Problem Solving 18.6 Solve a similar problem with the help of an interactive guided tutorial.
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Reversible Reactions and Equilibrium
>
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Equilibrium Constants
Equilibrium Constants
What does the value of Keq indicate about the equilibrium position of a reaction?
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© Copyright Pearson Prentice Hall
Reversible Reactions and Equilibrium
> Equilibrium Constants
The equilibrium constant (Keq) is the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation.
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Reversible Reactions and Equilibrium
> Equilibrium Constants
A value of Keq greater than 1 means that products are favored over reactants; a value of Keq less than 1 means that reactants are favored over products.
18.2
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SAMPLE PROBLEM
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SAMPLE PROBLEM
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18.1
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Practice Problems for Sample Problem 18.1
Problem Solving 18.7 Solve Problem 7 with the help of an interactive guided tutorial.
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Practice Problems for Sample Problem 18.2
Problem Solving 18.9 Solve Problem 9 with the help of an interactive guided tutorial.
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Section Quiz
-or-Continue to: Launch:
Assess students’ understanding of the concepts in Section
18.2 Section Quiz.
18.2.
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18.2 Section Quiz.
1. In a reaction at equilibrium, reactants and products
a. decrease in concentration.
b. form at equal rates.
c. have equal concentrations.
d. have stopped reacting.
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18.2 Section Quiz.
2. In the reaction 2NO2(g) 2NO(g) + O2(g), increasing the pressure on the reaction would cause
a. the amount of NO to increase.
b. the amount of NO2 to increase.
c. nothing to happen.
d. the amount of O2 to increase.
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18.2 Section Quiz.
3. Changing which of the following would NOT affect the equilibrium position of a chemical reaction?
a. concentration of a reactant only
b. concentration of a product only
c. temperature only
d. volume only
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4. For the following reaction, Keq = 1.
A(g) + B(g) C(g) + D(g) Therefore, at equilibrium
a. [C] = [A].
b. [A][B] = 0.
c. [AB] = [CD] = 1.
d. [A][B] = [C][D].
18.2 Section Quiz.
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