Title: Lesson 4 The Equilibrium Law Learning Objectives: Know how to quantify K c using equilibrium concentrations Know how to determine K c when given.

Slides:

Advertisements

Similar presentations

When do you use this? You use Keq to find the concentration of a reversible reaction at equilibrium. You use Q to find the concentration of a reversible.

Advertisements

AP Notes Chapter 16 Equilibrium Dynamic chemical system in which two reactions, equal and opposite, occur simultaneously.

Equilibrium Follow-up

Chapter 12 Gaseous Chemical Equilibrium. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the.

Chapter 15 Chemical Equilibrium. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.

AP Chapter 15.  Chemical Equilibrium occurs when opposing reactions are proceeding at equal rates.  It results in the formation of an equilibrium mixture.

Ch. 14: Chemical Equilibrium I.Introduction II.The Equilibrium Constant (K) III.Values of Equilibrium Constants IV.The Reaction Quotient (Q) V.Equilibrium.

Ch. 14: Chemical Equilibrium Dr. Namphol Sinkaset Chem 201: General Chemistry II.

16-2: The Law of Chemical Equilibrium. Remember… Chemical equilibrium is achieved when the rate of the forward rxn is equal to the rate of the reverse.

Ch 18: Chemical Equilibrium

Chemical Equilibrium. Reversible Reactions A reaction that can occur in both the forward and reverse directions. Forward: N 2 (g) + 3H 2 (g)  2NH 3 (g)

EQUILIBRIUM. Many chemical reactions are reversible: Reactants → Products or Reactants ← Products Reactants form Products Products form Reactants For.

1 CHEMICAL EQUILIBRIUM. Chemical Equilibrium Chemical Reactions Types; What is equilibrium? Expressions for equilibrium constants, K c ; Calculating K.

Chemical Equilibrium. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.

Equilibrium Law. Introduction to the Equilibrium law 2H 2 (g) + O 2 (g)  2H 2 O (g) Step 1:Set up the “equilibrium law” equation Kc = Step 2:Product.

Applications of Equilibrium Constants. Example For the reaction below 2A + 3B  2C A 1.5L container is initially charged with 2.3 mole of A and 3.0 mole.

Chapter 15 Chemical Equilibrium

Equilibrium The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.

Lecture 31/26/05. Initial 1.00 M 0 Change (  ) Equil M What if 1.00 mol of SO 2 and 1.00 mol of O 2 put into 1.00-L flask at 1000 K. At equilibrium,

CH 18: CHEMICAL EQUILIBRIUM. SECTION 18.2 SHIFTING EQUILIBRIUM.

Sample Exercise 15.7 Calculating K When All Equilibrium Concentrations Are Known After a mixture of hydrogen and nitrogen gases in a reaction vessel is.

Unit 07: Equilibrium IB Topics 7 & 17 Notes do not inlclude “k p ” gas calculations or heterogeneous eq’m. These are “AP only” concepts that will be revisited.

EQUILIBRIUM BASICS Chapter Lesson Objectives Know -Factors that affect/don’t affect a reaction reaching equilibrium -K is equilibrium constant.

Equilibrium. How do we write the equilibrium constant expression for the following reaction? 2SO 2 (g) + O 2 (g)  2SO 3 (g)

Chapter 14.  Physical state of reactants:  Reactants must come in contact with one another in order for a reaction to occur.  Concentration of reactants:

2 Equilibria 2.1 Chemical Equilibrium (and Equilibrium Constant) 2.2 Calculations using Kc expressions 2.3 Effect of changing conditions on equilibria.

Section 8.3—Reaction Quotient

Chemical Equilibrium K p (gases) and heterogeneous equilibria Chapter 13: Sections 3 & 4 AP.

Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Gaseous Chemical Equilibrium TEXT REFERENCE Masterton and Hurley Chapter 12.

Equilibrium Notes Mrs. Stoops Chemistry. Eqm day 1 Chapter problems p 660 – 665: 14, 16, 20, 28, 32, 38, 42, 46, 50, 52, 59, 61, 70,

Equilibrium Calculations. How can we describe an equilibrium system mathematically? reactants products ⇌ reactants The Keq is the equilibrium constant-

Kp When the reactants and products are gases, we can determine the equilibrium constant in terms of partial pressures. Dalton’s Law of Partial Pressures.

Equilibria: Part III Reviewing the rules.

Equilibrium: A State of Dynamic Balance Chapter 18.1.

1. - ICE Tables - 2  Previous chemistry courses, stoichiometric calculations were straightforward when reactions proceed to completion (called quantitative.

Chemical Equilibrium. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.

Equilibrium. This is usually Question #1 on FR write equilibrium expressions convert between K P and K c eq. constants calculate eq. constants calculate.

Chapter 15 Equilibrium. © 2009, Prentice-Hall, Inc. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed.

Ch 18: Chemical Equilibrium. Section 18.2 Shifting Equilibrium.

Chapter 14: Chemical Equilibrium Sections Sarah Rodriguez.

Chemical Equilibrium Q, K, and Calculations Chapter 16.

The Extent of a Reaction The tendency for a reaction to occur is indicated by the magnitude of the equilibrium constant. A value of K larger than 1 means.

Equilibrium Calculations Lesson 7. How can we describe an equilibrium system mathematically? Keq = =2.5 The Keq is the equilibrium constant- a number.

Equilibrium Calculations Lesson 7. How can we describe an equilibrium system mathematically? reactants products ⇌ reactants The Keq is the equilibrium.

The Concept of Dynamic Equilibrium – The Equilibrium Constant (K)

Section 8.2—Equilibrium Constant How can we describe a reaction at equilibrium?

Title: Lesson 5 Free Energy and Equilibrium Learning Objectives: Know that the position of the equilibrium corresponds to a maximum value of entropy and.

Equilibrium Constant in terms of pressure, Heterogeneous Equilibria, and the Reaction Quotient.

Equilibrium The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. © 2012 Pearson Education,

Chemical Equilibrium Chapter 13 4 out of 75 m/c Free Response: Required Every Year.

Chapter 13 Chemical Equilibrium Reversible Reactions REACTANTS react to form products. PRODUCTS then react to form reactants. BOTH reactions occur: forward.

Chemical Equilibrium Reactants Products Reactants Products As the time increases… [Reactants] decrease, so the rate of forward reaction decreases; [Products]

 Chemical Equilibrium occurs when opposing reactions are proceeding at equal rates.  When the forward reaction equals the reverse reaction.  It results.

“K” Chemistry (part 2 of 3) Chapter 14: Chemical Equilibrium.

1 Equilibrium Constant even though the concentrations of reactants and products are not equal at equilibrium, there is a relationship between them the.

EQUILIBRIUM. Equilibrium Constant (K Values)  The equilibrium constant (Keq) is a number showing the relationship between the concentration of the products.

Equilibrium Calculations Comparing K to Q. Value of the Equilibrium Constant K tells where the equilibrium lies How likely (to what extent) the reaction.

Chemical Equilibrium.

Topic 7- Equilibrium.

Common Ion Effect.

Using Equilibrium Constants

Equilibrium Pressure If the values at equilibrium are given in partial pressure, then solving for the constant is the same, but use Kp instead of Kc. What.

Equilibrium Constants

Applications of the equilibrium constant

10.4 Using Equilibrium Constants

Chapter 13 Reaction Rates and Chemical Equilibrium

RICE BOXES Write a balanced chemical equation for reaction

Equilibrium Constant (Keq)

Presentation transcript:

Title: Lesson 4 The Equilibrium Law Learning Objectives: Know how to quantify K c using equilibrium concentrations Know how to determine K c when given initial concentrations using the ICE method Know how to determine equilibrium concentrations using K c

Main Menu The equilibrium law  So far we know how to derive the equilibrium constant K c and considered what the value tells us about the composition of an equilibrium mixture.  Now we will quantify these values...  We can use the equilibrium law to quantify equilibrium constant or the concentrations of reactants and products in an equilibrium.

Main Menu

Quantifying concentrations of reactants or products from data on initial concentrations of other components  Step 1: Write the balanced equation.  Step 2: Under the equation, write the values of each component using three rows: initial, change, and equilibrium.  Step 3: Write the expression for K c from the balanced equation. Substitute values for equilibrium concentration and calculate K c. Initial – Change – Equilibrium = ICE method

ASG has a dance, and lets 100 boy-girl couples into the gym. Throughout the evening some couples have fights and break apart, forming single boys and single girls. Of course some of these singles form new couples. At the end of the evening there are 12 single girls. Calculate the equilibrium numbers. 1 Couple  1 girl + 1 boy Initial Let’s start with a silly, non-chem example…

ASG has a dance, and lets 100 couples into the gym. Throughout the evening some couples have fights and break apart, forming single boys and single girls. Of course some of these singles form new couples. At the end of the evening there are 12 single girls. Calculate the equilibrium numbers. 1 Couple  1 girl + 1 boy Initial Equilibrium

ASG has a dance, and lets 100 couples into the gym. Throughout the evening some couples have fights and break apart, forming single boys and single girls. Of course some of these singles form new couples. At the end of the evening there are 12 single girls. Calculate the equilibrium numbers. 1 Couple  1 girl + 1 boy Initial Change Equilibrium

ASG has a dance, and lets 100 couples into the gym. Throughout the evening some couples have fights and break apart, forming single boys and single girls. Of course some of these singles form new couples. At the end of the evening there are 12 single girls. Calculate the equilibrium numbers. Equilibrium Couple  1 girl + 1 boy = 1.64

Example: 4 moles of H 2 gas and 6 moles of Cl 2 gas are pumped into a 2 liter tank at 30  C. At some time later, it is found that there are 2 moles of HCl gas in the tank. Calculate the Equilibrium Constant. H 2 + Cl 2  2HCl

Example: 4 moles of H 2 gas and 6 moles of Cl 2 gas are pumped into a 2 liter tank at 30  C. At some time later, it is found that there are 2 moles of HCl gas in the tank. Calculate the Equilibrium Constant. Initial Concentration H 2 + Cl 2  2HCl 0

Example: 4 moles of H 2 gas and 6 moles of Cl 2 gas are pumped into a 2 liter tank at 30  C. At some time later, it is found that there are 2 moles of HCl gas in the tank. Calculate the Equilibrium Constant. Initial Concentration H 2 + Cl 2  2HCl 0[2]

Example: 4 moles of H 2 gas and 6 moles of Cl 2 gas are pumped into a 2 liter tank at 30  C. At some time later, it is found that there are 2 moles of HCl gas in the tank. Calculate the Equilibrium Constant. Initial Concentration H 2 + Cl 2  2HCl Change Equilibrium Conc. 0[2][3]

Example: 4 moles of H 2 gas and 6 moles of Cl 2 gas are pumped into a 2 liter tank at 30  C. At some time later, it is found that there are 2 moles of HCl gas in the tank. Calculate the Equilibrium Constant. Initial Concentration H 2 + Cl 2  2HCl Change Equilibrium Conc. 0[2][3] [1] +1- ½ [1.5][2.5] =  0.3 The changes that occur must be in the same ratio as the co-efficients in the balanced equation

Main Menu

Calculating equilibrium concentrations from the equilibrium constant

Main Menu More complex when you’re only given K c and initial concentrations... Continued on next slide...

Main Menu

Calculating equilibrium concentrations when K c is very small...  In some reactions Kc is very small, less than  This represents a reaction in which the forward reaction has hardly proceeded.

Main Menu

Solutions

Main Menu