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

Slides:

Advertisements

Similar presentations

For an ideal gas, molarity is directly proportional to pressure M = P

Advertisements

Equilibrium Unit 10 1.

ICE Tables I nitial (Concentrations) C hange E quilibrium (Concentrations)

Equilibrium Follow-up

ADVANCED PLACEMENT CHEMISTRY EQUILIBRIUM. Chemical equilibrium * state where concentrations of products and reactants remain constant *equilibrium is.

Equilibrium Chapter 15. At room temperature colorless N 2 O 4 decomposes to brown NO 2. N 2 O 4 (g)  2NO 2 (g) (colorless) (brown)

Chemical Equilibrium Chapter 6 pages Reversible Reactions- most chemical reactions are reversible under the correct conditions.

Chemical Equilibrium - General Concepts (Ch. 14)

Chemistry. Chemical equilibrium-I Session Objectives.

A.P. Chemistry Chapter 13 Equilibrium Equilibrium is not static, but is a highly dynamic state. At the macro level everything appears to have stopped.

Chapter 13 Equilibrium. Unit Essential Question Z How do equilibrium reactions compare to other reactions?

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Equilibrium The state where the concentrations of all reactants and products.

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.

Chemical Equilibrium The study of reactions that occur in both directions.

Equilibrium Constant. Example H 2 + F 2  2HF The equilibrium constant for the reaction above is found to be 2.1 x 10 3 at a specific temperature. At.

Chemistry 1011 TOPIC TEXT REFERENCE Gaseous Chemical Equilibrium

Equilibrium Chemical reaction in which reactants are forming as fast as products yet the net concentrations of each remains constant A + B  C + D N 2.

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.

Lecture 41/24/07 Quiz Friday. Manipulating K Multiply the equation by a constant Reverse equation Add equations.

Chemical Equilibrium Chapter 15. aA + bB cC + dD K C = [C] c [D] d [A] a [B] b Law of Mass Action Must be caps! Equilibrium constant Lies to the rightLies.

Equilibrium Basic Concepts Reversible reactions do not go to completion. –They can occur in either direction Chemical equilibrium exists when two opposing.

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,

Chemical Equilibrium Introduction to Chemical Equilibrium Equilibrium Constants and Expressions Calculations Involving Equilibrium Constants Using.

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.

and cooking with chemicals

Gases The Ideal Gas Law.  Objectives  State the ideal gas law  Using the ideal gas law, calculate pressure, volume, temperature, or amount of gas when.

Chemical Equilibrium The big one!! This is your first required FRQ on the AP test.

Chapter #11 Molecular Composition of Gases. Chapter 11.1 Gay-Lussac’s law of combining volumes of gases states that at constant temperature and pressure,

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.

Chapter 13 Chemical Equilibrium  The state where the concentrations of all reactants and products remain constant with time  Equilibrium is reached.

Some reactions go to completion Some reactions go to completion A precipitate forms A precipitate forms A gas forms A gas forms CH 4 (g) + O 2 (g)  CO.

Predicting if a Reaction is in Equilibrium Trial Keq Lesson 9.

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.

Chemical Equilibrium The state where the concentrations of all reactants and products remain constant with time. On the molecular level, there is frantic.

Chapter 13 Chemical Equilibrium The state where the concentrations of all reactants and products remain constant with time. On the molecular level, there.

Chapter 13.  Equilibrium is not static. It is a highly dynamic state.  Macro level reaction appears to have stopped  Molecular level frantic activity.

A more appropriate definition of K (for the same chemical reaction discussed previously) is With this definition, each concentration term is divided by.

Chapter 12: Chemical Equilibrium. The Dynamic Nature of Equilibrium A. What is equilibrium? 1. Definition a state of balance; no net change in a dynamic.

Review 2 Chapter 16 Chemical Equilibrium. Equilibrium Condition: Study equilibrium tells us more about whether a reaction will occur or not. Closed system.

6-3:Calculating Equilibrium Constants: The actual value of K eq is found experimentally. The individual concentrations of all the reactants is calculated,

6-4. Steps for solving equilibrium problems: 1. Write out the equation. 2. Balance the equation if it is not. 3. Make a chart. (ICEBOX) I – initial C.

CHAPTER 14 Chemical Equilibrium. 14.1: Equilibrium Constant, K eq  Objective: (1) To write the equilibrium constant expression for a chemical reaction.

Chapter 14: Chemical Equilibrium Sections Sarah Rodriguez.

Chemical Equilibrium Q, K, and Calculations Chapter 16.

C h a p t e r 13 Chemical Equilibrium. The Equilibrium State01 Chemical Equilibrium: A state achieved when the rates of the forward and reverse reactions.

What is equilibrium?What is equilibrium? Chemical reaction stops BEFORE the limiting reactant is consumed. All of the reactants are not COMPLETELY.

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

Stoichiometry and cooking with chemicals.  Interpret a balanced equation in terms of moles, mass, and volume of gases.  Solve mole-mole problems given.

Equilibrium Chemistry— Introduction. Chemical Equilibrium State for a chemical reaction where the reaction stops BEFORE all of the limiting reactant has.

Chapter 15; CHEMICAL EQUILIBRIUM 14 | 1 Describing Chemical Equilibrium Chemical Equilibrium—A Dynamic Equilibrium The Equilibrium Constant Heterogeneous.

Applications of the Equil. Constant Predicting the direction of approach to equilibrium: At 448C the equilibrium constant kc for the reaction H 2 (g) +

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

When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes. Section 3: Gas Stoichiometry K.

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.

13.1 EQUILIBRIUM CONDITION CHEMICAL EQUILIBRIUM The state where the concentrations of all reactants and products remain constant with time. On the molecular.

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

© 2009, Prentice-Hall, Inc. The Reaction Quotient (Q) Q gives the same ratio the equilibrium expression gives, but for a system that is not necessarily.

Chapter 15 Chemical Equilibrium. Equilibrium - Condition where opposing processes occur at the same time. - Processes may be physical changes or chemical.

Ch 12.2 Chemical Calculations

10.3 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

Chapter 13 Reaction Rates and Chemical Equilibrium

Equilibrium Expressions mass-action expression

Chapter 17 Chemical Equilibrium.

Value for K Large K (>1) = equilibrium will contain mostly products (equilibrium position is to the right) Small K (

Introduction to Equilibrium

Presentation transcript:

Equilibrium

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

Objectives To calculate K c, the equilibrium constant, for a reaction To define K p To calculate K p from the value of K c CLE3221.Inq.2

Evaluating K c When we know the equilibrium concentrations of N 2 O 4 and NO 2 in the reaction below, we can calculate K c, the equilibrium constant. N 2 O 4 (g)  2NO 2 (g)

If [NO 2 ] at equilibrium is.0172 M, and the [N 2 O 4 ] at equilibrium is M, we calculate K c with the following equation: N 2 O 4 (g)  2NO 2 (g) K c = [NO 2 ] 2 = (0.0172) 2 = [N 2 O 4 ] ( ) Notice that we will not include units when we calculate K c.

Study Check The following reaction is at equilibrium: H 2 (g) + I 2 (g)  2HI(g) [H 2 ] = M, [I 2 ] = 0.15 M, and [HI] = 0.30M. Calculate K c for this reaction.

Equilibrium Constants in Terms of Pressure, K p When the reactants and products in a chemical reaction are gases, we can use partial pressures instead of molarities to calculate the equilibrium constant. If we do this, we call the constant K p to show that we used partial pressures in our calculation.

Study Check What is the difference between K c and K p ?

Calculating K p N 2 O 4 (g)  2NO 2 (g) K p = [P NO2 ] 2 [P N2O4 ] If given the partial pressures of N 2 O 4 andNO 2, we would just substitute them into the equation.

When we are given the value of K c and we want to find K p, we can use the following equation: K p = K c (RT) /\n R= ideal gas constant, L-atm/mol-K T= temperature in Kelvins /\n= (moles of gaseous product) – (moles of gaseous reactant)

Calculating /\ n To calculate /\ n, the change in moles when all reactants and products are gases, you subtract the moles of reactants from the moles of your product. The coefficients in the balanced equation are used to do this. PCl 5 (g)  PCl 3 (g) +Cl 2 (g) /\n= (moles of gaseous product) – (moles of gaseous reactant) /\ n= (1+1) - 1 = 1

Study Check For the following reaction, calculate K p when K c = 9.60 at 573 K. N 2 (g) + 3H 2 (g)  2NH 3 (g)

K c = 9.60 at 573 K. K p = K c (RT) /\n R= ideal gas constant, L-atm/mol-K T= temperature in Kelvins /\n= (moles of gaseous product) – (moles of gaseous reactant)

Homework p. 660 in your book Problem a,b,c,d,e Problem 15.17