Lecture 41/25/06 Quiz Friday Seminar 1:30 on Friday.

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

Equilibrium and Le Chatelier’s Principle

Standard 9: Chemical Equilibrium chapter 18

Section Disturbing a Chemical Equilibrium Le Chatelier’s Principle

Equilibrium Unit 10 1.

Chemical Equilibrium AP Chem Unit 13.

15.1c: Using ICE Tables Predicting Equilibrium Concentrations.

Equilibrium Follow-up

CHEMICAL EQUILIBRIUM Cato Maximilian Guldberg and his brother-in-law Peter Waage developed the Law of Mass Action.

Chemical Equilibrium CHAPTER 15

Chemical Equilibrium - General Concepts (Ch. 14)

Applications of Equilibrium Constants K c and K p can be used to determine the concentration of reactants and/or products at equilibrium.

Equilibrium Chapter 13. What Is It? The state where concentrations of all reactants and products remain constant with time. At the molecular level, the.

Equilibrium Le Chatelier’s Principle. Equilibrium Brown gasColourless gas.

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.

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.

Chemical Equilibrium Objectives: 1. Describe a reversible reaction. 2. Define chemical equilibrium and explain how it is achieved. 3. Explain Le Chatelier's.

Chemical equilibrium. Forward and reverse reactions Not all chemical reactions occur in one direction. They can go “forward” – to the right. They can.

Chemical Equilibrium What is a reversible reaction? What is LeChatlier’s Principle? Predicting Equilibrium Shifts.

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 Equilibria. Manipulating Equilibrium Expressions : N 2 (g) + 3 H 2 (g)  2 NH 3 (g) K = =5.5 x 10 5 Reversing Reactions Multiplying.

Time for… fun with probes!. Chapter 15: Chemical Equilibria.

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

1 Reversible Reactions & Equilibrium reversible reaction A reversible reaction is one which can be made to go in either forward or reverse direction. Only.

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,

Lecture 41/28/05. Quiz 2 1. Given the following reaction: 2 H 2 S (g) ↔ 2 H 2 (g) + S 2 (g) Calculate K c and K p at 1400 K if at equilibrium a flask.

Lecture 72/4/05 Seminar: Monday 2/7 4:30 Room 006 Eric Howe “Untangling sickle-cell anemia and the discovery of heterozygote protection to address students’

Chapter 15: Chemical Equilibria. Manipulating Equilibrium Expressions : N 2 (g) + 3 H 2 (g)  2 NH 3 (g) K = =5.5 x 10 5 Reversing Reactions.

Chemical Equilibrium Chapter 15.

© 2013 Pearson Education, Inc. Chapter 9, Section 1 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 9 © 2013 Pearson.

Chemical Equilibrium PART 2.

Chemical Equilibrium 4/24/2017.

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,

Section 17.3 Application of Equilibria 1.To learn to predict the changes that occur when a system at equilibrium is disturbed 2.To learn to calculate equilibrium.

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

UNIT 12 REVIEW Supplies: Marker Board Marker & Paper Towel Calculator.

Equilibrium. Reversible Reactions Able to proceed in both directions (forward and reverse) PE (kJ) Reaction coordinate Forward AE f Reverse AE r HH.

Equilibrium: Le Chatelier’s Principle

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

CHEMICAL EQUILIBRIUM REVIEW. REVIEW Look at the review objectives and your notes. 1. Describe a reversible reaction.  Be sure you can describe what a.

What is equilibrium? What is equal at equilibrium? What is stable at equilibrium? What must be met for a system to be at equilibrium? Draw a rate vs. time.

Gaseous Chemical Equilibrium. The Dynamic Nature of Equilibrium A. What is equilibrium? a state of balance; no net change in a dynamic process.

Chemical Equilibrium Q, K, and Calculations Chapter 16.

Chapter 16 Chemical Equilibrium. Different States a System Can Be In A state of change A state of change No change (there are several no change states.

1 HOW ARE EQUILIBRIUM EXPRESSIONS WRITTEN? Q VS. K.

What do we know?What do we know?  Direction of reaction to shift for equilibrium  NEED TO KNOW: quantify amount of reactants and products at equilibrium.

Gas Equilibria Unit 10. Equilibrium Reactions are reversible Reactants are not consumed Equilibrium mixture containing both products and reactants is.

K c can be used to find a missing [equilibrium] Exam.14.6(p. 625) 0.3 mol CO, 0.1 mol H 2, 0.02 mol H 2 O, plus an unknown amount of CH 4 in 1L. What is.

U1 s3 L3 Predicting the shift in equilibrium: Q vs K p 517 – 520 The effect of temp on K:p 526 Review Table p 528 Home work: p 519 # p 536 item:

© 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.

Quantitative Changes in Equilibrium Systems Chapter 7.5.

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

CHEMICAL EQUILIBRIUM Dynamic Equilibrium Equilibrium constant expression – K c – K p – Q c Le Chatelier’s principle.

Reversible Reactions and Equilibrium

LeChatelier’s Principle

Equilibrium Suroviec Spring 2014

Assign. #13.3 – Le Chatelier’s Principle

Le Chatelier’s Principle

Equilibrium Part 2.

Le Chatelier's Principle and Equilibrium

Le Chatelier’s Principle

Review: Which type of disturbance happens at t = 2 minutes in each of the following concentration vs. time graphs for the reaction N2O4.

Equilibrium Chapter 19-2.

Shifting Equilibrium.

Unit 7 Vocabulary.

Equilibrium Notes

Equilibrium Constant (Keq)

Presentation transcript:

Lecture 41/25/06 Quiz Friday Seminar 1:30 on Friday

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, mol of SO 3 have been formed. Calculate K Calculate K from concentrations

Skills - recap Need to be able to: Balance a reaction Equilibrium constant expression Make ICE table

Manipulating K Multiply the equation by a constant Reverse equation Add equations

Multiply by a constant 2SO 2 (g) + O 2 (g) ⇄ 2SO 3 (g) K = 283 vs. SO 2 (g) + ½ O 2 (g) ⇄ SO 3 (g) K = ?

Reversing the equation 2SO 2 (g) + O 2 (g) ⇄ 2SO 3 (g) K = 283 vs. 2SO 3 (g) ⇄ 2SO 2 (g) + O 2 (g) K = ?

Adding equations N 2 (g) + O 2 (g) ⇄ 2NO (g) K 1 = 4.3 x NO (g) + O 2 (g) ⇄ 2NO 2 (g) K 2 = 6.4 x 10 9 N 2 (g) + 2O 2 (g) ⇄ 2NO 2 (g) K net = ?

Le Chatelier’s Principle system at equilibrium Disturb equilibrium Shifts system to new equilibrium Ways to disturb equilibrium

Add / Remove  Product /Reactant

Example: For the reaction, PCl 3 (g) + Cl 2 (g) ⇄ PCl 5 (g), the system is at equilibrium when [PCl 3 ] = 0.20 M, [Cl 2 ] = 0.125, [PCl 5 ] = 0.6 M. What is the new equilibrium, if the concentrations of Cl 2 is increased by M?