Chemical Equilibrium Chapter 15. 15.8 Write the expressions for the equilibrium constants K P of these thermal decompositions:

Slides:

Advertisements

Similar presentations

Equilibrium Unit 10 1.

Advertisements

Chemical Equilibrium AP Chem Unit 13.

Equilibrium Follow-up

Chemical Equilibrium A Balancing Act.

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

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

TIER 6 Combine the knowledge of gases and solutions to perform stoichiometric calculations.

1) In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the.

Disturbing Equilibrium and Non-equilibrium conditions

Introduction to Chemical Equilibrium Chapter 15 CHEM 160.

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

Chapter 14 Chemical Equilibrium

Chapter 18 Reaction Rates and Equilibrium 18.3 Reversible Reactions

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.

THE STATE OF CHEMICAL EQUILIBRIUM Chemical Equilibrium: The state reached when the concentrations of reactants and products remain constant over time.

Chapter 18: Chemical Equilibrium

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.

CHEMICAL EQUILIBRIUM …….occurs when the forward and reverse reactions progress at the same rate in a reversible reaction, i.e. dynamic equilibrium. ……..is.

Chemical Equilibrium Chapter 14.

Chemical Equilibrium Chapter 13.

Chemical Equilibrium The reversibility of reactions.

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.

CH 18: CHEMICAL EQUILIBRIUM. SECTION 18.2 SHIFTING EQUILIBRIUM.

Chemical Equilibrium Chapter 6 Web-site:

Chemical Equilibrium Unit 11. My Chemistry Presentation Chemical Reactions We usually think of chemical reactions as having a beginning and an end. reactants.

CHEMICAL EQUILIBRIA GENERAL CONCEPTS.

Factors that Affect Equilibrium Concentrations!. 2 Le Chatalier’s Principle The first person to study and comment on factors that change equilibrium concentrations.

Chapter 9: Chemical Equilibrium The forward and reverse reaction are both taking place at the same rate.

Chemical Equilibrium Chapter 15.

Chemical Equilibrium The reversibility of reactions.

Chemical Equilibrium PART 2.

Equilibrium slideshttp:\\asadipour.kmu.ac.ir1.

Chemical Equilibrium 4/24/2017.

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,

CHEMICAL EQUILIBRIUM - RATES OF REACTION k F Reactants  products k B Chemical reactions are a dynamic process, that is, reactions involve both forward.

Chapter 15 Chemical Equilibrium 1. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same.

Copyright ©2009 by Pearson Education, Inc. Upper Saddle River, New Jersey All rights reserved. Introductory Chemistry, Third Edition By Nivaldo J.

8–1 John A. Schreifels Chemistry 212 Chapter 15-1 Chapter 15 Chemical Equilibrium.

Calorimetry. Calculating Heat Q can be found experimentally by measuring the heat flow accompanying a reaction This is done by measuring temperature This.

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

Chapter 16 Chemical Equilibrium.

Energy transformations

LeChâtelier’s Principle Regaining Equilibrium 6-2.

Chapter 15 Chemical Equilibrium

Chemical equilibrium By Dr. Hisham Ezzat Abdellatef Professor of Pharmaceutical Analytical Chemistry First Year

Heterogeneous Equilibria: A homogenous reaction is one in which all the substances are in the same state. A heterogeneous reaction is one in which all.

1 Chemical Equilibrium Chapter 14 Henri L. le Chatlier Adapted thermodynamics to equilibria; formulated the principle known by his name.

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.

CHAPTER FIFTEEN Copyright © Tyna L. Gaylord All Rights Reserved 1.

AP Chemistry Chapter 15 Jeopardy Jennie L. Borders.

V. Equilibrium Problems 2 main categories of equilibrium problems:  Finding K c or K p from known equilibrium concentrations or partial pressures  Finding.

Gaseous Equilibrium Equilibrium systems are reaction systems that are reversible. Reactants are not completely consumed causing the reaction system to.

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]

Do Now 1.What is reaction rate? 2.What does the term “equilibrium” signify? Can you describe physical changes in the chemistry lab where equilibrium is.

Equilibrium.  In equilibrium, the concentrations of the chemical species are constant, not necessarily equal.  Equilibrium constants:  K = equilibrium.

Chemical Equilibrium Unit 11. My Chemistry Presentation Chemical Reactions We usually think of chemical reactions as having a beginning and an end. reactants.

Chapter 13 Chemical Equilibrium. The Concept of Equilibrium Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate.

Chapter Fourteen Chemical Equilibrium.

Chapter 15 Chemical Equilibrium

Chapter Fourteen Chemical Equilibrium.

Chemical Equilibrium Chapter 6

Equilibrium Practice.

Chemical Equilibrium What is equilibrium? Expressions for equilibrium constants, K c ; Calculating K c using equilibrium concentrations; Calculating equilibrium.

Chemical Equilibrium.

Chapter 17 Chemical Equilibrium.

Presentation transcript:

Chemical Equilibrium Chapter 15

15.8 Write the expressions for the equilibrium constants K P of these thermal decompositions:

15.14 Consider the following equilibrium process at 700 o C: Analysis shows that there are 2.50 moles of H 2, 1.35 x mole of S 2, and 8.70 moles of H 2 S present in a 12.0-L flask at equilibrium. Calculate the equilibrium constant K c for the reaction.

15.32 A sample of pure NO 2 gas heated to 1000 K decomposes: The equilibrium constant K P is 158. Analysis shows that the partial pressure of O 2 is 0.25 atm at equilibrium. Calculate the pressure of NO and NO 2 in the mixture.

15.48 Consider the equilibrium process: Predict the direction of the shift in equilibrium when (a) the temperature is raised, (b) more chlorine gas is added to the reaction mixture, (c) some PCl 3 is removed from the mixture, (d) the pressure on the gases is increased, and (e) a catalyst is added to the reaction mixture.

15.52 Consider the reaction at equilibrium in a closed container: What would happen if (a) the volume is increased, (b) some CaO is added to the mixture, (c) some CaCO 3 is removed, (d) some CO 2 is added to the mixture, (e) a few drops of an NaOH solution are added to the mixture, (f) a few drops of an HCl solution are added to the mixture (ignore the reaction between CO 2 and water), and (g) the temperature is increased.

Practice exercise, p. 491 The equilibrium constant (K c ) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine is 6.5 x 10 4 at 35 o C. In a certain experiment, 2.0 x mole of NO, 8.3 x mole of Cl 2, and 6.8 moles of NOCl are mixed in a 2.0-L flask. In which direction will the system proceed to reach equilibrium?