(7.3) Le Chatelier’s Principle - Regaining Equilibrium.

Slides:

Advertisements

Similar presentations

Equilibrium and Le Chatelier’s Principle

Advertisements

Le Châtelier’s Principle

Le Chatelier’s Principle Chem 12 Chapter 13, Pg

Le Chatelier’s Principle Chem 12 - Unit 3. Le Chatelier’s Principle The French chemist Henri Le Chatelier ( ) studied how the equilibrium position.

Chemical Systems and Equilibrium

Le Châtelier’s Principle

Drill – 5/28 1. Write the equilibrium expression for sulfuric acid.

Concentration and Temperature.  If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.  Stresses.

Disturbing Equilibrium and Non-equilibrium conditions

Equilibrium Systems and Stress. Chemical Equilibrium  When the rates of the forward and reverse reactions are equal in a chemical reaction  The concentration.

Section 8.4—Le Chatelier’s Principle How can we push a reaction to make more products?

We can qualitatively predict the effects of changes in concentration, pressure, and temperature on a system at equilibrium by using Le Chatelier’s principle.

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

Le Chatelier’s Principle Ways to change rate of reaction: 1. Change concentration 2. Change temperature 3. Add a catalyst 4. Increase the surface area.

Equilibrium Chemistry 30.

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

EQUILIBRIUM TIER 4 Apply LeChatelier’s principle to predict the qualitative effects of changes of temperature, pressure and concentration on the position.

Le Chatelier’s Principle. When a system at equilibrium is placed under stress, the system will undergo a change in such a way as to relieve that stress.

Qualitative Changes in Equilibrium Systems. Le Châtelier’s Principle Le Châtelier’s Principle – chemical systems at equilibrium shift to restore equilibrium.

If a stress is applied to a system at equilibrium, the position of the equilibrium will shift to reduce the stress This shift occurs because the stress.

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

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.

Le Chatelier’s principle and more

Le Chatelier’s Principle The 4 most commons changes to make for equilibrium reactions are: 1. Concentration changes for reactants 2. Concentration changes.

Le Chatelier’s Principle  A reaction at equilibrium, when “stressed,” will react to relieve the stress.  (If you mess with it, it will work to return.

Le Chatelier's Principle. What if the conditions of the equilibrium changed? Le Chatelier’s principle states that if a closed system at equilibrium is.

Le Châtelier’s Principle. If a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. Stress is anything.

Factors Affecting Equilibrium Chapters 18 When a system is at equilibrium, it will stay that way until something changes this condition.

LeChâtelier’s Principle Regaining Equilibrium 6-2.

Preview Lesson Starter Objectives Predicting the Direction of Shift Reactions That Go to Completion Common-Ion Effect Chapter 18 Section 2 Shifting Equilibrium.

Le Chatelier’s Principle.  When a chemical system at equilibrium is disturbed by a change in a property of the system, the system always appears to react.

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

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.

Le Chatelier’s Principle Ways to change rate of reaction: 1. Change concentration 2. Change temperature 3. Add a catalyst 4. Increase the surface area.

15.2: Le Châtelier’s Principle.  can predict how certain changes in a reaction will affect the position of equilibrium  when a chemical system at equil.

When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance (the system will respond to relieve.

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.

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

Reaction Rates and Le Chatelier’s Principle

Chemical Equilibrium. NO 2 N 2 O 4 Le Châtelier’s Principle When a stress is applied to a system at equilibrium, the equilibrium shifts to relieve.

Chemical Equilibrium. Unit Objectives  Define chemical equilibrium.  Explain the nature of the equilibrium constant.  Write chemical equilibrium expressions.

Equilibrium Le Chatelier's Principle - if a change in conditions, a stress is imposed on a reversible reaction at equilibrium, the equilibrium will shift.

Chapter 7.4 Qualitative Changes in Equilibrium Systems

Reaction Rates and Le Chatelier’s Principle

Le Chatelier’s Principle

LeChatelier’s Principle

Le chÂtelier’s principle

Le’ Chatelier’s Principle

Le Chatelier’s Principle

Le Chatelier’s Principle

LECTURE 9.5 – LE CHATELIER’S PRINCIPLE

What is Le Châtelier’s Principle (LCP)?

Le Châtelier’s Principle

Le Chatelier’s Principle

Le Chatelier’s Principle

Le Chatelier’s Principle

Le Chatelier’s Principle

Le Chatelier’s Principle and Equilibrium

Le Chatelier’s Principle Chapter 11

Le Chatelier’s Principle

Chapter 18: Chemical Equilibrium

18-2 Shifting Equilibrium

What is Le Châtelier’s Principle (LCP)?

Shifting Equilibrium.

CHEMICAL EQUILIBRIUM:

Equilibrium Notes

Qualitative Changes in Equilibrium Systems

Presentation transcript:

(7.3) Le Chatelier’s Principle - Regaining Equilibrium

Le Chatelier’s Principle Le Chatelier's Principle states: If something is changed in a system at equilibrium, the system shifts in equilibrium composition in order to counteract (or oppose) this change.

Le Chatelier’s Principle A change imposed on an equilibrium system is called a stress. There are 3 types of stress: 1)Changing concentration 2)Changing temperature 3)Changing pressure (for gases) The equilibrium always responds in such a way so as to counteract the stress.

Concentration Changes If concentration is increased - eqm shifts to consume some of the added reactant or product If concentration is decreased - eqm shifts to replace some of the removed reactant or product e.g. 2A (g) ↔2B (g) + C (g) kJ - If A is added, eqm shifts right - If B is added, eqm shifts left - If A is removed, eqm shifts left

Temperature Changes If temperature is increased - eqm shifts to consume some of the added thermal energy If temperature is decreased - eqm shifts to replace some of the removed thermal energy Energy in chemical eqm equation is treated as a reactant (endothermic) or product (exothermic) e.g. 2A (g) ↔2B (g) + C (g) kJ - If temperature is reduced, eqm shifts right - If temperature is increased, eqm shifts left e.g. X (g) kJ ↔ Y (g) - If temperature is increased, eqm shifts right

Gas Volume Changes To predict whether a change in pressure will affect eqm, consider total moles of gas reactant and total moles of gas products. e.g. 2A (g) ↔ 2B (g) + C (g) kJ (2 moles) (3 moles) If volume is increased (pressure is decreased) - eqm shifts toward the side with the larger number of moles of gaseous entities e.g. eqm shifts right If volume is decreased (pressure is increased) - eqm shifts toward in the direction that has the smaller number of moles e.g. eqm shifts left Note – In some cases the eqm will not shift because n reactants = n products

Other Effects? Adding catalyst - affects only how fast reaction reaches eqm - no effect on eqm Nature of Reactants - only effect is how fast reaction reaches equilibrium - no effect on eqm Adding inert gases - no effect on eqm See Summary Table p 456