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.

Slides:

Advertisements

Similar presentations

Keq vs. Q Period 2 Sandra.

Advertisements

Keq vs. Q Javell, Shantell, Akosua

Equilibrium. Equilibrium Some reactions (theoretically all) are reversible reactions, in which the products take part in a separate reaction to reform.

The Equilibrium Law.

Sulfur trioxide is an important precursor to the production of sulfuric acid on an industrial level. The equation of the chemical reaction is given below.

Chemical Equilibrium Chapter 18. Chemical Equilibrium Happens to any reversible reaction in a closed system Happens to any reversible reaction in a closed.

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.

Chemical Equilibrium Introduction to the Law of Mass Action.

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

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

15.1b Equilibrium Constant, K c. created in 1864 by Guldberg and Waage (Norweigen) for a reaction: aA + bB ⇄ cC + dD equilibrium constant: K c.

Chapter 18 Equilibrium A + B  AB We may think that all reactions change all reactants to products, or the reaction has gone to completion But in reality,

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.

Chemical Equilibrium. Rate of forward Rx = Rate of reverse Rx As a system approaches equilibrium, both the forward and reverse reactions are occurring.

AA + bB cC + dD Equilibrium RegionKinetic Region.

Lecture 21/21/05. Law of Mass Action Example H 2 (g) + I 2 (g) ↔ 2HI (g)

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.

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

Equilibrium Math Concepts

Section 8.3—Reaction Quotient

 To simplify expressions containing positive integral exponents.  To solve exponential equations.

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 Constant - 1.  Please READ pp. 439 – 440  Equilibrium constant (K eq ) is the value obtained from the mathematical combination of equilibrium.

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

Equilibrium: A State of Dynamic Balance Chapter 18.1.

Equilibrium Constant (K eq ) A constant which can tell you which side of an equilibrium is favored under certain conditions. A constant which can tell.

1.Equilibrium Equilibrium 2. The Formula 3. Applying the Formula 4. How that applies to Solubility.

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 15 Equilibrium. Equilibrium N H 2  2 NH 3 N H 2  2 NH 3 Both reactions occur, Both reactions occur, Closed system Closed system.

Reaction Rates Measures concentration (molarity!) change over time Measures concentration (molarity!) change over time Example: Example: 2H 2 O 2  2H.

Chemical Equilibrium Q, K, and Calculations Chapter 16.

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.

Balancing Chemical Equations

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.

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

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

Exponents and Monomials. Monomial is an expression that is a number, a variable, or a product of a number and variables. Constant is a monomial containing.

Quantitative Changes in Equilibrium Systems Chapter 7.5.

Q is the reaction quotient Gives the condition of the reaction at any point during the reaction. [X] o indicates the initial concentration of a species.

Equilibrium Expressions. Equilibrium When the rate of the forward and reverse reactions are equal. The equilibrium constant K eq is a value that shows.

Equilibrium -Keq.

THE EQUILIBRIUM CONSTANT CHAPTER 18 PAGES

Pick up notes. Get out Study Guide for Content Mastery. DO NOW.

Law Conservation of Mass and Balanced and Unbalanced Equations

CHEMICAL EQUILIBRIUM.

Equilibrium Constant Kc = [C]c[D]d [A]a[B]b

A reaction reaches equilibrium

Writing and Solving Equilibrium Constant Expressions

Chapter 17: Chemical Equilibrium

Equilibrium Expressions mass-action expression

Unit 2, Lesson 10: Equilibrium Calculations – Part II

“Products over reactants, the coefficients are the powers”

Chapter 16 Equilibrium.

Announcements Review session: 5:00pm Study Guide on web site

Michael Grab, “Gravity Glue”

Chemical Equilibrium Chapter 11

Predicting Equilibrium

The Extent of a Reaction

Kinetics Lesson # 3 Rate Law.

EQUILIBRIUM LAW.

9.2 Equilibrium Constant and Reaction Quotient Obj S1:e-g

Parts of an Expression EE2b. Identify parts of an expression using mathematical terms (sum, term, product, factor, quotient, coefficient).

Equilibrium Constants

Reaction Equilibrium.

Pick up the notes. Get out your homework handouts. DO NOW.

Equilibrium Constant (Keq)

Unit 13: Equilibrium 13.1 Equilibrium 13.2 Le Chatelier’s Principle

Presentation transcript:

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 reaction at a given time before equilibrium to know in which direction the reaction goes.

What are the definitions? Keq: Law of mass action express the relative concentration of reactants and products at equilibrium in terms of quantity called the equilibrium constant Q: The reaction Quotient of Keq

Steps/Rules Keq: 1. Balance the equation 2.Put the products on top and the reactants on the bottom 3.coefficients are exponents 4.only use (g) and (aq) 5. Use the M of reactants and products to find keq. Keq>>1= reaction lies to the right Keq<<1= reaction lies to the left Keq=1 at equilibrium

More Steps and Rules Q: 1. Do all for Keq 2.Use given M at given temperature. 3.Compare with value of Keq. Q<Keq= reaction lies to the right (product side) Q>Keq= reaction lies to the left (reactant side)

A solved EXAMPLE (Keq) 2CO(g) + O2 (g) ↔ 2CO2 (g) Keq = [CO2]^2/ [CO]^2 [O2] (Q) COCL2(g) ↔ CO(g) Cl2(g) and Keq =170. If the concentration of CO and C2 are each 0.15M and the concentration of COCL2 is 1.1 x 10^-3 is the reaction at equilibrium? [CO][Cl2] / [COCl2] = (.15)(.15)/1.1x10^-3 = 20 Q=20

Here's Something to SOLVE >:) Keq: NH4NO3 (s) ↔ N2O(g) + H2O Q: At 448 degrees C K= 50.5 for the reaction H2(g) + I2(g) ↔ 2HI (g), Find Q and the direction of the reaction of the reaction if [H2] = .15 M, [I2] = .175 M, [HI] = .950 M.

Here are the answers @_@ Keq = [N2O][H20]^2 Q= 34.4. Reaction lies to the right.