Chemical Equilibrium Chapter 14.2 & 14.3.

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

Ch. 14: Chemical Equilibrium Dr. Namphol Sinkaset Chem 201: General Chemistry II.
1 CHEMICAL EQUILIBRIUM. Chemical Equilibrium Chemical Reactions Types; What is equilibrium? Expressions for equilibrium constants, K c ; Calculating K.
Equilibrium Chemistry. Equilibrium A + B  AB We may think that all reactions change all reactants to products, or the reaction has gone to completion.
Section 8.1—Equilibrium What is equilibrium?. Reversible Reactions Reversible Reaction – A chemical reaction that can proceed in both direction (represented.
Chapter 8: Chemistry in Industry. Introductory Activity What do you think a chemical engineer does? What do you think are a chemical manufacturer’s main.
EQUILIBRIUM BASICS Chapter Lesson Objectives Know -Factors that affect/don’t affect a reaction reaching equilibrium -K is equilibrium constant.
Equilibrium: A State of Dynamic Balance Chapter 18.1.
Chapter 13.  Equilibrium is not static. It is a highly dynamic state.  Macro level reaction appears to have stopped  Molecular level frantic activity.
Chapter: Chemical Reactions Table of Contents Section 1: Chemical Formulas and Equations What you will learn and why is it important: page 492.
Chemical Equilibrium. n In systems that are in equilibrium, reverse processes are happening at the same time and at the same rate. n Rate forward = Rate.
The Concept of Dynamic Equilibrium – The Equilibrium Constant (K)
Chapter 14:Chemical Equilibrium Dynamic Equilibrium and the Equilibrium Constant.
“K” Chemistry (part 2 of 3) Chapter 14: Chemical Equilibrium.
Chapter 14 Lecture © 2014 Pearson Education, Inc. Sherril Soman Grand Valley State University Lecture Presentation Chapter 14 Chemical Equilibrium.
1 Equilibrium Constant even though the concentrations of reactants and products are not equal at equilibrium, there is a relationship between them the.
Balancing Chemical Equations
Balancing Chemical Equations
Chapter 13 Equilibrium Dr. Walker DE Chemistry.
Balancing Chemical Equations
Balancing Chemical Equations
Chapter 9 Chemical Equilibrium
Balancing Chemical Equations
Balancing Chemical Equations
Solving Linear Equations and Inequalities
Reversible Reactions and Equilibrium
Balancing Equations Review
Balancing Chemical Equations
Law of Conservation of Mass through Balancing Equations
Balancing Chemical Equations
Warm up Take out the handout on ionic and covalent bonding
Ppt 808 EQUILIBRIUM: IS ESTABLISHED WHEN THE RATE OF THE FORWARD REACTION EQUALS THE REVERSE RATE. AT EQUILIBRIUM THE MOLARITIES OF ALL SPECIES ARE STABLE,
Writing and Solving Equilibrium Constant Expressions
Balancing Chemical Equations
Balancing Chemical Equations
Chemical Reactions.
CHEMICAL EQUILIBRIUM.
Balancing Chemical Equations
Section 8.1—Equilibrium What is equilibrium?.
Dynamic Equilibrium and the Equilibrium Constant
Approaching Equilibrium Lesson 1.
Reaction Rate.
Chemical Equilibrium.
Section 8.1—Equilibrium What is equilibrium?.
CHEMICAL EQUILIBRIUM.
Reversible Reactions and Equilibrium
Balancing Chemical Equations
Balancing Chemical Equations
Balancing Chemical Equations
Balancing Chemical Equations
Review When converting FROM moles you MULTIPLY.
Balancing Chemical Equations
Chapter 15 Chemical Equilibrium -occurs when opposing reactions proceed at equal rates -no reactant or product is escaping -when at equilibrium, conc.
Balancing Chemical Equations
Reaction rates and equilibrium
4.2 Combinations of Atoms.
Chemical Reactions Section 2.2.
Approaching Equilibrium Lesson 1.
Equilibrium.
Balancing Chemical Equations
Balancing Chemical Equations
Chapter 14 Chemical Equilibrium 14.2–14.3
Balancing Chemical Equations
Balancing Chemical Equations
Balancing Chemical Equations
Reversible Reactions Some reactions may be reversible –the conversion of reactants to products and the conversion of products to reactants occur simultaneously.
Equilibrium Constant (Keq)
Balancing Chemical Equations
Balancing Chemical Equations
Chapter 16 Chemical Equilibrium
Presentation transcript:

Chemical Equilibrium Chapter 14.2 & 14.3

Dynamic Equilibrium Is the point at which the forward and reverse rates of a reaction are equal to each other Is represented in equations by a double arrow in a reaction Ex. 2H2+O2 ⇌ 2H2O In addition to equal rates concentrations become stable on both sides of the equation Although rates are equal concentrations at equilibrium are not equal

How to look at a Reaction Considering Dynamic Equilibrium Beginning Only reactant molecules exist so only reactant molecules collide, there is only the forward reaction happening Middle Concentration of the product(s) is increasing so collisions increase causing reverse reaction Equilibrium Collisions are happening at the same rate on both sides

What Does This Look Like Graphically?

Equilibrium Constant (K) The equilibrium constant (K) is the way to quantify the concentrations at equilibrium and how far the reaction proceeds after equilibrium K>>1 means the forward reaction is favored and there are high concentration for products and low concentration for reactants, forward reaction proceeds fully K<<1 means the reverse reaction is favored and there are low concentrations for products and high concentration for reactants, forward reaction doesn’t proceed far K≈1 means neither is favored and the reaction proceeds about half way

How to find K To find K we use the Law of Mass Action Using the base equation aA+bB⇌cC+dD where lowercase represent coefficients we divide the concentration of the products by that of the reactants while all values are raised to their respective coefficients as following Note that this formula is in your reference tables at the top of the section labeled Equilibrium

Changes to the Equilibrium Constant When the base equation you are working with needs to be modified in some way the equilibrium constant must be change to account for the modifications There are three common modifications Reversing the equation Adjusting coefficients Adding multiple equations together

Adjusting the Constant When reversing the equation invert the equilibrium constant When adjusting coefficients (multiplying the coefficients by a factor) raise the equilibrium constant to the same factor When combining equations find the individual constants then multiply them together to obtain an overall equilibrium constant for the combined equation

What the college board says

Find the Equilibrium constant for the following equation 2H2S(g)⇌2H2(g) + S2(g) K=[H2]² [S2] / [H2S]²

Consider the reaction A(g)⇌ B(g) where K=10 If initially [A]=1.1M and [B]=0.0M which of the following would be the result at equilibrium? [A]=1.0M and [B]=0.1M 2. [A]=0.1M and [B]=1.0M 3. Concentrations will be equal

Consider the following reaction and solve for K 2A + B ⇌ C + 2D Where the concentrations at equilibrium are 0.100M , 0.600M, 0.200M and 0.400M respectively. [0.200][0.400]²/[0.100]²[0.600] = K K= 5.33 And if we reverse the reaction? [0.100]²[0.600]/[0.200][0.400]² K=.1875