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.

Slides:



Advertisements
Similar presentations
AP Notes Chapter 16 Equilibrium Dynamic chemical system in which two reactions, equal and opposite, occur simultaneously.
Advertisements

Equilibrium. Equilibrium Some reactions (theoretically all) are reversible reactions, in which the products take part in a separate reaction to reform.
Equilibrium Unit 10 1.
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.
Disturbing Equilibrium and Non-equilibrium conditions
Solving Equilibrium problems using the RICE method.
TOPIC A: EQUILIBRIUM Equilibrium, Le Chatelier’s Principle, Acid- Base Equilibrium, Ksp, pH.
Chemical Equilibrium – Part 2b GD: Chpt 7 (7.2, 17.2); CHANG: Chpt 14 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction.
Stoichiometry 2 slices bread + 1 slice ham  1 ham sandwich.
Equilibrium Entry Task: Jan 8 th Tuesday At 1100 K, K p = 0.25 atm  1 for the reaction: 2 SO 2 (g) + O 2 (g) ↔ 2 SO 3 (g) What is the value of Kc at this.
Chapter 14 Chemical Equilibrium
Chapter 16: Chemical Equilibrium- General Concepts WHAT IS EQUILIBRIUM?
Equilibrium.  Equilibrium is NOT when all things are equal.  Equilibrium is signaled by no net change in the concentrations of reactants or products.
ANNOUNCEMENTS Reminder- Exam #3 is on Friday (April 23 rd ) Review session: Wednesday, April 21 5:00pm.
Chemical Equilibrium Chapter 13.
Chemical Equilibrium Chapter 18 Modern Chemistry
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 109/21/05. Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Stoichiometric Calculations.
Problem Set Sulfuryl Chloride Equilibria. Gaseous Equilibrium Edward A. Mottel Department of Chemistry Rose-Hulman Institute of Technology.
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 41/25/06 Quiz Friday Seminar 1:30 on Friday.
Sample Exercise 15.7 Calculating K When All Equilibrium Concentrations Are Known After a mixture of hydrogen and nitrogen gases in a reaction vessel is.
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.
and cooking with chemicals
Chemistry Chapter 12 – Quantitative Equilibrium Teacher: H. Michael Hayes.
Chemical Equilibrium CHAPTER 15 Chemistry: The Molecular Nature of Matter, 6 th edition By Jesperson, Brady, & Hyslop.
Equilibrium. How do we write the equilibrium constant expression for the following reaction? 2SO 2 (g) + O 2 (g)  2SO 3 (g)
I. the temperature of the system II. the nature of the reactants and products III. the concentration of the reactants IV. the concentration of the products.
Chemical Equilbrium Chemistry in Two Directions. Chemical Reactions Up until now, we have talked about reactions as though they proceed in one direction:
Solving Limiting Reactant Problems. Background In limiting reactant problems, we have the amounts (masses or mols) of two of the reactants. The problem.
Chemical Equilibrium PART 2.
Chemical Equilibrium………..  Let’s look at problem #12 in the homework….  The reaction of elemental hydrogen and fluorine to form hydrofluoric acid has.
1 Chapter 12: Day 5 Ch12_stoic. 2 STOICHIOMETRY CALCULATIONS Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Molar mass.
Chemical Equilibrium 4/24/2017.
Chemical Equilibrium Chemistry in Two Directions 1.
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,
Kp When the reactants and products are gases, we can determine the equilibrium constant in terms of partial pressures. Dalton’s Law of Partial Pressures.
Chemical Calculations Stoichiometry OBJECTIVES: – Calculate stoichiometric quantities from balanced chemical equations using units of moles and mass.
Reactions are reversibleReactions are reversible  A + B C + D ( forward)  C + D A + B (reverse)  Initially there is only A and B so only the forward.
Energy transformations
Sections 15.3 Using Equilibrium Constants in Calculations Bill Vining SUNY Oneonta.
1.Equilibrium Equilibrium 2. The Formula 3. Applying the Formula 4. How that applies to Solubility.
Chemical Equilibrium Chapter Write the expressions for the equilibrium constants K P of these thermal decompositions:
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.
Chemical Equilibrium Q, K, and Calculations Chapter 16.
The Extent of a Reaction The tendency for a reaction to occur is indicated by the magnitude of the equilibrium constant. A value of K larger than 1 means.
Equilibrium Chemistry— Introduction. Chemical Equilibrium State for a chemical reaction where the reaction stops BEFORE all of the limiting reactant has.
Chapter 15; CHEMICAL EQUILIBRIUM 14 | 1 Describing Chemical Equilibrium Chemical Equilibrium—A Dynamic Equilibrium The Equilibrium Constant Heterogeneous.
V. Equilibrium Problems 2 main categories of equilibrium problems:  Finding K c or K p from known equilibrium concentrations or partial pressures  Finding.
STOICHIOMETRY. What is stoichiometry? Stoichiometry is the quantitative study of reactants and products in a chemical reaction.
 Chemical Equilibrium occurs when opposing reactions are proceeding at equal rates.  When the forward reaction equals the reverse reaction.  It results.
“K” Chemistry (part 2 of 3) Chapter 14: Chemical Equilibrium.
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 Calculations Example 4—Using Trial K eq to Predict Which Way a Reaction Will Move to Reach Equilibrium.
Topic Extension Equilibrium Acid-Base Equilibrium Solubility Equilibrium Complex-Ions Equilibrium Qualitative Analysis.
Quantitative Changes in Equilibrium Systems Chapter 7.5.
PROBLEM: The equilibrium constant for the butane < - - > isobutane isomerization reaction is 2.5 at 25°C. If 1.75 mol of butane and 1.25 mol of isobutane.
STOICHIOMETRY.
Equilibrium Pressure If the values at equilibrium are given in partial pressure, then solving for the constant is the same, but use Kp instead of Kc. What.
Chemical Equilibrium Chapter 13
Stoichiometric Calculations
Option 1: Running Reactions in Reverse
Announcements Exams will be handed back in lab next week.
AP Chem Turn in Equilibrium Lab Challenge
Presentation transcript:

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.

Using K C to determine [products] and [reactants] at equilibrium  Only know K C and initial concentrations of reactants  Changes in concentration of chemical compounds ( Δ C)  Related to STOICHIOMETRIC ratios in chemical equation.  Represents concentration change from initial to equilibrium conditions.

Example 1Example 1  2H 2 + O 2  2H 2 O  So what is [H 2 ] at equilibrium?  [H 2 ] at equilibrium = [H 2 ] initial – Δ H 2 **Use stoichiometric ratios to determine the amount of Δ C**

Example 2:Example 2:  1 mole of butane is in a 1L flask at 25°C with no isobutane present. What will be the equilibrium concentrations of butane and isobutane with a K C of 2.5 for this reaction?

Equilibrium Key Elements in Problem  Balanced Equation  Equilibrium constant  Initial Conditions  Problem’s Objective

Steps for Complex Problems 1)Decide if the reaction is at equilibrium 2)Set up equilibrium expression 3)Make an ICE Chart 4)Solve for Δ C 5)Is assumption valid for Δ C? 6)Determine the final concentrations of the chemical compounds.

Ice ChartIce Chart “ICE”ReactantsProducts Initial Concentrations (I): Change in Concentration ( Δ C or x): Equilibrium Concentrations (E):

Assumption with Δ CAssumption with Δ C  If Δ C < 5% of initial concentration, ignore the Δ C for adding and subtracting in equilibrium expression.  If Q< K, both small values so initial concentrations close to equilibrium  Always validate this assumption in an equilibrium problem

Assumption with Δ C (cont.)Assumption with Δ C (cont.)  If K eq < 1x10 -4, remove the “x or Δ C” value in denominator.  Δ C is very small compared to initial concentration so subtraction would not be a huge difference.  Only works when adding or subtracting Δ C  If concentrations or partial pressures are very small where their magnitude is approximately equal to K eq, CANNOT discount Δ C value.

Example 3:Example 3:  H 2 O (g) is present in a rigid container at 25°C with an initial partial pressure of atm. What are the partial pressures of H 2(g) and O 2(g) at equilibrium? (K P = 2.0 x )

Example 3: continuedExample 3: continued

Example 4:Example 4:  Sulfur trioxide decomposes to form sulfur dioxide and oxygen at 300°C°. Calculate the concentrations of all chemical compounds at equilibrium with an initial SO 3 concentration of 0.100M and K C = 1.6 x

Example 4: continuedExample 4: continued

Example 5:Example 5:  mol of COCl 2 comes to equilibrium in a 5.8L container at 25°C (K C = 7.27 x ). Find the equilibrium concentrations of all chemical compounds in the following equation. ( Hint: first find the initial [COCl 2 ] )  COCl 2 (g)  CO (g) + Cl 2 (g)

Example 5: continuedExample 5: continued

In ClassIn Class  Problems on Equilibrium II Worksheet

Homework  AP Equilibrium and ICE method worksheet (#1-5)