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Chemical Equilibrium Section 17.1 A State of Dynamic Balance Section 17.2 Factors Affecting Chemical Equilibrium Section 17.3 Using Equilibrium Constants Click a hyperlink or folder tab to view the corresponding slides. Exit Section 17.1 A State of Dynamic Balance (cont.) reversible reaction chemical equilibrium law of chemical equilibrium equilibrium constant homogeneous equilibrium heterogeneous equilibrium Chemical equilibrium is described by an equilibrium constant expression that relates the concentrations of reactants and products. Equilibrium Expressions • Some chemical systems have little tendency to react, others go to completion. • The majority reach a state of equilibrium with some of the reactants unconsumed. Types of chemical reactions Nonreversible chemical reactions: the reaction proceeds until all of the reactants are used up and the products are formed A+B C+D • Nonreversible reactions often produce – a gas that escapes – Insoluble solid product (precipitate) • Here, there is likely a limiting reactant What is equilibrium? (cont.) • A reversible reaction is a chemical reaction that can occur in both the forward and reverse directions, such as the formation of ammonia. N2(g) + 3H2(g) ↔ 2NH3(g) What is equilibrium? • Chemical reactions often reach a balancing point, or equilibrium. •When the rate of the forward and the reverse reactions are the same •http://ull.chemistry.uakron.edu/genobc/Chapter_08/ A saturated solution in equilibrium • Start with a beaker of solid RADIOACTIVE NaI at the bottom • Pour a saturated solution of nonradioactive NaI into the beaker • This solution is already saturated—it already holds the max amount of NaI possible • Wait several hours • Solid is filtered out and the solution is tested. It is radioactive! What does this tell us? •http://dbhs.wvusd.k12.ca.us/webdocs/Equilibrium/Dynamic-Equilibrium.html What is equilibrium? (cont.) • How does reversibility affect the production of ammonia? • Decreases in the concentrations of N2 and H2 cause the reaction to slow. • The reaction reaches equilibrium in figure d. What is equilibrium? (cont.) • Chemical equilibrium is a state in which the forward and reverse reactions balance each other because they take place at equal rates. • Equilibrium is a state of action, not inaction. Equilibrium in chemical reactions • Being in equilibrium does not imply that 50% of the amount present is reactant and 50% is product • There may be more total moles of product or more total moles of reactant A+B C + D The longer arrow implies that there is more reactant Equilibrium Expressions (cont.) • The law of chemical equilibrium states that at a given temperature, a chemical system might reach a state in which a particular ratio of reactant and product concentrations has a constant value. The Equilibrium Constant Expression Consider the reaction: aA + bB cC + dD Equilibrium Expressions (cont.) • The equilibrium constant, Keq, is the numerical value of the ratio of product concentrations to reactant concentrations, with each concentration raised to the power equal to its coefficient in the balanced equation. • The value of Keq is constant only at a specified temperature. Keq > 1: Products are favored at equilibrium Keq < 1: Reactants are favored at equilibrium Z + 2B 2C + X (all substances are gases at the same conditions) Concentrations are as follows: Z= 0.75M, B = 1.25M, C = 1.1M, X = 1.0M •Keq = [Z]a ·[B]b [C]c ·[X]d •[1.1]2 ·[1.0] = •1.0 2 [0.75] ·[1.25] •What does the Keq value of 1.0 represent? •Relative amounts of product and reactant are equal since the equilbrium constant is equal to 1.0! Equilibrium Expressions (cont.) H2(g) +I2(g) ↔ 2HI(g) • This reaction is a homogeneous equilibrium, which means that all the reactants and products are in the same physical state. Equilibrium Expressions (cont.) • When the reactants and products are present in more than one physical state, the equilibrium is called a heterogeneous equilibrium. • Ethanol in a closed flask is represented by C2H5OH(l) ↔ C2H5OH(g). Equilibrium Constants • For a given reaction at a given temperature, Keq will always be the same regardless of the initial concentrations of reactants and products. Section 17.1 Assessment A reaction is in equilibrium when: A. there are more products than reactants B. the amount of products equals the reactants D C 0% A D. the rate of the forward and reverse reactions are equal A. A B. B C. C 0% 0% 0% D. D B C. the rate of the forward reaction is greater than the reverse reaction Section 17.1 Assessment The value of the equilibrium constant is constant for a given ____. A. temperature B. pressure D A 0% C D. density A. A B. B C. C 0% 0% 0% D. D B C. volume Section 17.2 Factors Affecting Chemical Equilibrium • Describe how various factors affect chemical equilibrium. • Explain how Le Châtelier’s principle applies to equilibrium systems. reaction rate: the change in concentration of a reactant or product per unit time, generally calculated and expressed in moles per liter per second. Le Châtelier’s principle When changes are made to a system at equilibrium, the system shifts to a new equilibrium position. Le Châtelier’s Principle • Le Châtelier’s Principle was proposed in 1888 and states that if stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress. Henri Le Chatelier (1850-1936) was interested in the relationship between science and industry. He wanted to find a way to maximize the yield that can be obtained from any chemical reaction. The Industrial Revolution was taking off and this led to the need for the production of all kinds of chemicals. • Intro to LeChats Le Châtelier’s Principle (cont.) • Principle #1 Adjusting the concentrations of either the reactants or the products puts stress on a system in equilibrium. • Adding reactants increases the number of effective collisions between molecules and upsets the equilibrium. Le Châtelier’s Principle (cont.) • The equilibrium shifts to the right to produce more products. • Stress is relieved by shifting to the left, converting products to reactants. Le Châtelier’s Principle (cont.) • Principle#2 Increasing pressure shifts the system to the left, and more products are formed. • Changing the volume (and pressure) of an equilibrium system shifts the equilibrium only if the number of moles of gaseous reactants is different from the moles of gaseous products. • If the number of moles is the same on both sides of the balanced equation, changes in pressure and volume have no effect on the equilibrium. Le Châtelier’s Principle (cont.) The reaction between CO and H2 is at equilibrium. Lowering the piston decreases the volume and increases the pressure. As a result, more molecules of the products form. Their formation relieves the stress on the system. Le Châtelier’s Principle (cont.) • Principle #3 Changes in temperature alter the equilibrium position and the equilibrium constant. • If heat is added to an equilibrium system, the equilibrium shifts in the direction in which the heat is used up. Ex. 2SO2 + O2----->2SO3 + heat In this exothermic rxn heat is a product. Le Châtelier’s Principle (cont.) • Any change in temperature results in a change in Keq. Le Châtelier’s Principle (cont.) • A catalyzed reaction reaches equilibrium more quickly, but with no change in the amount of product formed. Section 17.2 Assessment Which does NOT result in a shift of the equilibrium to the right? A. removing products B. adding reactants C. increasing concentration of reactants A. A D C A 0% B. B C. C 0% 0% 0% D. D B D. adding products Section 17.2 Assessment Any change in ____ results in a change in Keq. A. temperature B. pressure D A 0% C D. concentration A. A B. B C. C 0% 0% 0% D. D B C. volume Section 17.3 Using Equilibrium Constants • Determine equilibrium concentrations of reactants and products. • Calculate the solubility of a compound from its solubility product constant. • Explain the common ion effect. solubility: the maximum amount of solute that will dissolve in a given amount of solvent at a specific temperature and pressure Section 17.3 Using Equilibrium Constants (cont.) solubility product constant common ion common ion effect Equilibrium constant expressions can be used to calculate concentrations and solubilities. Calculating Equilibrium Concentrations • Equilibrium constants can be used to calculate unknown concentrations of products when other concentrations are known. • Some ionic compounds dissolve readily in water, and some barely dissolve at all. • The equilibrium constant expression for the dissolving of a sparingly soluble compound is called the solubility product constant, Ksp. The Solubility Product Constant (cont.) • The solubility product constant expression is the product of the concentrations of the dissolved ions, each raised to the power equal to the coefficient of the ion in the chemical equation. The Solubility Product Constant (cont.) The Solubility Product Constant (cont.) • The values in the table can be used to determine the solubility of a sparingly soluble compound. • Ksp can be used to predict whether a precipitate will form when any two ionic solutions are mixed. The Solubility Product Constant (cont.) • Use the initial concentrations of ions in solution in the solubility product constant expression to calculate Qsp. • If Qsp < Ksp the solution is unsaturated and no precipitate will form. • If Qsp = Ksp the solution is saturated and no change will occur. The Solubility Product Constant (cont.) • If Qsp > Ksp a precipitate will form, reducing the concentrations of the ions in the solution until the product of their concentrations in the Ksp expression equals the numerical value of Ksp. The Solubility Product Constant (cont.) The Common Ion Effect (cont.) • A common ion is an ion that is common to two or more ionic compounds. • The lowering of the solubility of a substance because of the presence of a common ion is called the common ion effect. Common Ion Effect Equilibrium constants provide many practical applications. BaSO4 is an insoluble salt that has medical applications. Doctors use it as an X-ray contrast medium (Ba absorbs more radiation than most atoms). Ba ions are poisonous and in order to make sure they are not digested, a soluble salt like Na2SO4 is given with the Ba. As SO4 ions increase the Ba ions must decrease-this is the common ion effect. The Common Ion Effect • Why is PbCrO4 less soluble in aqueous solution of K2CrO4 than in pure water? • The K2CrO4 solution contains CrO42– ions before any PbCrO4 dissolves. Section 17.3 Assessment The presence of a common ion ____ the solubility of the dissolved substance. A. decreases B. increases D A 0% C D. speeds up A. A B. B C. C 0% 0% 0% D. D B C. does not change Section 17.3 Assessment If Qsp > Ksp A. the solution is unsaturated and no precipitate will form D D. a common ion must be present A 0% C C. a precipitate will form, reducing the concentrations of the ions in the solution A. A B. B C. C 0% 0% 0% D. D B B. the solution is saturated and no precipitate will form Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion Section 17.1 A State of Dynamic Balance Key Concepts • A reaction is at equilibrium when the rate of the forward reaction equals the rate of the reverse reaction. • The equilibrium constant expression is a ratio of the molar concentrations of the products to the molar concentrations of the reactants with each concentration raised to a power equal to its coefficient in the balanced chemical equation. • The value of the equilibrium constant expression, Keq, is constant for a given temperature. Section 17.2 Factors Affecting Chemical Equilibrium Key Concepts • Le Châtelier’s principle describes how an equilibrium system shifts in response to a stress or a disturbance. • When an equilibrium shifts in response to a change in concentration or volume, the equilibrium position changes but Keq remains constant. A change in temperature, however, alters both the equilibrium position and the value of Keq. Section 17.3 Using Equilibrium Constants Key Concepts • Equilibrium concentrations and solubilities can be calculated using equilibrium constant expressions. • Ksp describes the equilibrium between a sparingly soluble ionic compound and its ions in solution. • If the ion product, Qsp, exceeds the Ksp when two solutions are mixed, a precipitate will form. • The presence of a common ion in a solution lowers the solubility of a dissolved substance. A change in ____ alters both the equilibrium position and the equilibrium constant. A. pressure A 0% D D. density C C. volume A. A B. B C. C 0% 0% 0% D. D B B. temperature A(n) ____ equilibrium is when all reactant and products are in the same physical state. A. endothermic A 0% D D. homogeneous C C. heterogeneous A. A B. B C. C 0% 0% 0% D. D B B. exothermic Which is NOT an example of a homogeneous equilibria? A. H2(g) +I2(g) ↔ 2HI(g) B. 2H2(g) +O2(g) ↔ 2H2OI(g) D A 0% C D. C2H5OH(l) ↔ C2H5OH(g) A. A B. B C. C 0% 0% 0% D. D B C. HCl(aq) + NaOH(aq) ↔ NaCl(aq) + H2O Barium sulfate is toxic to humans, so why can it be ingested for use with gastrointestinal x-rays? A. It is minimally poisonous. A 0% D D. Your body readily absorbs it. C C. It has low solubility. A. A B. B C. C 0% 0% 0% D. D B B. It has high solubility. The state in which the forward and reverse chemical reactions take place at the same rate is called ____. A. Le Châtelier’s Principle A 0% D D. chemical equilibrium C C. Charles’s Law A. A B. B C. C 0% 0% 0% D. D B B. Henry’s Law Which does NOT describe a system that has reached chemical equilibrium? A. No new product is formed by the forward reactions. D. All the reactants have been used up. D A 0% C C. The concentration of products is equal to the concentration of reactants. A. A B. B C. C 0% 0% 0% D. D B B. The forward and reverse reactions occur at equal rates. Adding product to a chemical equilibrium: A. does nothing B. creates a stress and shifts the equilibrium to the right D A 0% C D. causes more product to form A. A B. B C. C 0% 0% 0% D. D B C. creates a stress and shifts the equilibrium to the left Ethylene (C2H4) reacts with hydrogen to form ethane (C2H6). C2H4(g) + H2(g) ↔ C2H6(g) + heat. How could you increase the amount of hydrogen in the system? A. Increase the heat. A 0% D D. Decrease the C2H6. C C. Increase the C2H4. A. A B. B C. C 0% 0% 0% D. D B B. Decrease the heat. Which does NOT result in a shift of the equilibrium to the right? A. removing products B. adding reactants D A 0% C D. decreasing the concentration of reactants A. A B. B C. C 0% 0% 0% D. D B C. increasing concentration of reactants A(n) ____ equilibrium is when all reactant and products are present in more than one physical state. A. endothermic A 0% D D. homogeneous C C. heterogeneous A. A B. B C. C 0% 0% 0% D. D B B. exothermic