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Equilibrium

Equilibrium. Chapter 13 and 14. Homework . Chapter 13 pg 628 1-71 odd Chapter 14 pg 688 11-87 odd. AP Test. Historically, the first question on the free response has ALWAYS been an equilibrium question.

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Equilibrium

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  1. Equilibrium Chapter 13 and 14

  2. Homework • Chapter 13 pg 628 1-71 odd • Chapter 14 pg 688 11-87 odd

  3. AP Test • Historically, the first question on the free response has ALWAYS been an equilibrium question. • The new style of test no longer requires that, however, I would be surprised if they didn’t have one on the test.

  4. Equilibrium • A state when two competing reactions are canceling each other out. • H3O+ + OH-⇌H2O + H2O • You reach equilibrium when the rate of forward reaction is equal to the rate of backwards reaction. • This does NOT mean the concentration of products and reactants are equal. • The above reaction is at equilibrium when [H3O+] = [OH-] = 1x10-7mol/L. In 1 L of water there are 55moles.

  5. Macro Micro • Macroscopically, anything that equilibrium is stable. Meaning the concentrations of the different substances are not changing. • Law of mass action- when the ratio of product to reactant is a constant value the system is at equilibrium • Microscopically, atoms and molecules are constantly reacting in both reactions • http://chemconnections.org/Java/equilibrium/index.html

  6. Changes in Concentration N2(g) + 3H2(g) ⇌ 2NH3(g)

  7. Equilibrium expression and constant • K is calculated form EQUILIBRIUM CONCENTRATIONS! Its values may only be calculated experimentally. • aA+ bB⇌cC+ dD • equilibrium constant = equilibrium expression •   K = [C]c[D]d • [A]a[B]b • [ ] means concentration in M

  8. Determine the equilibrium expression • For the following: • Br2(g) ⇌2Br(g) • N2(g) + 3H2(g) ⇌2NH3(g) • H2 (g) + Br2(g) ⇌2 HBr(g) • HCN(aq) ⇌H+(aq) + CN-(aq)

  9. K values, k is always positive • Intermediate K. 0.1<K<10 • Significant concentrations of all substances are present. • Very Large K. K >> 1 • The product concentration is very large with virtually no reactant concentration (the reaction has gone to completion). • Very Small K. K<<1 • The reactant concentration is very large with virtually no product concentration.

  10. Types of K • Kc= equilibrium constant in terms of concentration. • Kp= equilibrium concentration in terms of pressure. • Ka= acid dissociation constant • Kb= base dissociation constant • Kw= ion-product constant for water • These are listed on your equation sheet

  11. Actual equation sheet

  12. K problem • The following equilibrium concentrations were observed for the Haber process at 127 C. • [NH3] = 3.1 x 10-2 M, [N2] = 8.5 x 10-1 M, [H2] = 3.1 x10-3 M • Forward Reaction. • N2(g) + 3H2(g) ⇌2NH3(g) • Reverse Reaction. • 2NH3(g) ⇌N2(g) + 3H2(g) • Multiply by Factor n. • 1/2N2(g) + 3/2H2(g) ⇌NH3(g) • K is unitless

  13. Summary • For forward reaction jA + kB⇌lC + mD, • K = [C]l [D]m • [A]j [B]k • Forreverse reaction jA + kB⇌lC + mD, • K’ = K-1= [A]j [B]k • [C]l [D]m • For reaction njA + nkB⇌nlC + nmD • K’’ = Kn = [C]nl [D]nm • [A]nj[B]nk • For an overall reaction of two or more steps, • Koverall = K1 x K2 x K3 x ...

  14. Equilibrium of Gases. • PV = nRT or P = (n/V)RT • n/V is mol/L, or a concentration. • Concentration of a gas is C = P/RT • Therefore you can determine the K of a gas from its pressure and temperature

  15. Problem • 2NO(g) + Cl2(g) ⇌ 2NOCl(g) • The reaction for the formation of nitrosyl chloride was studied at 25oC. The pressures at equilibrium were found to be • PNOCl = 1.2 atm • PNO = 5.0 x10-2atm • PCl2 = 3.0 x10-1atm • Calculate the value of K for the reaction at 25oC. • PV = nRT R = .0821 atm L / mol K

  16. Kp • Since we are always dividing by the pressure value by RT, there has to be a way to cancel that out. • Kp is a value that looks at the pressure of the gases involved instead the concentrations • To convert Kp to K • K may be written Kc, or K with respect to conc. • Kp = K(RT)n • Where n=  coefficients of products -  coefficients of reactants

  17. Same Problem • 2NO(g) + Cl2(g) ⇌2NOCl(g) • The reaction for the formation of nitrosyl chloride was studied at 25oC. The pressures at equilibrium were found to be • PNOCl = 1.2 atm • PNO = 5.0 x10-2atm • PCl2 = 3.0 x10-1atm • Calculate the value of Kp for the reaction at 25o C, and then convert that Kp to K.

  18. Example N2(g) + 3H2(g) ⇌2NH3(g)

  19. Pressure Problem • Dinitrogen tetroxide in its liquid state was used as one of the fuels on the lunar lander for the NASA Apollo missions. In the gas phase it decomposes to gaseous nitrogen dioxide: •   N2O4(g)⇌2NO2(g) • Consider an experiment in which gaseous N2O4 was placed in a flask and allowed to reach equilibrium at a temperature where Kp = 0.133. At equilibrium, the pressure of N2O4 was found to be 2.71 atm. Calculate the equilibrium pressure of NO2(g).

  20. Homogeneous Equilibria • Homogeneous equilibria – involve the same phase: N2(g) + 3H2(g) ⇌2NH3(g) HCN(aq) ⇌H+(aq) + CN-(aq)

  21. Heterogeneous Equilibria • Heterogeneous equilibria – involve more than one phase: 2KClO3(s) ⇌2KCl(s) + 3O2(g) 2H2O(l) ⇌2H2(g) + O2(g)

  22. The position of a heterogeneous equilibrium does not depend on the amounts of pure solids or liquids present. • The concentrations of pure liquids and solids are constant. 2KClO3(s)⇌2KCl(s) + 3O2(g)

  23. Write expressions for Kfor the following: • The decomposition of solid phosphorus pentachloride to liquid phosphorus trichloride and chlorine gas. • Deep blue solid copper(II) sulfate pentahydrate is heated to drive off water vapor to form solid green copper(II) sulfate.

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