1 / 21

Chapter 18 Equilibrium

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, products may start to change back into reactants; the reaction is reversible . A + B ↔ AB. CO 2 + H 2 O  C 6 H 12 O 6 + O 2

makya
Download Presentation

Chapter 18 Equilibrium

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 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, products may start to change back into reactants; the reaction is reversible. A + B ↔ AB

  2. CO2 + H2O  C6H12O6 + O2 O2 + C6H12O6  CO2 + H2O

  3. Equilibrium • Equilibrium is the state where the forward and reverse reactions balance because they are occurring at equal rates. • NO OVERALL CHANGE!

  4. The Law of Chemical Equilibrium • the point in the reaction where a ratio of reactant and product concentration has a constant value, Keq

  5. Homogeneous equilibrium • States of all compounds are the ____________ H2(g) + I2(g)↔ 2HI (g) • Heterogeneous equilibrium • States of compounds are ________________ CaCO3(g)↔ CaO (s) + CO2(g) Remember we only pay attention to the GASES when we calculate Keq!

  6. What is the correct the Keq? N2(g) + 3H2(g)↔ 2NH3(g)

  7. What is the correct the Keq? 2 NbCl4(g)↔ NbCl3(g) + NbCl5(g)

  8. What is the correct Keq? H2O (l)↔ H2O(g)

  9. If Keq = 2.4, which is more favored? A. products B. reactants C. neither is favored D. not enough information

  10. Chemical Equilibrium Problems I • Write the equilibrium constant expression (Keq) for these homogeneous equations. 1. N2O4 (g) ↔ 2 NO2 (g)

  11. 2. CO (g) + 3H2(g)↔ CH4(g)+ H2O (g) 3. 2 H2S (g)↔ 2 H2(g) + S2(g)

  12. Write the equilibrium constant expression (Keq) for these heterogeneous equations. • C10H8(s)↔ C10H8(g) • CaCO3(s) ↔ CaO (s) + CO2(g)

  13. 3. C (s) + H2O(g) ↔ CO(g) + H2(g) 4. FeO(s) + CO(g) ↔ Fe(s) + CO2(g)

  14. 0.98 • 15.59 • 0.064 • 1.02 • 2.05 1. Calculate the Keq for the following equation using the data: [N2O4] = 0.0613 mol/L [NO2] = 0.0627 mol/L N2O4(g)↔ 2NO2(g)

  15. A. 0.25 B. 0.72 C. 0.04 D. 3.93 E. 0.02 2. [CO] = 0.0613 mol/L [H2] = 0.1839 mol/L [CH4]=0.0387 mol/L [H2O]=0.0387 mol/L CO (g) + H2 (g)↔ CH4(g)+ H2O (g)

  16. 3. [H2]=1.5 mol/L [N2]=2.0 mol/L [NH3]=1.8 mol/L 3H2(g) + N2(g)↔ 2NH3(g) • 0.48 • 0.24 • 2.5 • 0.40

  17. 3. If the Keq = 0.48, we know that the equilibrium favors… a. reactants b. products c. neither

  18. 4. [Mg]=2 mol/L [HCl]=3 mol/L [MgCl]=6 mol/L [H2]=3 mol/L 2 Mg (s) + 2 HCl (g)↔ 2 MgCl (g) + H2(g) • 3 • 12

  19. 4. Since Keq = 3, we know that the equilibrium favors a. reactants b. products c. neither

  20. 5. [H2]=0.52 mol/L [I2]=0.23 mol/L [HI]=1.7 mol/L H2(g) + I2(g)↔ 2HI (g) • 202 • 0.04 • 24.16

  21. 5. Since Keq= 24.16, we know that the equilibrium favors a. reactants b. products c. neither

More Related