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Kinetics/Equilibrium Game

Kinetics/Equilibrium Game. Review. What happens to the reaction rate of many reactions when the temperature is increased by 10 o C?. Doubles.

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Kinetics/Equilibrium Game

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  1. Kinetics/Equilibrium Game Review

  2. What happens to the reaction rate of many reactions when the temperature is increased by 10oC? • Doubles

  3. For a reversible reaction, a state of equilibrium exists when the forward and backward reactions are proceeding under the same conditions at the same ___________. • rate

  4. For a given reaction, the value of the equilibrium constant will change when the ____________ is changed. • temperature

  5. Define “activated complexes” • Unstable, intermediate species that form when particles of the reactants collide with sufficient energy

  6. The catalysts in many biochemical changes in the human body are • enzymes

  7. Determine the equilibrium constant for the system S2O4(g) 2SO2(g) at 25oC. The equilibrium concentrations are shown here: [S2O4]= 5.62 x 10-3, [SO2]= 2.3 x 10-4 • [SO2]2/[S2O4]=(2.3 x 10-4)2/5.62 x 10-3= • K= 9.4 x 10-6

  8. 4CH3(g)+ 5O2(g) 4CO(g) + 6H2O(g) • Which direction will the equilibrium shift if CO is added to the system? • Left • What would happen to the CO concentration if the total pressure was decreased? • The CO concentration would increase

  9. 4CH3(g)+ 5O2(g) 4CO(g) + 6H2O(g) • Given that the reaction is exothermic, what direction would the reaction shift if the temperature of the system were increased? • Left

  10. CH4(g) + 2H2S(g) + heat ↔ CS2(g) + 4H2(g) • If the concentration of 2H2S is increased, the concentration of H2 will • Increase • If the pressure is increased, the number of moles of CH4 molecules formed will • Increase • Lowering the temperature will favor (a) the reverse exothermic reaction (b) the forward endothermic reaction (c) both reactions • (a) The reverse exothermic reaction

  11. 2X(s) + 3Y(l) C(aq) + 4D(aq) • The equilibrium expression for the reaction is • [C][D]4

  12. The solubility of Ca(OH)2(s) in water at 25oC is 1.5 x 10-4mol/L. Calculate the Ksp for Ca(OH)2(s) at 25oC. • Ca(OH)2(s)  Ca2+(aq) + 2OH-(aq) • Ksp = [Ca2+][OH-]2 • Ksp = [1.5 x 10-4mol/L][1.5 x 10-4mol/L]2 • = 3.4 x 10-12

  13. Write the equilibrium dissociation reaction for the dissolving of the following substances in water. • H2PO4 • H2PO4 2H+(aq) + PO43-(aq) • Ba3(PO4)2(s)  • Ba3(PO4)2(s)  3Ba2+(aq) + 2PO43-(aq) • MgSO4(s) • MgSO4(s)Mg2+(aq)+ SO42-(aq) • H2SO4(s) • H2SO4(s) 2H+(aq)+ SO42-(aq)

  14. For the reaction 2H2(g) + S2(g)  2H2S(g), the concentration of H2 is .020 mols/L and the concentration of H2S is .350 mol/liter. If the equilibrium constant is 33.0, what is the concentration, in moles/L of S2? • Keq= [H2S]2/[H2]2[S2]= • 33.0= [.350]2/[.020]2[S2]= • [S2]=[.350]2/([.020]2x33.0) • [S2]= 9.28 mol/L

  15. For the reaction: Br2(g)2Br-(g) at a particular temperature, the concentrations at equilibrium were observed to be [Br2] = 2.0 x 10-4mol/L and [Br-] = 1.4 x 10-5mol/L. Calculate the value of the equilibrium constant from these data. (K has no units) • Keq = [Br-]2/[Br2] • = [1.4 x 10-5mol/L]2/[2.0 x 10-4mol/L] • K = 9.8 x 10-7

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