1 / 54

Subjective Question # 1 Kinetics

Subjective Question # 1 Kinetics. A. Increase the rate CaCO 3(s) + 2HCl (aq) → CO 2(g) + CaCl 2(aq) + H 2 O (l) Increase temperature Increase [HCl] Add a Catalyst Increase Surface Area of CaCO 3. B. Measure the rate

eldora
Download Presentation

Subjective Question # 1 Kinetics

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. Subjective Question # 1 Kinetics

  2. A. Increase the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) Increase temperature Increase [HCl] Add a Catalyst Increase Surface Area of CaCO3

  3. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l)

  4. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass

  5. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass [HCl]

  6. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass [HCl] volume

  7. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass [HCl] volume [CaCl2]

  8. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass [HCl] volume [CaCl2] can’t

  9. B. Measure the rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) mass [HCl] volume [CaCl2] can’t over time Measure the decrease in mass of an open container Measure the increase in pressure of an closed container

  10. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min

  11. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min

  12. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min (82.07 - 81.63) g CO2 75 s

  13. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min (82.07 - 81.63) g CO2 x 1 mole 75 s 44.0 g

  14. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min (82.07 - 81.63) g CO2 x 1 mole x 2 mole HCl 75 s 44.0 g 1 mole CO2

  15. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min (82.07 - 81.63) g CO2 x 1 mole x 2 mole HCl x 36.5 g 75 s 44.0 g 1 mole CO2 1 mole

  16. C. Calculate the Rate CaCO3(s) + 2HCl(aq) → CO2(g) + CaCl2(aq) + H2O(l) 1. Calculate the rate in grams HCl/min (82.07 - 81.63) g CO2 x 1 mole x 2 mole HCl x 36.5 g x 60 s = 0.56 g/min 75 s 44.0 g 1 mole CO2 1 mole 1 min

  17. D. Collision Theory More Collisions Harder Collisions Lower Ea

  18. Subjective Question # 2 Equilibrium

  19. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g)

  20. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I C E

  21. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I 0.400 M 0.400M 0 C E 0.300 M

  22. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I 0.400 M 0.400M 0 C -0.300 M -0.150 M +0.300 M E 0.300 M

  23. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I 0.400 M 0.400M 0 C -0.300 M -0.150 M +0.300 M E 0.100 M 0.250 M 0.300 M

  24. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I 0.400 M 0.400M 0 C -0.300 M -0.150 M +0.300 M E 0.100 M 0.250 M 0.300 M Equilibrium concentrations go in the equilibrium equation! Keq = [SO3]2 [SO2]2[O2]

  25. When 0.800 moles of SO2 and 0.800 moles of O2are placed into a 2.00 litre container and allowed to reach equilibrium, the equilibrium [SO3] is to be 0.300 M. Calculate the Keq value. 2SO2 (g) + 1O2 (g)⇋2SO3 (g) I 0.400 M 0.400M 0 C -0.300 M -0.150 M +0.300 M E 0.100 M 0.250 M 0.300 M Equilibrium concentrations go in the equilibrium equation! Keq = [SO3]2 (0.3)2 = [SO2]2[O2] (0.1)2(0.25)

  26. If 4.00 moles of CO, 4.00 moles H2O, 6.00 moles CO2, and 6.00 moles H2 are placed in a 2.00 L container at 670 oC, Keq = 1.0 CO(g) + H2O(g) ⇄ CO2(g) + H2(g) Is the system at equilibrium? If not, how will it shift in order to get there? Calculate all equilibrium concentrations. Get Molarities 2.00 M 2.00 M 3.00 M 3.00 M Calculate a Kt Kt = (3)(3) = 2.25 (2)(2) Not in equilibrium Shifts left!

  27. Do an ICE chart CO(g) + H2O(g) ⇄ CO2(g) + H2(g) I 2.00 M 2.00 M 3.00 M 3.00 M C +x +x -x -x E 2.00 + x 2.00 + x 3.00 - x 3.00 - x Keq = (3 - x)2 = 1.0 (2 + x)2 Square root 3 - x = 1.0 2 + x 3 - x = 2 + x 1 = 2x x = 0.50 M [CO2] = [H2] = 3.00 - 0.50 = 2.50 M [CO] = [H2O] = 2.00 + 0.50 = 2.50 M

  28. Subjective Question # 3 Solubility

  29. 200.0 mL 0.10 M Pb(NO3)2 is mixed with 300.0 mL of 0.20 M NaCl, will a precipitate occur? PbCl2(s)⇌ Pb2+ + 2Cl- 200 0.10 M 300 0.20 M 500 500 0.040 M 0.12 M TIP = [Pb2+][Cl-]2 TIP = [0.040][0.12] 2 = 5.8 x 10-4 Ksp = 1.2 x 10-5 TIP > Ksp ppt forms

  30. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution. AgCl(s)⇄ Ag+ + Cl- 0.20 M Ksp = [Ag+][Cl-] 1.8 x 10-10 = [0.20][Cl-] [Cl-] = 9.0 x 10-10 M BaCl2(s)⇄ Ba2+ + 2Cl- 4.5 x 10-10 M9.0 x 10-10 M 0.50 L x 4.5 x 10-10mole x 208.3 g = 4.7 x 10-8 g 1 L mole

  31. PbCl2(s)⇌ Pb2+ + 2Cl- Ksp = 4s3

  32. Subjective Question # 4 to 6 Acids

  33. HClStrong AcidHCl  H+ + Cl- 0.10 M 0.10 M pH = -Log[H+] = 1.0 No ICE HFWeak AcidHF ⇌ H+ + F- I0.10 M 0 0 C x x x E 0.10 - x x x small Ka x2 = 3.5 x 10-4 x = 0.005916 M 0.10 pH = -Log[0.005916] = 2.23

  34. NaOHStrong BaseBa(OH)2 Ba2+ + 2OH- 0.20 M 0.40 M pOH = -Log[OH-] = 0.40 No ICE NH3Weak BaseNH3 + H2O ⇌NH4+ + OH- I0.20 M 0 0 C x x x E 0.20 - x x x small Kb x2 = Kb = Kw = 1.0 x 10-14 = 1.786 x 10-5 0.20 Ka 5.6 x 10-10 x = 0.001890 M pOH = -Log[0.001890] = 2.73 pH = 11.27

  35. Subjective Question 7 & 8 Redox

  36. Review of Cells ElectrochemicalElectrolytic Is a power supplyRequires power supply Spontaneous (+ ve)Nonspontaneous(-ve) Makes electricityMakes chemicals Reduction is highest on Chart Reduction is the –ve

  37. For all cells: Cations migrate to the cathode, which is the site of reduction. Anions migrate to the anode, which is the site of oxidation. Electrons travel through the wire from anode to cathode.

  38. Complete the Chart Electrochemical Cell: Zn, Zn(NO3)2 II Cu, CuSO4 Anode:Reaction: Cathode:Reaction: E0 =

  39. Complete the Chart Electrochemical Cell: Zn, Zn(NO3)2 II Cu, CuSO4 Anode:ZnReaction: Cathode:CuReaction: E0 = Higher on reduction Chart

  40. Complete the Chart Electrochemical Cell: Zn, Zn(NO3)2 II Cu, CuSO4 Anode:ZnReaction:Zn → Zn2+ + 2e- 0.76 v Cathode:CuReaction: E0 = Higher on reduction Chart

  41. Complete the Chart Electrochemical Cell: Zn, Zn(NO3)2 II Cu, CuSO4 Anode:ZnReaction:Zn(s) → Zn2+ + 2e- 0.76 v Cathode:CuReaction:Cu2+ + 2e- → Cu(s) 0.34 v E0 = Higher on reduction Chart

  42. Complete the Chart Electrochemical Cell: Zn, Zn(NO3)2 II Cu, CuSO4 Anode:ZnReaction:Zn(s) → Zn2+ + 2e- 0.76 v Cathode:CuReaction:Cu2+ + 2e- → Cu(s) 0.34 v E0 = 1.10 v Higher on reduction Chart

  43. Electrolytic Cell: Molten AlCl3 Anode: Reaction: Cathode: Reaction:

  44. Electrolytic Cell: Molten AlCl3 Al3+ Cl- Anode: C Reaction: Cathode: C Reaction:

  45. Electrolytic Cell: Molten AlCl3 Al3+ Cl- Anode: C Reaction: Cathode: C Reaction: Put the vowels together: Anode Anion Oxidation

  46. Electrolytic Cell: Molten AlCl3 Al3+ Cl- Anode: C Reaction: 2Cl- → Cl2 + 2e- -1.36 v Cathode: C Reaction: Put the vowels together: Anode Anion Oxidation Oxidation of Anion

  47. Electrolytic Cell: Molten AlCl3 Anode: C Reaction: 2Cl- → Cl2 + 2e- -1.36 v Cathode: C Reaction: Put the consonants together: Cathode Cation Reduction

  48. Electrolytic Cell: Molten AlCl3 Anode: C Reaction: 2Cl- → Cl2 + 2e- -1.36 v Cathode: C Reaction: Al3+ + 3e- → Al -1.66 v Put the consonants together: Cathode Cation Reduction Reduction of Cation

  49. Electrolytic Cell: Molten AlCl3 Anode: C Reaction: 2Cl- → Cl2 + 2e- -1.36 v Cathode: C Reaction: Al3+ + 3e- → Al -1.66 v E0 = -3.02 v

  50. Electrolytic Cell: 1M AlCl3 Anode: Reaction: Cathode: Reaction: E0 = MTV =

More Related