Chemistry+A

NY Regents Review Schedule Titration Introduction to Voltaic Cells

Period 3 Period 6

Period 6 - Redox Test is on TUESDAY 5/25

Period 3 - Redox Test is on WEDNESDAY 5/26

REVIEW all of your homework. Do pink MC packet and golden rod Free Response problems. MC answers 51-140 are below. 51) 1   52)  1   53)  1   54)  4   55)  4   56)  2   57)  1   58)  2   59)  3   60)  3   61)  2   62)  3   63)  1   64)  3   65)  2   66)  1   67)  3   68)  3   69)  1   70)  1   71)  2   72)  2   73)  2   74)  2   75)  1   76)  1   77)  1   78)  3   79)  3   80)  3   81)  4   82)  3   83)  2   84)  4   85)  1   86)  2   87)  1   88)  2   89)  1   90)  4   91)  2   92)  4   93)  1   94)  3   95)  3   96)  2   97)  3   98)  1   99)  2   100)  1   101)  4   102)  3   103)  4   104)  2   105)  1   106)  3   107)  4   108)  4   109)  1   110)  1   111)  4   112)  3   113)  1   114)  2   115)  1   116)  1   117)  1   118)  4   119)  3   120)  1   121)  1   122)  4   123)  half cell 1, Pb, left, lead   124)  1 125) 1   126)  3   127)  4   128)  3   129)  3   130)  3   131)  2   132)  1   133)  4   134)  4   135)  3   136)  1   137)  1   138)  3   139)  2   140)  1

Organic HW Due MONDAY

Go to the following website: []

Answer questions 1-5. Check your answers at the end. Write down the numbers of any that you do not understand so that we can go over them on Tuesday. Write down your answers on a separate sheet of paper to turn in.

Here are the answers to your acid base HW review assignment:

NY Chemistry a Brief Review []

Quiz on Chapter 1 is Friday

Next Friday there will be a quiz on chapters 2-3

Key to Review 1. 3 2. 4 3. 4 4. 3 5. 4 6. 3 7. 1 8. 2 9. 5 10. 2 11. answer is not there: 1.2 g 12. 3 13. 5 14. 1 15. 2 16. 1 17. 5 18. 3 19. 4 20. 2 21. 2 22. 3 23. 1 24. 2 25. 1 26. 1 27. 1 28. 5 29. 1 30. 2 31. 3 32. 2 33. 5 34. 4 35. 2 (should say at the lower temps not at 700K) 36. 5 37. 4 38. 3 39. 3 40. 4 41. 3 42. 4 (catalysts do only sometimes!!!!! so 4 is the best answer) 43. 2 44. 2 45. 4 46. 4 47. 2 48. 5 49. 2 50. 4 51. 3 52. 1 53. 5 54. 5 55. 5 56. 3 57. 4 58. 3 59. 1

Free Response Problem 1 (b) Problem 2 (a) Problem 3 SKIP Problem 4 SKIP Problem 5 (a) Problem 6 (b) 7b) Increasing c) 1.33 ml/s d) 5.35 x 10^-5 mol/s 8a) endothermic b) positive c) increase d) spontaneous e) reverse, exothermic, decrease in entropy, so spontaneous at low temp 9) increases reaction rate because it increases the concentration of oxygen which is a reactant 10a) decrease b) increases c) decrease d) increase e) decreases f) increases 11a) increase b) decrease c) decrease d) no effect 12) Sorry the numbering is off. Just make sure you can do the endo and exothermic potential energy diagram 13) HOT PACK - reaction is exothermic which means it releases energy to the surroundings as it forms bonds so the pack feels hot and the products have less potential energy than the reactants. COLD PACK - reaction is endothermic which means it absorbs energy from the surroundings which makes it feel cooler to the surroundings and the reactants have less potential energy than the reactants. 14) PHOTOSYNTHESIS a) nonspontaneous b) endothermic c) positive d) decrease CELLULAR RESPIRATION a) spontaneous b) exothermic c) exothermic d) increase / e) Products have more energy in photosynthesis f) they are the reverse of each other so they balance the amount of carbon dioxide by equally the input (cellular respiration) and output (photosynthesis). 15) C7H16 (l) + 11O2 (g) --> 7CO2 (g) + 8H2O (l) a) increase b) decrease c) no effect d) decrease 16) 2H2O2 (aq) --> 2H2O (l) + O2 (g) a) manganese oxide b) decreases the activation energy so at the same temperature more molecules have enough kinetic energy so their are more effective collisions c) a flame test will show the gas is oxygen 17a) 0.106 L of hydrogen b) 1.9 mol/s 18) The equilibrium constant does not tell you about the reaction rate, it only tells you whether the forward or reverse rate is favored; in other words whether there will be more products or reactants once equilibrium is reached. 19) If you increase the temperature the equilibrium will shift to the endothermic reaction, which in this case is forward. Therefore the product concentration will increase and so will the K value. 20) Reaction rate would increase because the concentration of the reactant oxygen is increased. It would probably explode. 21) a) increase pressure decrease temp b) increase pressure decrease temp c) decrease temp d) increase pressure decrease temp 22) a) shifts towards fewer gas molecules so that the pressure will go back down b) shifts to exothermic reaction so that the energy will be released and temperature will increase again c) reverse to decrease conc of porducts back down to equilibrium concentration d) reverse to increase reactants back to equilibrium concentration 23a) neither b) reverse c) forward 24a) forward b) reverse c) reverse d) no effect e) reverse 25a) k = [H2]^4/[H2O]^4 b) k = [CO2][H2O]^2/[CH4][O2]^2 c) k=1/[Cl2] d) ksp = [Fe3+][OH-]^3

33) MAKE SURE YOU DO THIS ONE!!!!!! 35) -125 kcal/mol 39)-133.2 J/K 41) -32.99 kJ (don't forget to change the J in the entropy to kJ)

=What's on the test?= =What affects the rate of reaction: temperature, concentration, pressure, volume, nature of reactants, catalyst. Explain why - Graphs: Average kinetic energy of molecules, potential energy reaction diagram for endo and exo and how all three charts change when you add a catalyst - Differences between homogeneous vs. heterogeneous reactions and give examples - Use data from a lab to make calculations about reaction rate. Graph data and explain the significance of the slope - Define: activation energy, endothermic, exothermic, enthalpy, entropy, Gibb's free energy. - Breaking bonds is endo and formation of bonds is exo - Use Hess's law - Use heats of formation to calculate enthalpies - Explain conditions required for spontaneous and nonspontaneous reactions - Explain deltaG= deltaH -TdeltaS and use it to make calculation and predication about spontaneity of reactions. - Explain the equation for the entropy of the universe. When is the change in entropy of the universe equal to zero? - Write Keq expressions and perform calculations. - Use and explain Le Chatelier's principle - Predict how an equilibrium will shift and how the equilibrium constant will change when you change temperature, pressure, volume, and concentration. - Write Ksp expressions and determine solubility and constant and use the Q value to predict whether or not a precipitate will form. - Write net ionic equations. Use reference tables to predict precipitates. For Worksheet C For the homework packet  These and the challenge problems are the hardest ones I think you'd see on the test. If you have any specific requests email me by 8pm and I'll get back to you. Happy studying!=