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Chem 100 Final Review ------------------------------ Potentially Useful Information for the Problems Below-----------------------------R=0.0821 (atm L)/(mol K) -------------------------------------------------------------------------------------------------1. An acidic solution has a pH of 3.43. What is the Hydronium ion concentration? What is the [OH-] concentration? 2. Rank the following from lowest to highest acidity. a) 1.8 10-5 b) 2.4 10-10 c) 1.2 10-2 d) 8.0 10-9 3. In the following reaction what is (are) the base(s) and the acid(s)? HCl + NH3 NH4+ + Cl- 4. Determine the number of moles of carbon dioxide produced in the following unbalanced combustion reaction. C8H17OH + O2 CO2 + H2O 5. How many grams of NaH2PO4 are needed to react with 0.0106 moles of NaOH in the balanced reaction: NaH2PO4 + 2NaOH Na3PO4 + 2H2O NaH2PO4 = 119.98 g/mol NaOH = 40.00 g/mol 6. In the following balanced reaction 8.00 g of oxygen is used to produce how many grams of HCN? 2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(l) 7. A gas has a volume (in Liters) of 6.00 liters at 27 C with a pressure of 1.0 atm. What is the volume of the gas at 327 C with a pressure of 3.00 atm. 8. When 35.6 L of ammonia is reacted with oxygen at 1.0 atm at 25 C, the answer closest to the number of grams of H2O produced in the unbalanced equations is: 4NH3 + 5O2 4NO + 6H2O 9. The answer closest to the number of grams of NaH2PO4 needed to react with 38.74 mL of 0.275 M NaOH, according to the following balanced equation is: (NaH2PO4 = 119.98 g/mol) NaH2PO4 (s) + 2NaOH (aq) Na3POH4 (aq) + 3H2O 1 10. In the following reaction identify the compounds that get oxidized and reduced, oxidizing agent and reducing agent. Al + O2 Al2O3 11. The number of lone pairs of electrons in CF3- is 12. The molecular arrangement of atoms around H3O+ is: 13. Polar arrows indicate the polarity of bonds, indicate to which atom the positive side of the arrow would point to for the molecular fragments N-B, N-O, Br-Cl, S-Se respectively. 1. 2. 3. 4. 5. N, O, Cl, S N, N, Cl, Se B, N, Cl, S B, N, Br, Se B, O, Cl, Se 14. What is the condensed electron configuration for Se 15. The maximum number of electrons an atom with a 1s, 2s, 2p, 3s electron configuration can have is? 16. What is the average atomic mass of iridium based on its two isotopes: 191 Ir 190.9609 amu (abundance = 37.120%) and 193Ir 192.9633 amu (abundance = 62.880%) 17. The amount of heat is required to raise 100.0 g of water from 1.00 C to 99.0C: [heat capacity of water = 1.00 cal/(g C)] is closet to: 18. Express 96,342 m using two significant figures a) 9.60 104 m b) 9.6 104 m c) 9.60 10-4 m d) 9.63 104 m e) 9.60 104 m 2 19. The largest volume among the following is 10 nL 10,000 L 1,000 pL 0.01 dL 100 mL 20. The symbol A=37, Z=17, X- (where X stands for the element symbol) represents an ion of a) b) c) d) e) chlorine with 20 electrons chlorine with 16 electrons rubidium with 38 electrons rubidium with 36 electrons chlorine with 18 electrons 21. The most likely ionic form of the elements Ca and F is: a) b) c) d) e) Ca2-, F+ Ca2+, F2Ca2+, FCa+, FCa+, F2- 22. Convert 233C to Fahrenheit. a) b) c) d) e) 451. F 506. F 112. F 130. F 273. F 23. The density of Au is 19.3 g/mL. How many 1-ounce coins could be manufactured from a 1 cubic foot block of gold? 1 ft3 = 0.02832 m3, 1 oz = 28.35 g 3.32 102 2.43 1010 1.93 105 8.21 10-2 3 24. A metal has a charge of 3+ and 39 electrons. The mass of one of its 7 isotopes is 96 amu and its abundance is 74.8%. Calculate the number of neutrons for this element and what is the element? a) b) c) d) e) neutrons = neutrons = neutrons = neutrons = neutrons = 19, Cl 47, Kr 54, Kr 54, Mo 54, Nb 25. A box of dimensions 2.00 inches 3.50 inches 2.500 inches (1 inch = 2.54cm) has a volume closest to a) b) c) d) e) 0.2868 L 17.5 L 0.287 L 0.04445 L 0.0444 L 26. Determine the number of moles of carbon dioxide produced in the following unbalanced combustion reaction. C8H17OH 2 8 6 12 18 + O2 CO2 + H2 O 27. What is the chemical formula given the following elemental analysis. 168.15g C, 20.16g H, 28.014g N, 32.06g S, 63.99 O a) b) c) d) e) C7H10NSO2 C30H20N2S4O4 C16H2N3S3O6 C16H20N28S32O63 C14H20N2SO4 28. How many grams of NaH2PO4 are needed to react with 38.74 mL of 0.275 M NaOH? NaH2PO4(s) + NaOH(aq) Na3PO4(aq) + H2O(l) a) b) c) d) e) 0.6392 0.2500 1.278 12.00 0.0106 4 29. In the following unbalanced reaction 8.00 g of oxygen are used to produce 2.14 g of HCN. What is the percent yield of HCN produced? NH3(g) + O2(g) + CH4(g) HCN(g) + H2O(l) 30. Given that 41.4 g of water reacts with 42.0 g of C 3H8, the limiting reactant is: C3H8 + H2O CO + H2 a) H2O b) C3H8 c) CO d) H2 e) None of these 31. The volume of 0.100 M Ba(OH)2(aq) solution needed to prepare 6.30 L of 0.003 M Ba(OH)2(aq) solution is 6.3 L 0.189 L 33.3 L 0.03 L 3.0 L 32. The chemical formula for a compound with the empirical formula C7H4O2 and a formula weight of 240.2 g/mol is a) b) c) d) e) C7H4O2 C13H4O5 C21H12O6 C14H8O4 C3.5H2O 33. The formula of Vitamin C is C6H8O6. How many moles of Vitamin C are there in two 500 mg tablet? a) b) c) d) e) 1.000 5.68 0.176 2.84 10-3 5.68 10-3 5 34. The number of chlorine atoms in one mole of aluminum chloride is approximately: a) b) c) d) e) 3 35.5 6.02 1023 18.06 1023 2.01 1023 35. Potassium nitrate decomposes on heating, producing potassium oxide, gaseous nitrogen and gaseous oxygen. Choose the closest number of grams of KNO3 that must decompose in order to produce 1.35 g of O2 (in the original exam the chemical formula was given…but I want you to write chemical equation for practice). a) b) c) d) e) 4.26 6.82 3.41 5.33 0.0338 36. The density of mercury (Hg) is 13.5 g/mL. If a chemist wants to add 2.00 moles of Hg to a reaction vessel, how many milliliters should he add? a) b) c) d) e) 401 29.7 7.38 10-4 mL 7.43 14.8 37. If 2.50 moles of H2 reacts with Cl2 to form HCl according to the following unbalanced equation, what number below is closest to the number of moles of HCl produced? H2(g) + Cl2(g) HCl(g) a) b) c) d) e) 1.25 5.00 2.50 3.75 0.625 6 38. Indicate whether the reactants and products are either a Solid (s), Gas (g) or Soluble in Water (aq) in the following double-replacement reactions. a) 2NaOH + Cd(NO3)2 Cd(OH)2 + 2NaNO3 b) 2NaI + PbNO3 2NaNO3 + PbI2 39. Using solubility rules to determine which of the following are soluble = Aquous (aq) or insoluble = Solid (s) in water. Ba(OH)2, BaSO4, BaS, Ba(NO3)2 40. How many grams of salt (NaCl mw = 58.44 g/mol) are needed to make 65.0 mL of a 0.220 % saline solution? 41. What is the mass percent in a solution containing 12.1 g of NaCl and 150.1 g water? 42. Calculate the number of grams of solute in the following: 50.0 mL of a 12.0 M HNO3 solution 43. Calculate the number of grams of solute in the following: 1.20 L of a 0.0032 M Na2SO4 solution 44. Calculate the molarity of the following: 14.0 g silver Nitrate (AgNO3) in 1.00 L of solution. 45. Calculate the molarity of the following: 0.025 mol of potassium chloride (KCl) in 50.0 mL of solution 46. describe what a colligative property is and what type of formulas are based on colligative properties. 47. Determine the final concentration of a solution by adding 45 mL of water to 90.0 mL of a 3.0 M NaCl solution. 7 48. Determine how many L of water must be added to 34.5 mL of a 12.0 M solution of nitric acid (HNO3) to make a 4.0 M solution. 49. Classify the following reaction as either a combination, decomposition, single replacement, or double displacement reaction. a) 2NaHCO3 Na2CO3 + CO2 + H2O b) 2Fe + 3Cl2 2FeCl3 50. Which of the following is Not a redox reaction? a) 2CuO 2Cu + O2 b) 2KClO3 2KCl + 3O2 c) CaCO3 CaO + CO2 51. Determine the oxidation number (oxidation state) of all the elements in the following reactions. a) Mg + 2HCl MgCl2 + H2 b) 2SO2 + O2 2SO3 c) 2Fe2O3 + 3C 4Fe + 3CO2 52. Which species (elements) are oxidized and which are reduced in the following reaction. a) Zn + CuCl2 ZnCl2 + Cu b) 3H2S + 2HNO3 3S + 2NO + 4H2O c) 2FeBr3 2FeBr2 + Br2 53. What is the correct Eeq for the following reactions: a) 2 NH4ClO4 N2 + Cl2 + 2O2 + 4H2O b) 2C6H6 + 15O2 12CO2 + 6H2O (this is the space shuttle fuel) 54. The oxidation number (oxidation state) of sulfur in the following are? K2SO2, K2S2O3, K2S 8 55. According to Le Chatelier’s principle what effects will take place on the equilibrium of the following reaction: CO2 + H2 H2O + CO a) Increase [H2] b) Increase [H2O] c) remove H2O and CO 56. Calculate the equilibrium constant for: N2O4 2NO2 [N2O4] = 0.12 M [2NO2] = 0.55 M 57. The answer that is closest to the number of grams of oxygen in 6.022 1023 molecules of O2 is: 1) 1.0 4) 64.0 2) 16.0 5) 6.022 1023 3) 32.0 58. Both water and sulfur dioxide are produced from the reaction of sulfuric acid (H 2SO4) with copper metal in the following balanced equation. How many moles of H2O will be produced at the same time that 10.0 moles of SO2 is produced? 2H2SO4 + Cu SO2 + 2H2O + CuSO4 1) 5 4) 25 2) 10 5) 30 3) 20 59. Chlorophyll, essential to plants for photosynthesis, contains one magnesium atom, three oxygen atoms, four nitrogen atoms, thirty three carbon atoms and twenty nine hydrogen atoms. What is the chemical formula for chlorophyll? 1) FeO3N4Ca33Hy29 2) Mn3O4N33C29H 3) NaO3Ni4Ca33H29 4) MgO3N4C33H29 5) MnO3N4C33H29 60. Vitamin C (mw = 176.12 g/mol) contains 40.9% C, 4.6% H and 54.5% O. What is the molecular formula of Vitamin C 9 61. If there are 2.62 1022 atoms in 1.00 g of sodium and they are lined up side by side, what is the length of the line of sodium atoms in miles? Assume that the atoms are spheres of diameter 0.372 nm. 62. Mystery element X combines with sulfur to form the compound X 4S3 . The molecular mass of X4S3 is 220.09 amu. Mystery element X is: 62. What is the percent yield of sodium carbonate if 1.254 g of sodium hydrogen carbonate (84.01 g/mol) decomposes to give 0.765 g of sodium carbonate (105.99 g/mol)? 2NaHCO3 (s) Na2CO3 (s) + H2O (g) + CO2 (g) a) 48.4% b) 96.7% c) 100% d) 103% e) 206% 63. What mass of BaSO4 is produced by starting with 12.1 g of Fe2(SO4)3, in the following balanced reaction? 3BaCl2 (aq) + Fe2(SO4)3 (aq) 3BaSO4 (s) + 2FeCl3 (s) -4 1) 8.98 10 4) 4.03 2) 2.34 5) 21.2 3) 3.03 64. Draw the Lewis dot structure for Barium, Lead, Bismuth, Polonium, and Radon 65. Draw the Lewis structure SF2 66. Draw a 3-D diagram for each molecule and indicate if the molecule is polar or non-polar. a. OF2 b. PBr3 67. Draw the 3-D structure. Give the VSEPR electron-pair name, the molecular shape name for the following. a. NF3 b. CCl4 c. CF368. Draw and example of hydrogen bonding between NH3 and HF 10 69. Would you expect the following pairs to be soluble with each other? a. CH4 with H2O H b. CH2F2 with H C O H H TOPICS: Lewis Dot Lewis Structure VESPR Class name VESPR Molecular Shape name Polarity Solubility: the phenomena is Likes Dissolve Likes, the fact is molecules dissolve if they have the same solubility Melting and Boiling Points Mole Amu, Molar Mass Empirical and Molecular Formula Balancing Chemical Formulas Limiting Reagents Theoretical and Percent Yield 11 KEY 1. Ans. [H3O+] = 3.7 10-4 What is the [OH-] concentration? pKw = pH + pOH 14 = 3.43 + pOH pOH=10.57 pOH=-log[OH-] -antilog (pOH)=[OH-] =2.69 10-11 2. Ans. B<D<A<C 3. HCl = acid, Cl- conjugate base, NH3= base, NH4+ conjugate acid 4. Ans = 8 moles 5. Ans 0.639 6 ans 4.51 7. Ans. 4.00 8. PV=nRT n = PV/RT=1 35.6 /0.0821 (25+273) = 9. Ans.0.639 10. Al ox, O2 red, Al RA, O2 OA 11. 12 Ans: 1 lone pair on Carbon 12. Trigonal Pyramidal 13. Ans. 4 14. [Ar] 4s23d104p4 15. Ans: 12 16. ans. 192.2200 17. heat absorbed = specific heat * mass * temp change 9.80 103 cal/(g C) 18. Ans: b 19. 100 mL 20. Ans e 21. Ans c 22. Ans a 23. 1oz/28.35g * 19.3g/mL * 1mL/cm3 * (100 cm/m)^3 * .02832m^3/1ft^3 * 1ft^3 = 19280 oz 13 24. Ans: e 25. 2in x 2.54cm/1in = 5.08cm 3.5in x 2.54cm/1in= 8.89 cm 2.5in x 2.54cm/1in=6.35 cm = 287 cm^3 * 1mL/1cm^3 * 1L/1000mL = .287L 26. Ans: 12 27. Ans: e 28. NaH2PO4(s) + 2NaOH(aq) Na3PO4(aq) + 2H2O(l) 1mol NaH2PO4/2mol NaOH x .275molNaOH/1L * .03864L NaOH /1 * 119g NaH2PO4/1mol NaH2PO4 Ans: a 29. Ans: 47.6% 30. C3H8 + 3H2O 3CO + 7H2 41.1 g water * 1mol water/18g water * 3 molCO/3molwater = 2.28 mol CO 42.0 g C3H8 * 1mol C3H8/44gC3H8 * 3molCO/1molC3H8 = 2.86 mol CO Ans: water 31. M1V1=M2V2 (6.3)(.003)/.1 = .189L 32. Ans: d 33. Ans E 34. 14 Ans: a 35. Ans: c 36. Ans: b 37. Ans: b 38. ans. 2NaOH (aq) + Cd(NO3)2(aq) Cd(OH)2(s) + 2NaNO3(aq) b) 2NaI(aq) + PbNO3(aq) 2NaNO3(aq) + PbI2(s) 39. ans. Ba(OH)2 (aq) , BaSO4 (s) , BaS (s) , Ba(NO3)2 (aq) 40. Ans. (0.220 g NaCl/100 mL solution) 65.0 mL solution = 0.143 g NaCl 41. Ans. 12.1 g NaCl /(12.1 g NaCl + 150.1 g water) 100 = 7.57 % 42. M = mol/L, mol = M L, 50.0 mL 1L/1000mL 12.0 M = 0.600 mol HNO3, mol = g/mw, g = mol mw = 0.600 mol 63.01 g / mol = 37.81 g HNO3 43. M = mol/L, mol = M L = 1.20 L 0.0032 M = 0.0038 mol Na2SO4, mol = g /mw, g = mol mw = 0.0038 g/mol 142.04 g/mol = 0.545 g 44. Mol = g mw = 14.0 g mol/169.87 g = 0.0824 mol, M = mol/L = 0.0824 / 1.00 L = 0.0824 M 45. M = mol/L = 0.025 mol / (50.0 mL 1L/1000mL) = 0.500 M 46. depends on the number of particles, molatiy is the standard unit, Freezing point depression formulas, boiling point elevation, and osmolatiry. 15 47. M1V1=M2V2, M2 = M1V1/V2 = 135 mL 3/45 mL = 2.0 M 48. M1V1= M2V2, V2 = M1V1/M2 = 34.5 mL 12/4 = 103.5 mL = 0.104 L 49. a) 2NaHCO3 Na2CO3 + CO2 + H2O b) 2Fe + 3Cl2 2FeCl3 decomp combination 50. Ans C 51. Determine the oxidation number (oxidation state) of all the elements in the following reactions. a) Mg + 2HCl MgCl2 + H2 b) 2SO2 + O2 2SO3 c) 2Fe2O3 + 3C 4Fe + 3CO2 0, 1+1- 2+1-, 0 4+2-, 0 6+23+2-, 0 0, 4+2- 52. Which species (elements) are oxidized and which are reduced in the following reaction. a) Zn + CuCl2 ZnCl2 + Cu b) 3H2S + 2HNO3 3S + 2NO + 4H2O c) 2FeBr3 2FeBr2 + Br2 Zn Ox/RA, Cu2+ Red/OA S Ox/RA, N Red/OX Fe Red/OA, Br Ox/RA 53. K=[prod]a/[reactans]b 54. Ans: 2+, 4+, 255. a) Increase [H2] b) Increase [H2O] c) remove H2O and CO shift to right shift to left shift to right 56. ans. = 2.5 16 57. Ans: 32 g or 3 58. Ans 20 moles, 3 59. Ans: 4 60. Ans: C6H8O6 61. 1mile/5280 ft * 1ft/12in * 1in/2.54cm * 100cm/1m * 10^-9m/nm * .372nm/atom * 2.62x10^22/1atom = 6,060,000,000 miles 62. S 32.1X3=96.3 220-96.3 = 123.7 123.7/4=30.9=P Ans: P 62. 1.254g/1 * 1mol/84.01 * 1/2 * 105.99 = .79g .765/.791 * 100 = 96.7% 63. Ans: 5 64. Ba 2 dots, Pb has 4 dots, Bi has 5 dots, Po has 6 dots, Ra has 8 dots 65. Ans: electron pair name is tetrahedral, molecular shape name is “V” bent 66. Draw a 3-D diagram for each molecule and indicate if the molecule is polar or non-polar. a. OF2 POLAR b. PBr3 POLAR 67. Draw the 3-D structure. Give the VSEPR electron-pair name, the molecular shape name for the following. a. NF3 tetrahedral/trigional pyramidal b. CCl4 tetrahedral/tetrahdral c. CF3 tetrahedral/trigional pyramidal 17 68. H-F-------H-NH2 F-H------NH3 69. Would you expect the following pairs to be soluble with each other? a. CH4 with H2O NO, CH4 is nonpolar, and water is polar H b. CH2F2 with H C O H YES, both are polar H 18