Final Exam Review Problems
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FINAL EXAM REVIEW PROBLEMS
The following problems are similar to the questions that will appear on your final exam. This review is NOT inclusive of all the possible questions that might be asked.
1. Write the numbers 4300 and 0.0102 in scientific notation.
2. Give the number of significant figures for each of the following: a. 0.00100 b. 2.0800 x 102 c. 480
3. Give the answer for each calculation to the correct number of significant figures: a. 12.6 X 0.53 b. (25.36 –4.15)2.317 c. (2.6 x .42) – 4.59
4. Which temperature is colder, 172 K or -75C?
5. An antifreeze solution in a car’s radiator boils at 239F. What is the temperature on the Celsius scale?
6. A student wants to identify the main component in a commercial liquid cleaner. He finds that 35.8 mL of the cleaner weighs 28.1 g. Of the following possibilities, which is the main component of the cleaner? chloroform 1.483 g/mL diethyl ether 0.714 g/mL isopropyl alcohol 0.785 g/mL toluene 0.867 g/mL
7. Which of the following are physical properties and which are chemical properties?
a. Gallium metal melts in your hand.
b. Platinum does not react with oxygen at room temperature.
c. This page is white.
d. Copper forms a greenish coating over years.
8. How many calories of energy correspond to 33.6 J?
9. Calculate the joules of energy required to heat 298 g of water from 7.6C to 81.5C?
10. A 5.63 g sample of metal is heated from 21C to 32C. This change in temperature requires 8.05 J of energy. What is the specific heat capacity of this metal?
11. Write the formula for each of the following compounds, list the elements in order given:
a. A molecule contains four phosphorus atoms and ten oxygen atoms
b. A molecule contains one sulfur atom and six fluorine atoms
c. A molecule contains one aluminum atom and three chlorine atoms 12. Give the number of protons, neutrons, and electrons for the following atoms: Sr, Hg, and C.
13. Give the isotope symbol for the phosphorus atom (Z=15) that contains 17 neutrons.
14. Name the following compounds.
a. Rb2O b. SrI2 c. K2S As needed, show all work on Separate Paper. You may not turn in these questions to show your work.
15. Give the names of the following compounds.
a. PbBr2 and PbBr4 b. FeS and Fe2S3
16. Name the following compounds.
a. CCl4 b. NO2 c. IF5
17. Name the following compounds
a. ClF3 d. HCl
b. HC2H3O2 e. HNO3
c. CuCl f. H2SO3
18. Name the following compounds.
a. NaHCO3 d. CsClO4
b. (NH4)2Cr2O7 e. Zn3(PO4)2
c. Cu(NO2)2 f. KMnO4
19. Write the formula for each of the following compounds. a. ammonium sulfate e. aluminum oxide b. vanadium (V) fluoride f. lead (IV) oxide c. disulfur dichloride g. cobalt (III) nitrate d. rubidium peroxide h. calcium chloride
20. Write the formula for each of the following. a. nitrous acid c. hydroiodic acid b. bromic acid d. phosphoric acid
21. Identify the reactants and products and write the unbalanced equation (including symbols for states) for each of the following chemical reactions.
a. Solid magnesium metal reacts with liquid water to form solid magnesium hydroxide and hydrogen gas.
b. Solid ammonium dichromate decomposes to solid chromium (III) oxide, gaseous nitrogen and hydrogen gas.
c. Gaseous ammonia reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.
22. Give the balanced equation for each of the following reactions.
a. When solid ammonium nitrite is heated, it produces nitrogen gas and water vapor.
b. Gaseous nitrogen monoxide decomposes to produce dinitrogen monoxide gas and nitrogen dioxide gas.
c. Liquid nitric acid decomposes to reddish brown nitrogen dioxide gas, liquid water, and oxygen gas.
23. Predict whether a solid will form when the following pairs of solution are mixed. If so, identify the solid and write the balanced equation for the reaction.
a. Ba(NO3)2 (aq) and NaCl(aq)
b. Na2S(aq) and Cu(NO3)2 (aq)
c. NH4Cl(aq) and Pb(NO3)2 (aq)
24. For each of the following reactions, write the molecular equation, the complete net ionic equation, and the net ionic equation. As needed, show all work on Separate Paper. You may not turn in these questions to show your work.
a. Aqueous sodium sulfide is mixed with aqueous copper (II) nitrate to produce solid copper (II) sulfide and aqueous sodium nitrate.
b. Aqueous ammonium chloride and aqueous lead (II) nitrate react to form solid lead (II) chloride and aqueous ammonium nitrate.
25. Classify each of the following reactions in as many ways as possible.
a. 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g)
b. S8 (s) + 8 O2 (g) 8 SO2 (g)
c. 2 Al(s) + 3 Cl2(g) 2 AlCl3 (s)
d. 2 AlN (s) 2 Al(s) + N2 (g)
e. BaCl2 (aq) + Na2SO4 (aq) BaSO4 (s) + 2 NaCl (aq)
f. 2 Cs (s) + Br2 (l) 2 CsBr (aq)
g. KOH (aq) + HCl (aq) H2O (l) + KCl (aq)
h. 2 C2H2 (g) + 5 O2 (g) 4 CO2 (g) + 2 H2O (l) 26. Predict the products of each reaction, balance the equation and classify the reactions in as many ways as possible.
a. Ca(OH)2 (aq) + 2 HNO3 (aq)
b. 2 NaI (aq) + Br2 (l)
c. 2 Zn(s) + O2 (g)
d. 2 NaCl (s)
e. 2 C8H18 (g) + excess 25 O2 (g)
f. Li2SO4 (aq) + BaCl2 (aq)
27. Calculate the number of moles and the mass of a sample of chromium containing 5.00 x 1018 atoms.
28. Calculate the molar mass of HC2H3O2.
29. A 314.5 g sample of sodium sulfite represents how many moles?
30. Calculate the mass percent of each element in C14H20N2SO4.
31. In an experiment it was observed that 0.6884 g of lead combines with 0.2356 g of chlorine to form a binary compound. Calculate the empirical formula of this compound.
32. A compound used as an additive in gasoline is 71.65% Cl, 24.27% C, and 4.07% H. The molar mass is 98.96 g. Determine the empirical formula and the molecular formula.
33. Calculate the moles of CO2 formed when 4.30 mol of C3H8 reacts with the required 21.5
mol of O2.
34. What mass of carbon dioxide is produced when 82.6 g of C3H8 reacts with sufficient oxygen?
35. Calculate the mass of lithium nitride formed from 56.0 g of nitrogen gas and 56.0 g of
lithium: 6 Li(s) + N2 (g) 2 Li3N (s)
36. TiCl4 (g) + O2 (g) TiO2 (s) + 2 Cl2 (g) 3 3 a. Suppose 6.71 x 10 g of titanium (IV) chloride is reacted with 2.45 x 10 g of oxygen. Calculate the maximum mass of titanium (IV) oxide that can form.
b. If the percent yield of TiO2 is 75%, what mass was actually produced?
37. Define the following terms: As needed, show all work on Separate Paper. You may not turn in these questions to show your work.
a. principle energy level c. orbital size b. orbitals d. sublevel
38. Write the complete electron configuration and the orbital diagram for aluminum, chlorine, argon, and copper.
39. Using your periodic table, write the noble gas configurations for fluorine, silicon, cesium, lead, and iodine.
40. For each of the following pairs of bonds, choose the bond that will be more polar. a. H-P or H-C b. O-F or O-I c. N-O or S-O d. N-H or Si-H
41. Draw the Lewis structure for each of the following (Five step math is optional):
a. CO2 d. CF4 + b. N2 e. NO - c. NH3 f. NO3
42. Sketch and give the name for the shape of each of the following molecules or ions: + a. NH4 d. H2S -2 - b. SO4 e. ClO3
c. NF3 f. BeF2
43. A sample of neon to be used in a neon sign has a volume of 1.51 L at a pressure of 615 torr. Calculate the volume of the gas after it is pumped into the glass tubes of the sign, where it shows a pressure of 795 torr.
44. A child blows a bubble that contains air at 28C and has a volume of 23 mL at 1 atm. As the bubble rises, it encounters a pocket of cold air. If there is no change in pressure, will the bubble get larger or smaller as the air inside cools to 18C? Calculate the new volume.
45. Consider two sample of nitrogen gas. Sample 1 contains 1.5 mol of N2 and has a volume of 36.7 L at 25C and 1 atm. Sample 2 has a volume of 16.5 L at 25C and 1 atm.
Calculate the number of moles of N2 in sample 2.
46. A weather balloon contains 1.10 x 103 mol of helium and has a volume of 2.70 x 104 L at 1.00 atm of pressure. Calculate the temperature of the helium in the balloon in Kelvin and in degrees Celsius.
47. A 2.0 L flask contains a mixture of nitrogen gas and oxygen gas at 25C. The total pressure of the gaseous mixture is 0.91 atm and the mixture is known to contain 0.050
mol of N2. Calculate the partial pressure of oxygen and moles of oxygen present.
48. Calculate the volume of hydrogen produced at 1.25 atm and 19C by the reaction by the reaction of 24.3 g of zinc with excess HCl according to the equation:
Zn + 2 HCl ZnCl2 + H2
49. A sample of NH3 occupies 5.00 L at 23C and 13.5 atm. What volume will the sample occupy at STP? 50. A 126 g sample of seawater is evaporated to dryness, leaving 4.73 g of solid residue. Calculate the mass percent of solute present in the original seawater. As needed, show all work on Separate Paper. You may not turn in these questions to show your work.
51. What mass of water must be added to 425 g of formaldehyde to prepare a 40.0% solution of formaldehyde?
52. Calculate the molarity of a solution prepared by dissolving 2.75 g of ethanol, C2H5OH, in enough water to give a final volume of 101 mL.
53. Give the concentrations of the ions in each of the following solutions:
a. 0.10 M Na2CO3
b. 0.010 M Al2(SO4)3
- -3 54. Calculate the number of moles of Cl ions in 1.75 L of 1.0 x 10 M AlCl3.
55. What volume of 12 M HCl must be taken to prepare 0.75 L of 0.45 M HCl?
56. When aqueous Na2SO4 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the PbSO4
formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M Na2SO4 are mixed.
57. Calculate the volume of 0.10 M HNO3 needed to neutralize 125 mL of 0.50 M KOH.
58. What volume of 0.50 N H2SO4 is required to react exactly with 0.250 L of 0.80 N KOH?
59. Write the equilibrium expression for each of the following reactions:
a. 4 NH3 (g) + 7 O2 (g) 4 NO2 (g) + 6 H2O (g)
b. S(s) + O2 (g) SO2 (g)
c. P4 (g) + 6 Cl2 (g) 4 PCl3 (g)
d. 2 AlCl3 (s) 2 Al (s) + 3 Cl2 (g)
60. For each of the following reactions, predict the direction the equilibrium will shift when the volume of the container is increased.
a. H2 (g) + F2 (g) 2 HF (g)
b. CO (g) + 2 H2 (g) CH3OH (g)
c. 2 SO3 (g) 2 SO2 (g) + O2 (g)
61. For the exothermic reaction: 2 SO2 (g) + O2 (g) 2 SO3 (g)
a. SO2 is added
b. SO3 is removed c. The volume is decreased d. The temperature is decreased
62. Write the balanced equation for the reaction describing the dissolving of each of the
following solids in water. Also write the Ksp expression for each solid. Skip
a. BaSO4 b. Fe(OH)3 c. Ag3PO4
-5 63. Calculate the Ksp value for barium sulfate, which has a solubility of 3.9 x 10 M at 25C. skip
-16 64. The Ksp value for PbCrO4 is 2.0 x 10 at 25C. Calculate the solubility. Skip
65. Which of the following represent conjugate acid-base pairs? + - -2 - a. H2O,H3O b. OH ,HNO3 c. H2SO4,SO4 d. HC2H3O2,C2H3O2
66. Calculate the [H+] in a solution in which [OH-] = 2.0 x 10-2M. Is this solution acidic, neutral, or basic? As needed, show all work on Separate Paper. You may not turn in these questions to show your work.
67. Calculate the pH value for each of the following solutions at 25C: a. A solution in which [H+] = 1. x 10-3 M b. A solution in which [OH-] = 5.0 x 10-5 M
68. A sample of rain in an area with severe air pollution has a pH of 3.5. What is the pOH of this rainwater?
69. The pOH of a liquid drain cleaner was found to be 10.50. What is the [OH-] for this cleaner?
70. The pH of rainwater in a polluted area was found to be 5.75. What is the [H+]?
71. Calculate the pH of a solution of 5.0 x 10-3 N HCl.
72. Given the following data:
Fe2O3 (s) + 3 CO (g) 2 Fe (s) + 3 CO2 (g) H = -23 kJ
3 Fe2O3 (s) + CO (g) 2 Fe3O4 (s) + CO2 (g) H = -39 kJ
Fe3O4 (s) + CO (g) 3 FeO (s) + CO2 (g) H = 18 kJ
Calculate the H for FeO (s) + CO (g) Fe (s) + CO2 (g)
73. Perform the indicated conversions. a. 45.62 kcal to kJ c. 72.94 kJ to kcal b. 2.751 kJ to cal d. 5.721 kcal to J
74. Are the following processes exothermic or endothermic? a. When solid KBr is dissolved in water, the solution gets colder.
b. CH4 is burned in a furnace. c. When concentrated sulfuric acid is added to water it gets very hot. d. Water is boiled in a tea kettle.
75. Given the following data:
2 O3 (g) 3 O2 (g) H = -427 kJ
02 (g) 2 O (g) H = 495 kJ
NO (g) + O3 (g) NO2 (g) + O2 (g) H = -199 kJ
Calculate the H for NO (g) + O (g) NO2 (g)