Time

Increasing Temperature

A

B

C

D E

Honors Chemistry Name ____________________________________________Final Exam Review Test Date: ____________ Time: ______________________

Room #: ______________ Proctor: ____________________

Unit 1: Measurement

1. A block of sodium with measurements 4.00 cm x 3.00 cm x 6.25 cm has a measured mass of 76.1 g. The accepted density for sodium if 0.971 g/cm3. Calculate the percent error.

2. A 49.5 gram sample of tin at 95.0°C is placed into 145 grams of water. The water and tin reach thermal equilibrium at a temperature of 26.1°C. What was the initial temperature of the water?

a. 22.4 °C b. 24.9 °C c. 27.3 °C d. 29.8 °C

3. If 145 J of heat are added to an unknown metal of mass 121 g, the temperature of the metal goes from 22.2°C to 24.3°C. Calculate the specific heat of the metal.

Unit 2: Matter & Energy

4. Benzene, C6H6, boils at 80.1˚C and has a density of 0.877 g/cm3. Determine the quantity of heat that is required to vaporize a 45.6 mL sample of benzene at 35.0˚C.

a. 3140 J b. 4370 J c. 15800 J d. 18900 J

5. If a gas’s temperature increases, what happens to the pressure and volume? a. Pressure increases and volume increasesb. Pressure decreases and volume decreases

c. Pressure decreases and volume increasesd. Pressure increases and volume decreases

6. A gas is collected over water in a eudiometer tube until the pressure is equilibrated with the atmospheric pressure. The volume of gas in the eudiometer is 28.5 mL. The temperature of the water is 36.0°C and the barometric pressure is 758 mm Hg. What is the volume of this gas at STP?

a. 23.6 mL b. 25.1 mL c. 30.3 mL d. 32.2 mL

7. Which of the following occurs during a phase change? a. Temperature increasesb. Kinetic energy increasesc. Heat energy increasesd. All of the above

8. Which lettered region represents the phase with the highest intermolecular forces?

a. Ab. Bc. Cd. De. E

9. A balloon is filled to a volume of 745 mL with 158 grams of steam at 112°C. After a brief period of cooling, the balloon’s volume is measured to be 735 mL. How much heat energy did the steam lose?

Unit 3: Atomic Theory & Nuclear

10. Complete the following chart:

Isotopic Symbol Isotope Name Atomic

NumberMass

Number # protons # electrons # neutrons

a O816

b manganese-56

11. If samples of two different elements each represent one mole, thena. they are equal in mass.b. they contain the same number of atoms

c. their molar masses are equald. they have the same atomic mass

12. Calculate the number of atoms in 10.0 g of aluminum.

13. Determine the mass in grams of 5.00 x 1023 mol of oxygen atoms.

14. Write balanced nuclear equations for the following:a. Alpha-particle bombardment of plutonium-239 produces a neutron and another isotope. b. With what particle would you bombard sulfur-32 with to produce hydrogen-1 and phosphorus-32?

15. A 900. mg sample of platinum-197 is found to have a mass of 56.3 mg after exactly 3 days. What is the half-life of platinum-197 in hours?

a. 24 hrs b. 18 hrs c. 0.75 hrs d. 16 hrs

Unit 4: Chemical Compounds

16. Write the name if given the formula or the formula if given the name.

a.HBr(aq) _____________________________

b.Cu2C2O4 _____________________________

c.Cl2O7 _____________________________

d.Al(ClO4)3 _____________________________

e.Fe(NO3)3 • 9H2O ___________________________

f. SO3_____________________________

g.HNO2 (aq) _____________________________

h.Pb(Cr2O7)2 _____________________________

i. N2O5 _____________________________

j. H3BO2 (aq) _____________________________

k.SnBr4 _____________________________

l. Ti(IO)3 _____________________________

m. Ga2(WO3)3 _____________________________

n.molybdous acid ___________________________

o.calcium phosphate _________________________

p.arsenic triiodide ___________________________

q.magnesium sulfate heptahydrate ______________

r. iron(III) carbonate _________________________

s. sodium acetate ___________________________

t. manganese(IV) telluride ____________________

u.scandium arsenite _________________________

v.tetraphosphorous decoxide ___________________

w. phosphorous acid ________________________

x.hydroselenic acid __________________________

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y.acetic acid ______________________________ z.platinum(II) perbromate _____________________

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17. Determine the percent composition of manganese(VII) arsenate.

18. How many electrons are present in a 20.54 gram sample of calcium ions?

19. What mass of aluminum hypochlorite contain 1.574 x 1023 hypochlorite ions?

20. An unknown gas has an effusion rate that is 0.845 times that of dinitrogen pentoxide. What is the molar mass of the unknown gas?

Unit 5: Mole

21. The following pertains to the compound, potassium hypomolybdite.

a. Calculate the mass of oxygen in potassium hypomolybdite if there are 3.91x1024 formula units.

b. Calculate the total number of ions in 154.3 g of potassium hypomolybdite.

c. Calculate the mass of potassium hypomolybdite needed to make 250. mL of a 0.500 M solution.

22. An unknown gas was collected over water. Determine the molar mass of the unknown gas if a 0.167 g sample occupies a volume of 69.8 mL at 60.0°C. The barometric pressure is 752.8 torr.

23. An unknown gas is determined to have an empirical formula of CH2. If a 0.176 g sample of this gas occupies a volume of 35.0 mL at 134 kPa and 175°C, determine its molecular formula.

24. 123g of sucrose is dissolved in 568g of water. The solution has a density of 1.34g/ mL. Determine the molarity and molality of the solution.

25. A compound is found to be 47.1% carbon, 6.54%H, and 46.4% chlorine. The rate of effusion of this compound in the gaseous state was measured relative to oxygen gas. Nitrogen was found to effuse at rate that was 2.34 times faster than this compound. Determine the molecular formula of the compound.

Unit 6: Chemical Equations

26. Calculate ∆H for the reaction 2Al (s) + 3Cl2 (g) 2AlCl3 (s) from the data.2Al (s) + 6 HCl (aq) →2 AlCl3 (aq) + 3 H2 (g) ∆H = -1049.0 kJHCl (aq) →HCl (g) ∆H = +74.8 kJ2 H2 (g) + 2 Cl2 (g) → 4 HCl (g) ∆H = -3690.0 kJAlCl3 (s) →AlCl3 (aq) ∆H = -323.0 kJ

27. Using bond energies, calculate the enthalpy change for the following reactions:

28. Using bond energies, calculate molar heat of combustion for 1 mole of methane (CH4):

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29. Write complete balanced chemical equations. Indicate precipitate for double replacement reactions.

a. Zinc carbonate decomposes.b. Strontium is mixed with chlorine gas.c. Combustion of octane.d. Iron is added to acetic acid.e. Potassium oxide is mixed with water.f. Lithium chlorate decomposes. g. Potassium hydroxide is added to sulfuric acid.h. Sulfur trioxide is bubbled through water. i. Zinc is dropped into hydrochloric acid.j. Decomposition of calcium oxide.k. Gold metal dropped into sulfurous acid.l. Silver nitrate is added to ammonium phosphate. m. Fluorine is added to sodium bromide.n. Carbonic acid is heated.

Unit 7: Stoichiometry

30. Given the reaction of propane (C3H8) burning in air, how many grams of oxygen gas are required to burn 3.01 1023 propane molecules?

a. 80.0 g b. 40.0 g c. 160 g d. 16.0 g e. 64.0 g

31. The following statements apply to the interpretation of chemical equations. Not all of the statements are true. Which response includes all of the true statements, and no others?

I. The sum of the number of moles of the reactants must equal the sum of the number of moles of products in a balanced equation.

II. The sum of the number of grams of the reactants that react must equal the sum of the number of grams of the products produced by the reaction.

III. The following equation for the reaction involving hypothetical substances, A, B, C, and D, implies that the products C and D are always produced in a three to one mole ratio. A + 2B 3C + D

IV. The equation shown in III implies that in any reaction involving A and B as reactants, A must be the limiting reactant.

V. The total number of atoms in the reactants that react must always equal the total number of atoms in the products produced by the reaction.

a. I and V b. I, II, and III c. II, IV, and V d. II, III, and V e. III, IV, and V

32. The thermite reaction is performed using 8.6 g iron(III) oxide and 1.8 g powdered aluminum metal. Which reactant is in excess and by how much?

a. Al, 0.3 g b. Fe2O3, 2.0 g c. Al, 2.1 g d. Al, 1.1 g e. Fe2O3, 3.3 g

33. Suppose 600. g of phosphorus reacts with 1300. g of sulfur in a synthesis reaction. How many grams of tetraphosphorus decasulfide can be produced, assuming an 80.0% yield for the reaction

a. 4.62x102 g b. 1.44x103 gc. 2.16x103g d. 4.92x103g e. 6.50x102g

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34. Sulfuric acid can be produced by a three step process. First, sulfur is burned in air to give sulfur dioxide. Second, the sulfur dioxide is converted to sulfur trioxide by passing the sulfur dioxide over a catalyst in the presence of oxygen at a high temperature. Third, the sulfur trioxide is reacted with water to form sulfuric acid. What mass of sulfuric acid would be formed from 1.00 x 103 kg of sulfur, if the three steps gave yields as listed below?

S + O2 → SO2 92.5%2SO2 + O2 → 2SO3 72.6%SO3 + H2O → H2SO4 98.2%

a. 4.03 x 103 kg b. 2.02 x 103 kg c. 3.06 x 103kg d. 2.84 x 103kg e. 2.22 x 103kg

35. What mass of a 25.0% barium nitrate solution contains 40.0 grams of barium nitrate?a. 117 gb. 160 g

c. 321 gd. 10.0 g

e. 62.5 g

36. If 45.0 mL of 0.250 M lead(IV) chloride solution reacts with 20.0 mL of ammonium sulfate, what is the molarity of the ammonium sulfate solution?a. 0.502 Mb. 1.25 M

c. 2.25 Md. 1.13 M

e. 0.563 M

37. What mass of calcium carbonate is required to react with 100. mL of a 2.00 M hydrochloric acid solution?a. 5.00 gb. 10.0 g

c. 15.0 gd. 20.0 g

e. 23.0 g

38. What volume of 0.0750M barium hydroxide will completely react with 125 mL of 0.0350M hydrochloric acid?a. 29.2 mLb. 42.0 mL

c. 230. mLd. 536 mL

e. 53.6 mL

39. What is the molarity of a sulfurous acid solution if 23.7 mL of this solution requires 16.8 mL of 0.296M sodium hydroxide for titration to its endpoint?a. 0.210 Mb. 0.358 M

c. 0.105 Md. 0.421 M

e. 0.0525 M

40. How much heat is evolved in the formation of 35.0 grams of iron(III) oxide from its elements at 25°C and 1.00 atm pressure?a. 90.4 kJb. 180.7 kJ

c. 151 kJd. 360.1 kJ

e. 243. 9 kJ

Unit 8: Electrons

41. Calculate and determine the type of EMR:a. the energy of a photon with a frequency of 8.77x1015 s−1 b. the frequency of a photon with an energy of 1.88x10−25 J.

42. Write the shortened configuration and orbital notation for Cadmium.

43. What is the total number of electrons that will be in p orbitals in 8.31 moles of ground state zinc atoms?

44. In the hydrogen atom, the energy associated with the fifth energy level is −8.72x10−20 J while the energy of the first energy level is −2.18x10−18 J.

a. Calculate the energy change from n=5 to n=1? B. Calculate the wavelength of the emitted photon?

45. Which of the following colors has the highest frequency?a. blue b. red c. violet d. yellow

46. Which of the following has the longest wavelength?

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a. U.V. b. I.R. c. X-ray d. gamma

47. An 18.36 g sample of hydrogen cyanide gas (C = 1.328 J/g•°C) is at STP in a 5.00 L expandable container. When 1.609 x 1021 photons of light with a wavelength of 945Å are added to the gas, the pressure of the gas changes to 1168 torr. What is the new volume of the gas after the addition of the photons?

Unit 9: Bonding

48.Draw the Lewis dot structure for strontium nitride.

49.By use of electronegativity, identify each of the following bonds as: nonpolar, polar covalent, or ionic.CH4 H2O RbI O2

50. How many single bonds are present in 6.93 x 1024 molecules of perchloric acid?

51.Draw the electron geometry, molecular geometry and bond angle for the carbonate ion?

52.Complete the following table using your knowledge of Lewis Structures and VSEPR theory.

Lewis Structure Structural Formula (indicate polarity)

electron geometry

bond angle

molecular geometry

CH2Cl2

H2S

BF3

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NF3

Unit 10: Solutions

53. Consider the three statements below. Which numbered response contains all the statements that are true and no false statements?

I. Hydration is a special case of solvation in which the solvent is water.II. The oxygen end of water molecules is attracted toward Ca2+ ions.III. The hydrogen end of water molecules is attracted toward Cl- ions.

a. I b. II c. III d. I and II e. I, II, and III

54. Which of the following solutions would not be expected to exist?a. NaCl in CCl4 (a nonpolar solvent)b. NaCl in waterc. Pentane, C5H12, in CCl4

d. Methyl alcohol, CH3OH, in watere. Vegetable oil in mineral oil

55. Calculate the molality of a solution that contains 25 g of H2SO4 dissolved in 80. g of H2O.a. 1.6 m b. 2.2 m c. 3.2 m d. 6.3 m e. 7.0 m

56. Calculate the molality of a 10.0% phosphoric acid solution in water.a. 0.380 m b. 0.760 m c. 1.13 m d. 1.51 m e. 1.89 m

57. Which aqueous solution would have the lowest vapor pressure at 25 C?a. 1 M NaClb. 1 M Na3PO4

c. 1M sucrose, C12H10O11

d. 1 M MgCl2

e. 1 M glucose, C6H12O6

58. If 4.27 grams of sucrose, C12H22O11, are dissolved in 15.2 grams of water, what will be the boiling point of the resulting solution?

a. 101.64C b. 100.42C c. 99.626C d. 100.73C e. 101.42C

59. Which of the following statements regarding a 1 M sucrose solution is not correct?a. The boiling point is greater than 100C.b. The freezing point is less than that of a 1 M NaCl solution.c. The freezing point is less than 0.0C.d. The boiling point is less than that of a 1 M NaCl solution.e. The vapor pressure at 100C is less than 760 torr.

60. When 35.0 g of an unknown nonelectrolyte is dissolved in 220.0 g of benzene, the solution boils at 83.2C. Calculate the molecular weight of the unknown nonelectrolyte. The Kb for benzene = 2.53C/m. The boiling point of pure benzene is 80.1C.

a. 130 g/mol b. 20.3 g/mol c. 183 g/mol d. 156 g/mol e. 194 g/mol

61. The following describe properties of substances. Which one is not a property of acids?a. They have a sour taste. b. They react with metal oxides to form salts and water.

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c. They react with other acids to form salts and water.d. Their aqueous solutions conduct an electric current.

e. They react with active metals to liberate H2.

62. Which of the following is not a common property of aqueous solutions of most bases?a. They have a bitter taste.

b. They have a slippery feeling.c. They change the colors of many indicators.d. They react with protonic acids to form salts and stronger bases.e. Their aqueous solutions conduct an electric current.

63. According to the Arrhenius theory, which of the following is an acid?a. NH3 b. CH4 c. HCl d. H2 e. NaOH

64. Which one of the following species could not react as a Brønsted-Lowry acid?a. HClb. H2O

c. CaOd. NH3

e. CH3COOH

65. Which of the following does not represent a conjugate acid-base pair?a. H2O/OH- b. H3O+/OH- c. HCl/Cl- d. HNO3/NO3

- e. NH4+/NH3

66. A solution having a pH of 1.4 would be described as __________.a. distinctly basicb. slightly basic

c. neutrald. slightly acidic

e. distinctly acidic

67. In the equation: HF + H2O H3O+ + F-

a. H2O is a base, and HF is its conjugate acid.b. H2O is an acid, and HF is the conjugate base.c. HF is an acid, and F- is its conjugate base.

d. HF is a base, and H3O+ is its conjugate acid.e. HF is a base, and F- is its conjugate acid.

68. Which of the following reactions is the net ionic equation for the acid-base reaction between H2CO3 and Sr(OH)2?a. H2CO3 + Sr2+ + 2 OH- SrCO3 + 2 H2Ob. H3O+ + OH- 2 H2Oc. 2 H3O+ + Sr2+ + 2 OH- Sr2++ 4 H2O

d. H2CO3 + 2 OH- 2 H2O+ CO32-

e. H2CO3 + Sr(OH)2 2H2O+ Sr2+ + CO32-

69. The molar concentration of the Ca2+ ion is ________ and the molar concentration of OH- ion is ________ in 0.015 M calcium hydroxide.

a. 0.015 M; 0.015 M

b. 0.015 M; 0.030 M

c. 0.030 M; 0.015 M

d. 0.030 M; 0.030 M

e. not enough information to calculate

70. Calculate the pH of a solution in which [OH-] = 2.50 10-4 M.a. 0.40 b. 3.60 c. -3.60 d. 10.40 e. 13.60

71. What is the concentration of H3O+ ions in a solution in which pH = 4.32?a. 4.8 10-5 M b. 6.2 10-4 M c. 5.1 10-4 M d. 8.6 10-5 M e. 3.5 10-4 M

72. What is the pH of 500. mL of solution containing 0.0124 gram of calcium hydroxide?a. 2.96

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b. 3.17 c. 9.68 d. 10.83 e. 11.04

73. A laboratory stock solution is 1.50 M sodium hydroxide. Calculate the volume of this stock solution that would be needed to prepare 300. mL of 0.200 M sodium hydroxide.

a. 2.25 mLb. 10.0 mL

c. 40.0 mLd. 1.00 mL

e. 0.100 mL

74. When a solution is diluted, what is the relationship of the number of moles of solute in the more concentrated initial volume of solution to the number of moles of solute in the less concentrated final volume of solution?

a. The ratio of the numbers is directly proportional to the two volumes.b. The ratio of the numbers is inversely proportional to the two volumes.c. The number of moles of solute in the more concentrated initial volume is always greater.d. The number of moles of solute in the less concentrated final volume is always greater.e. The number of moles of solute in both solutions is the same.

75. Calculate the molarity of the resulting solution if 25.0 mL of 2.40 M sulfuric acid solution is diluted to 300.mL.a. 0.200 Mb. 29.0 M

c. 2.00 Md. 0.400 M

e. 0.0400 M

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