The Haber process is a method to produce ammonia from hydrogen and nitrogen gasses. The reaction is

                     N₂ (g) + 3 H₂ (g) ↔ 2 NH₃ (g)

If hydrogen gas is added after the reaction has reached equilibrium, the reaction will:

A. shift to the right to produce more product

b. shift to the left to produce more reactants
c. stop. All the nitrogen gas has already been used up. d. Need more information.

Chemical Reaction Classification Practice Test

1 The chemical reaction: 2 H₂O → 2 H₂ + O₂ is a

a. synthesis reaction b. decomposition reaction  

c. single displacement reaction

d. double displacement reaction                          e. combustion reaction

2 The chemical reaction: 2 H₂ + O₂ → 2 H₂O is a

a. synthesis reaction  b. decomposition reaction  

c. single displacement reaction

d. double displacement reaction                            e. combustion reaction

3 The chemical reaction: 2 KBr + Cl₂ → 2 KCl + Br₂ is a

a. synthesis reaction b. decomposition reaction   

c. single displacement reaction

d. double displacement reaction            e. combustion reaction

4  The chemical reaction: 2 H₂O₂ → 2 H₂O + O₂ is a

a. synthesis reaction b. decomposition reaction   

c. single displacement reaction

d. double displacement reaction                            e. combustion reaction

5 The chemical reaction: Zn + H₂SO₄ → ZnSO₄ + H₂ is a

a. synthesis reaction b. decomposition reaction

c. single displacement reaction

d. double displacement reaction                        e. combustion reaction

6 The chemical reaction: AgNO₃ + NaCl → AgCl + NaNO₃ is a

a. synthesis reaction   b. decomposition reaction 

c. single displacement reaction

d. double displacement reaction                            e. combustion reaction

7 The chemical reaction: C₁₀H₈ + 12 O₂ → 10 CO₂ + 4 H₂O is a

a. synthesis reaction b. decomposition reaction  

c. single displacement reaction

d. double displacement reaction                  e. combustion reaction

8 The chemical reaction: 8 Fe + S₈ → 8 FeS is a

a. synthesis reaction b. decomposition reaction  

c. single displacement reaction

d. double displacement reaction                   e. combustion reaction

9 The chemical reaction: 2 CO + O₂ → 2 CO₂ is a

a. synthesis reaction b. decomposition reaction  

c. single displacement reaction

d. double displacement reaction                         e. combustion reaction

10 The chemical reaction: Ca(OH)₂ + H₂SO₄ → CaSO₄ + 2 H₂O is a

a. synthesis reaction b. decomposition reaction   

c. single displacement reaction

d. double displacement reaction                           e. combustion reaction

Test questions

1. What is the equivalent weight of MgO

А. 20  В. 30   С. 10  D. 35  Е. 40

2. What is the equivalent weight of H₃PO₄

А. 20  В. 32  С. 10  D. 35  Е. 40

3. What is the equivalent weight of Fe₂O₃

А. 20  В. 32  С. 10  D. 35  Е. 26

4. What is the equivalent weight of HNO₂

А. 20  В. 32  С. 47  D. 35  Е. 40

5. What is the equivalent weight of H₂CrO₄

А. 59  В. 32  С. 10  D. 35  Е. 40

6. What is the equivalent weight of H₂ZnO₂

А. 20  В. 32  С. 10  D. 35  Е. 49

7. What is the equivalent weight of CO 

А. 20  В. 32  С. 14  D. 35  Е. 49

8. What is the equivalent weight of Al₂O₃

А. 20  В. 17  С. 10  D. 35  Е. 49

9. What is the equivalent weight of Fe(OH) ₂

А. 20  В. 32  С. 10  D. 35  Е. 45

10. What is the equivalent weight of Fe(OH) ₃

А. 20  В. 41  С. 10  D. 105  Е. 49

11. The elements of Group VII are known as the:

A. lanthanides    B. noble gases    C. halogens D. neutrons  E. nonmetals

12. ₃₀ ⁶⁴Zn and ₃₀ ⁶⁸Zn  are examples of:

A. isotopes    B. allotropes  C. phenemones D. neutrons   E. nonmetals

13. An atom of strontium-90 (⁹⁰₃₈Sr) contains

А. 38 electrons, 38 protons, 52 neutrons

В. 38 electrons, 38 protons, 90 neutrons

С. 52 electrons, 52 protons, 38 neutrons

D. 52 electrons, 38 protons, 38 neutrons

E. 30 electrons, 30 protons, 38 neutrons

14. Which of the following pairs of species would have the greatest similarities in chemical properties?

А. ³⁹K and ³⁹K⁺          В. ³⁹K and ²³Na        С. ³⁹K and ⁴⁰K     

D. ⁴⁰K and ⁴⁰Ca         E. ⁴⁴K and ⁴⁰Ca

15 The species ¹⁰⁴₄₄Ru contains

А. 44 neutrons and 44 electrons.      В. 44 protons and 44 electrons.

С. 44 protons and 104 neutrons.      D. 60 neutrons and 60 electrons.

E. 80 neutrons and 60 electrons.

16. An atom of strontium-90 (⁹⁰₃₈Sr) contains

А. 38 electrons, 38 protons, 52 neutrons     В. 38 electrons, 38 protons, 90 neutrons

С. 52 electrons, 52 protons, 38 neutrons      D. 52 electrons, 38 protons, 38 neutrons

E.59 electrons, 38 protons, 40 neutrons

17. The nucleus of a radon atom, ²²²₈₆Rn, contains

А. 222 protons and 86 neutrons.          В. 86 protons and 140 neutrons.

С. 86 protons and 222 neutrons.              D. 86 protons, 136 neutrons and 86 electrons.

E. 86 protons, 136 neutrons.

18. The species ¹⁰⁴₄₄Ru contains

А. 44 neutrons and 44 electrons.      В. 44 protons and 44 electrons.

С. 44 protons and 104 neutrons.      D. 60 neutrons and 60 electrons.

E. 86 protons, 136 neutrons

19. What is the order of decreasing radii of species S, S²⁺ and S^2-?

A. S >S^2->S²⁺     B. S^2->S²⁺>S     C. S^2->S>S²⁺     D. S²⁺>S>S^2- E. S>S²⁺>S

20. Which subtance does not have the correct formula?

A. iron(lll) sulfate Fe₂(SO₄)₃ B. iron(ll) oxide Fe₂O    

C. copper(l) sulfate Cu₂SO₄

D. copper(ll) nitrite Cu(NO₃)₂ E. Carbon dioxide CO

21. Тhe smallest particle of an element is ….

A. Atom B. Molecule    C. Ion D. Elements        

E. Substanses

22. The smallest particle of a substance that can have an independent existence.

A.Atom B. Molecule      C. Ion     D. Elements        

    E. Substanses

23. Pure substances, that make up everything in the universe

A. Atom  B. Molecule     C. Ion     D. Elements    

E. Substanses

24 Law of equivalent proportions - law stating that …

A. the proportions in which two elements separately combine with a third element are also the proportions in which they combine together.

B. The mass of the substances entering into a reaction equal the mass of the substances formed as a result of the reaction.

C. On mole of any substance in the gaseous state occupies the same volume at the same temperature and pressure.

D. One mole of any gas in standard conditions (0°C = 273°K, 1 atm = 101.3 kPa) occupies a volume of 22.4 litres.

25. Law of mass conversation - law stating that …

A. the proportions in which two elements separately combine with a third element are also the proportions in which they combine together.

B. The mass of the substances entering into a reaction equal the mass of the substances formed as a result of the reaction.

C. On mole of any substance in the gaseous state occupies the same volume at the same temperature and pressure.

D. One mole of any gas in standard conditions (0°C = 273°K, 1 atm = 101.3 kPa) occupies a volume of 22.4 litres.

26. Equal volumes of all gases at the same conditions (temperature, pressure) contain the same number of molecules.

A. Law of constant composition.   B. Law of multiple proportions   C. Avogadro law

D. Law of combining volumes

28 The elements in the Periodic Table are arranged in order of increasing

A. Ionization energy B. Atomic volume C. Relative atomic mass D. Nuclear charge

Е. Relative molecular mass

29 Which pair of elements has the most similar chemical properties?

A. As and Br     B. As and Se        C. As and P    D. C and F    

E. Cu and P

30 Which subtance does not have the correct formula?

A. iron(lll) sulfate Fe₂(SO₄)₃   B. iron(ll) oxide Fe₂O₃

C. copper(l) sulfate Cu₂SO₄ D. copper(ll) nitrite Cu₃(NO₃)₂

E. copper(ll) nitrite CuSO₄

31 Which is not a property of metallic solids?

A. conduct electricity      B. usually high melting       

C. high freezing point

D. They are all properties of metallic solids

32. Oxygen gas can be produced by the decomposition of all of the following substances expect:

A. mercury(II) oxide B. hydrogen peroxide C. Ozone    

D. copper E. iron

33. Which one of the following combinations of names and formulas is incorrect?

A. H₃PO₄ phosphoric acid   B. HNO₃ nitric acid  

C. NaHCO₃ sodium carbonate

D. AlPO₄  aluminium fluoride E. CaCl₂ calcium oxide

34. The name for the ion, S ^{2 –} is:

A. sulfide   B. sulfate    C. Sulfite D. Sulfur E. Carbon

35. Calculate the HO⁺ ion concentration (in M) in a solution with  a pH = 7

A. 1·10^–7 M  B. 2.0·10^–7 M   C. 8.0·10^–7 M D. 5.0·10^–7 M E. 6.0·10^–7 M

36. Calculate the pH of a solution whose [H⁺ ] = 10^-12.

A. 2 B. 10  C. 12     D. 8  E. 6

37. Calculate the pH of a solution whose [H⁺ ] = 10^-5.

A. 2      B. 10         C. 5     D. 8     E. 6

38. A pH buffer is best described as a solution containing:

A. A weak acid                   B. A strong acid

C. A mixture of a weak acid and the salt of a weak acid

D. A strong acid            E. A strong base

39. When NaCl dissolves in water, it is present as:

A. NaCl molecules  B. Na atoms and Cl atoms   C. Na cations and Cl anions

D. Na                        E. Cl₂

40. Insoluble salt is an example of...

A. weak electrolyte     B. strong electrolyte C. Cathode D. Anode E. They are all right

41. Soluble salt is an example of...

A. weak electrolyte   B. strong electrolyte C. Anode D. Cathode E. They are all right

42. pH equation

A. -log[Ka]  B. -log[OH^-] C. -log[H⁺]      D. -log[C₁/C₂]   E. -log[K_b]

43. pOH equation

A. -log[Ka]  B. -log[OH^-]  C. -log[H⁺]     D. -log[C₁/C₂]  E. -log[K_b]

44. Which is a characteristic of a strong acid?

A. It has a pH greater than 7.                B. It completely ionizes in solution.

C. It contains many hydroxide ions.       D. It reacts only with a strong base.

E. It has a pH less than 7.

45. Calculate the ionic strengths of the solution 0.30 M NaCl.

A. 0.30  B. 0.90   C. 0.80   D. 3.3         E. 6.5

46. Calculate the ionic strengths of the solution 0.30 M Na₂SO₄.

A. 0.50        B. 0.90              C. 0.20        D. 3.5 E. 6.5

47. Calculate the ionic strengths of the solution 0.30 M NaCl and 0.20 M K₂SO₄.

A. 0.50    B. 0.90    C. 0.20        D. 3.5        E. 6.50

49 Calculate the ionic strengths of the solution 0.20 M Al₂(SO₄)₃ and 0.010 M Na₂SO₄.

A. 0.50    B. 0.90        C. 0.20    D. 3.30   E. 6.80

48. Calculate the ionic strengths of the solution 0.5 M AlCl₃ and 0.010 M Na₂SO₄.

A. 0.50     B. 0.90         C. 0.20         D. 3.30      E. 5.50

50.  Qualitative analysis

А. what chemicals are present         В. how much of a chemical is present

С. occurs only with the substance of interest (rare) D. atomic structure

E. matter and energy

51. quantitative analysis

А. what chemicals are present           В. how much of a chemical is present

С. occurs only with the substance of interest (rare) D. atomic structure

E. matter and energy

52. gross sample

A. consists of several portions of the material to be tested 

B. small portion of the gross sample

C. small portion of the laboratory sample that is analyzed       

53. analysis sample

A. consists of several portions of the material to be tested

B. small portion of the gross sample

C. small portion of the laboratory sample that is analyzed

54. Selective separation of the analyte by precipitation followed by measurement of a physical property

A. gravimetric analysis B. volumetric/titrimetric analysis     

C. instrumental analysis

D. spectral analysis      E. spectrometers methods

55. Analyte reacts with a measured volume of reagent of known concentration. a change in some property signals the completion of the reaction

A. gravimetric analysis   B. volumetric/titrimetric analysis  

C. instrumental analysis

D. spectral analysis         E. spectrometers methods

56. More slective. may be less precise. based on the measurement of a physical property of a sample.

A. gravimetric analysis B. volumetric/titrimetric analysis    

C. instrumental analysis

D. spectral analysis     E. Chromatography

57. Is the process by which ions are retained on the surface of a solid

A. Adsorption  B. Digestion  C. Agglomeration  D. Dissolution   

E. Corrosion

58. mixtures from which particles settle out upon standing

A. Suspensions B.Colloids C. Emulsions D. Complexes   E. Solutions

59. geterogeneous mixtures containing particles that are intermediate in size

A. Suspensions B. Colloids C. Emulsions D. Complexes   E. Solutions

60 Colloidal dispersion of liquids in liquids

A. Suspensions B. Colloids C. Emulsions D. Complexes  E. Solutions

61 Solid particles dispersed in a gas (solid aerosol), example:

A. dust in air    B. slime, paste C. whipped cream D. whipped cream 

E. Shaving cream

62 Solid particles dispersed in a liquid (sol); example:

A. cloud B. slime, paste C. foam rubber  D. mayonnaise        

E. hand cream

63. Liquid dispersed in a solid (gel); example:

A. some glasses  B. jelly      C. whipped cream   D. milk         

E. hand cream

64. What is the equilibrium constant for the general equation aA bB «cC dD?

A.  B.  C. D.

 

65. The rate of for the general equation aA bB cC dD?

A. V=k[A]^a[B]^b B. V=k[C]^a[D]^b C. V=k[A][B] D.V=k[A]^c[B]^d

E. V=k[C]^c[D]^d

66. Consider the following mechanism for a reaction:

Step 1: HBr + O₂ ® HOOBr

Step 2: HBr + HOOBr ® 2HOBr

Step 3: 2HOBr + 2HBr ® 2Br₂ + 2H₂O  

67. Which of the following statements is correct?

A. Br₂ is a reactant.          B. HBr is a catalyst.  C. HOBr is a catalyst.

D. HOOBr is a reaction intermediate. E. H₂O is a catalyst.

68. Consider the following reaction mechanism:

Step 1: ClO^- +H₂O ® HClO + OH^-    Step 2: I^- + HClO ® HIO + Cl^-

Step 3: HIO + OH^- ® IO^- + H₂O

The catalyst is

A. IO^-       B. H₂O     C. ClO^-     D. HClO  E. OH^-

69. Adding or taking away one species in an equilibrium causes the relative rates of reaction to shift to compensate for the change

A. Nernst Equation B. Le Chatelier's Principle      

C. Bronsted-Lowry Theory

D. Mendeleev’s law      E. Beer-Lambert law

70. Which of the following can be used to represent the rate of a reaction?

A.g / L         B. g / mol C. (g · min) / mol D. M / min

71. What is the coordination number of cobalt in the complex ion [Co(en)Cl₄]^-? (en = ethylenediamine)

A. 1       B. 2           C. 3             D. 5           E. 8

72. In the compound K[Co(C₂O₄)₂(H₂O)₂] (where C₂O₄^2- = oxalate) the oxidation number and coordination number of cobalt are, respectively:

A. -1 and 4   B. -1 and 6      C. 3 and 4     D. 1 and 5     E. 2 and 3

73. Choose the correct name for the formula, [Cr(NH₃)₄(OH)₂]Br

A) chromium(II) tetraamminebis(hydroxo) bromide

B) chromium(III) tetraamminebis(hydroxo) bromide

C) tetraamminedihydroxochromium(III) bromide

74. Choose the correct name for the formula, [Co(en)₃][Cr(ox)₃]. en = ethylenediamine and ox = C₂O₄^2-, oxalate

A. tris(ethylenediamine)cobalt(III) tris(oxalato)chromium(III)

B. tris(ethylenediamine)cobaltate(III) tris(oxalato)chromate(III)

C. tris(ethylenediamine)cobalt(III) tris(oxalato)chromate(II)

D. tris(ethylenediamine)cobalt(III) chromate(II) E. cobalt(III) tris(oxalato)chromate(II)

75. What is the coordinate number for the central atom in [Co(en)(NH₃)₃Cl]SO₄?

A. 2 B. 3 C. 5 D. 7   E. 10

76. In which one of the following pairs is the oxidation number of chromium the same?

A. Cr₂O₃ and CrCl₂           B. CrO₃ and CrCl₃   C. CrO₄^2- and Cr₂O₇^2-

D. Cr²⁺ and CrO₂^-           E. Cr⁺² and Cr₂O₇^2-

77.  A reducing agent in the cell

A. Electron Donor    B. Electron Acceptor C. Cation D.Anion E. Electrolyte

78. An oxidizing agent in the cell

A. Electron Donor    B. Electron Acceptor C. Cation D.Anion E. Electrolyte

79. What is the oxidation number of copper in Cu⁺²?

A. 0     B. +2     C. -3    D. +3        E. -2

80. What is the oxidation number of Br in the BrO₃^- ion?

A. +2 B. -2     C. +5   D. -5    E. -1

81. What kind of reaction is Cl₂ «Cl^- + ClO₂ (aside from unbalanced)?

A. An oxidation B. A reduction C. A disproportionation  D. Redox E. Dissolution

82. In the reaction HNO₂ + I^- «NO + I₃^-, what atoms are being  oxidized and reduced, respectively?

A. O, I B. I, N     C. N, I        D. I, O   E. H, I

83. Which one of the following reactions is not a redox reaction?

А. Ag⁺(aq) + Cl^-(aq) ® AgCl(s)                  В. 2Na(s) + Cl₂(g) ® 2NaCl(s)

С. Mg(s) + 2HCl(aq) ® MgCl₂(aq) + H₂(g)     

 D. Cu²⁺(aq) + Zn(s) ® Cu(s) + Zn²⁺(aq)

E. 2Zn (s) + O₂ (g) ® 2ZnO (s)

84. The oxidation numbers of nitrogen in NH₃, HNO₃, and NO₂ are, respectively

A. -3, -5, +4 B. +3, +5, +4 C. -3, +5, -4  D. -3, +5, +4       

 E. +3, +4, -5

85. What is the oxidation number for Cl in the chlorate ion, ClO₃^-?

A. -1              B. +3             C. +5             D.+7               E. -5

86. What is the oxidation number of Cl in KClO₃?

A. -1            B. +2        C. +5         D. -5   E. +7

87. Which equations represent oxidaton-reduction reactions?

I. CaO(s) + CO₂(g) ® CaCO₃(s)

II. Zn(s) + H₂SO₄(aq) ® H₂(g) + ZnSO₄(aq)

A.I only  II only      B. Both I and II   C. Neither I nor II

88.  What is the next step in balancing the half reaction

Cr₂O₇^-2 «2 Cr⁺³?

A. Add 7 H₂O to the right B.Add 7 H₂O to the left C. Add 3.5 O₂ to the left

D. Add 7 O₂ to the left    E. Add 3.5 O₂ to the right

89.  What is the next step in balancing the reaction

SO₃^-2+H₂O«SO₄^-2+2H⁺?

A. Add 3 H₂O to the left B. Add 2 electrons to the left C. Nothing - it is balanced           

D. Add 3 H₂O to the right  E. Add 3 O₂ to the right

90.  What is the next step in balancing the REDOX reaction having the two half reactions:

Cr(OH)₄^- → CrO₄^-2 +4 H⁺ + 3 e^- and ClO^- + 2 H⁺ + 2 e^- → Cl^- + H₂O?

A. Add the two half reactions  B. Multiply both by 3  

C. Multiply the oxidation by 2 and the reduction by 3

D. Multiply the oxidation by 2 and the reduction by 3          

E. Multiply both by 2    

91.  What is wrong with the REDOX reaction 

Cl₂ + 2 Br ^- → 2Cl^- + Br₂?

A. Nothing is being reduced           B. Chloride can not be oxidized    

C. Bromide can not be oxidized   D. Chloride can not be reduced    

E. Bromide can not be reduced

92.  When the balanced reaction

2 MnO₄^- + SO₃^-2 + H₂O → 2 MnO₄^-2 + SO₄^-2 + 2 H⁺ is changed to be balanced in basic solution, the result is:  

A. 2 MnO₄^- + SO₃^-2 ® 2MnO₄^-2 + SO₄^-2 + H₂O   

B. 2 MnO₄^- + SO₃^-2 + 2OH^- ® 2MnO₄^-2 + SO₄^-2 + H₂O    

C. 2 MnO₄^- + SO₃^-2 ® 2MnO₄^-2 + SO₄^-2 + H₂O + 2 OH^-  

D. 3MnO₄^- + SO₃^-2 ® 3MnO₄^-2 + SO₄^-2 + H₂O + 3OH^-  

E. 2MnO₄^- + SO₃^-2 ® 4MnO₄^-2 + SO₄^-2 + H₂O

93.  What are the oxidation numbers of the V, O and Cl atoms in VOCl₃?

A. -5, -2, -1 B. -5, +2, -1  C. +5, -2, -1  D. -5, -1, +1  E. -2, +5, +1

94. The molar mass of MgSO₄

A.120.00 g/mol B.193.03 g/mol C.165.02 g/mol D. 170.85 g/mol E. 130.85 g/mol

95. Calculate the molar mass of (NH₄)₃AsO₄

A. 417.80 g/mol B. 193.03 g/mol   C. 165.02 g/mol D. 250.02 g/mol

E. 365.52 g/mol

96. Calculate the molar mass of (NH₄)₂Ca

A. 76.00 g/mol B. 193.03 g/mol C. 165.02 g/mol D. 250.02 g/mol  

E. 365.52 g/mol

97. Calculate the molar mass of K₃PO₄

A. 417.80 g/mol B. 212.00 g/mol C. 165.02 g/mol D. 250.02 g/mol 

E. 365.52 g/mol

98. Calculate the molar mass of Ag₃AsO₄

A. 417.80 g/mol B. 463.03 g/mol C. 545.02 g/mol D. 250.02 g/mol 

E. 365.52 g/mol

99. The empirical formula of a compound is CH₂. If the molecular weight of the compound is 56, how many carbon atoms does a molecule contain?

A. 4 B. 1  C. 3   D. 5      E. 6

 

100. One mole of KClO₃ decomposes to yield:

A. 1 mole of oxygen atoms B. 1.5 moles of O₂   C. 2 moles of KCl

D. 2 moles of O₂                         E. 1 moles of KCl

101. A given liquid occupies 445 mL and weighs 540 g. The density of this liquid is (units missing):

A. 0.73 B. 0.85   C. 0.82         D. 0.65    E. 0.96

102. To what volume must you dilute 200 mL of a 6.00 M solution of NaCl to obtain a 0.3 M solution of NaCl?

A. 1.0 L    B. 2.0 L      C. 4.0 L           D. 5.0 L    E. 6.0 L

103.  A compound is subjected to chemical analysis and you receive the following report from the analysis laboratory. Determine the simplest formula for the compound

% P = 31.6%   O = 65.4% H=3.06.

A. PH₃O₄   B. P₂H₆O₈      C. P₂H O₂          D. P₃H₆O₈          E. P₂ H₃O₈

104. How much iron can be made from 495 g of aluminum by the following process:

                            Fe₂ O₃ + 2 Al «Al₂ O₃ + 3 Fe

A. 495 g    B. 1644 g     C. 149 g      D. 153 g      E. 253 g

105. How many grams of water will be formed when a mixture containing 1.93 g C₂ H₄ and 5.92 g O₂ is ignited in a closed vessel?

A. 2.22 g    B. 5.89 g        C. 10.21 g        D. 15.3 g       

E. 25.3 g

106.  This balanced equation represents a chemical reaction: 2KClO₃ (s) ® 2KCl(s) + 3O₂ (g) How many moles of KCl are produced when 4.25 moles of KClO₃ decompose?

A. 1.06 moles   B. 2.57 moles  C. 4.25 moles  D. 8.50 moles E. 8.95 moles

107. Considering this balanced chemical equation, how many grams of HgO will be produced when 44 g of Hg react with excess O₂? 2Hg (l) + O₂ (g) → 2HgO (s)

A. 28 g B. 44 g     C. 47 g     D. 96 g         E. 55 g

108. What is the molarity of 28.9 g of CaCl₂ dissolved in water to make 0.78 L of solution?

A. 0.33 M B. 0.69 M    C. 1.5 M    D. 3.0 M    E. 0.82 M

109. What is the molarity of 60 g of MgCl₂ dissolved in water to make 2 L of solution?

A. 0.31 M   B. 0.69 M C. 1.5 M     D. 3.0 M    E. 0.56 M

110. What is the molarity of a solution containing 9.478 grams of RuCl₃ in enough water to make 1.00 L of solution?

А. 0.045 M В. 0.25 М С. 0.036 М    D. 0.56 М  E. 0.085 М
     111. What is the molarity of a solution containing 5.035 grams of FeCl₃ in enough water to make 500 mL of solution?

А. 0.036 М  В. 0.062 M     С. 0.085 М      D. 0.027 М   E. 0.046 М

112. What is the molarity of a solution containing 72.9 grams of HCl in enough water to make 500 mL of solution?

А. 5.0 М В. 6.0 М   С. 4.0 M  D. 3.0 M      E. 2.0 M

113. What is the molarity of a solution containing 11.522 grams of KOH in enough water to make 350 mL of solution?

А. 0.362 М  В. 0.586 M С. 0.256 М D. 0.158 М  E. 0.615 М

114. What is the molarity of a solution containing 72.06 grams of BaCl₂ in enough water to make 800 mL of solution?

А. 0.433 M В. 0.255 М  С. 0,852 М    D. 0,358 М     e. 0,758 М

115. How many grams of NaCl are required to prepare 100 mL of a solution of 1 M NaCl?

A. 5.844 grams of NaCl    B. 6.024 grams of NaCl   C. 5.044 grams of NaCl

D. 2.585 grams of NaCl     E. 3.086 grams of NaCl

116. How many grams of KMnO₄ are required to prepare 1.0 L of a solution of 1.5 M KMnO₄?

A. 237 grams of KMnO₄   B. 452 grams of KMnO₄   C. 156 grams of KMnO₄

D. 325 grams of KMnO₄  E. 758 grams of KMnO₄

117. How many grams of HNO₃ are required to prepare 500 mL of a 0.601 M HNO₃ solution?

A. 12.92 grams of HNO₃ B. 15.92 grams of HNO₃           C. 18.92 grams of HNO₃

D. 25.34 grams of HNO₃    E. 16.58 grams of HNO₃
118. What is the volume of a 0.1 M HCl solution containing 1.46 grams of HCl?

A. 0.200 L or 200 mL B. 0.400 L or 400 mL  C. 0.600 L or 600 mL

D. 0.500 L or 500 mL   E. 0.300 L or 300 mL
119. What is the volume of a 0.2 M AgNO₃ solution containing 8.5 grams of AgNO₃?

A. 0.15 L or 150 mL B. 0.35 L or 350 mL C. 0.25 L or 250 mL

D. 0.45 L or 150 mL E. 0.55 L or 350 mL

120. The correct relationship for the solubility of a gas in a liquid is:

A. solubility increases with increasing pressure and increasing temperature.

B. solubility increases with increasing pressure and decreasing temperature.

C. solubility increases with decreasing pressure and increasing temperature

D. solubility increases with decreasing pressure and decreasing temperature

B. solubility increases with decreasing volume and decreasing temperature

121. Bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other.

A. Covalent bond  B. Ionic bond   C. Metallic Bond D. Hydrogen Bond

E. Oxygen Bond

122. Bond in which one or more pairs of electrons are shared by two atoms.

A. Covalent bond B. Ionic bond C. Metallic Bond D. Hydrogen Bond

E. Oxygen Bond

123. When electrons are shared by two metallic atoms may be formed…

A. Covalent bond B. Ionic bond C. Metallic Bond D. Hydrogen Bond

E. Oxygen Bond

124. can exchange both matter and energy with an outside system

A. Open systems    B.Closed systems    

C. Isolated systems  D. Standard system

E. Dynamic system

125. exchange energy but not matter with an outside system.

A. Open systems      B. Closed systems      C. Isolated systems  

D. Standard system

E. Dynamic system

126. can exchange neither energy nor matter with an outside system

A. Open systems     B. Closed systems     C. Isolated systems    

D. Standard system

E. Dynamic system

127. Thermodynamic Extensive Properties

A. volume        B. Pressure    C. Temperature  D. Density  E. Energy

128. It is not a thermodynamic Extensive Properties

A. volume    B. Pressure C. Temperature D. Density E. energy

129. Energy and matter can be neither created nor destroyed; only transformed from one form to another. 

A. The first law of thermodynamics. B. The second law of thermodynamics.

C. Hess’s Law                 D. Mendellev’s law     E. Vant Goff’s law

130. If DG<0 (is negative)

A. the reaction is spontaneous           B. the reaction is nonspontaneous

C. the reaction is at equilibrium          D. Oxidation           E. Reduction

131. If DG> 0 (is positive)

A. the reaction is spontaneous                 B. the reaction is nonspontaneous

C. the reaction is at equilibrium D. Oxidation          E. Reduction

132. If DG =0

A. the reaction is spontaneous           B. the reaction is nonspontaneous

C. the reaction is at equilibrium    D. Oxidation                   E. Reduction

133. Which number gives the number of energy levels in a Bohr-Rutherford diagram of an atom?

A. Atomic mass number      B.Atomic number C. Group number  

D. Period number                Е. None of the obove

134. What is the number of electrons in 17³⁵ Cl^-1?

A. 16      B. 17    C. 18        D. 34         E. 35

135. What are the forces between ionic molecules called?

A. Electrostatic B.Covalent C. Dipole-dipole     D.Polar covalent 

E. Ionic bond

136. Which atom has the largest electron affinity?

A.In      B.Sb    D. Rb         E. Al

137. Which of the following elements has the smallest radius?

A. Rb   B. Ba        C. F     D. Zn     E. Li

138. Elements in the same family tend to be similar in which way?

A. Electron arrangements    B. Numbers of electrons    C. Atomic mass

D. Similar isotopes            E. Both a and c are correct

139. Which of the following is a non-metal?

A. Ti         B. Cu         C. Sr        D. Cl      E. Fe

140. The elements in the periodic table are arranged according to?

A. Atomic mass B. Number of neutrons C.Reactivity D. Atomic number

E. Number of electrons

141. Which of the following elements is most reactive?

A. Mg   B. Cl   C. Br     D. Kr     E. S

142. Which of the following compounds has the most polar bond?

A. K₂O    B. SO₂        C. CaO    D. Li₂O    E. H₂O

143. What is the correct formula of the ionic compound formed when calcium and nitrogen bond?

A. CaN    B. Ca₂N₃         C. Ca₃P         D. CaP₃          E. CaN₂

144. What type of bond forms when there is only fluorine present?

A. Ionic B.Non-polar covalent   C. Polar Covalent D. Covalent E. Metallic

145. What type of bond forms when barium and bromine react?

A. Ionic B. Non-polar covalent  C. Polar Covalent D.Covalent  E. Metallic

146. The correct Lewis Diagram for ammonia, NH₃ will have _____ non bonding electrons on the central atom?

A. 0       B. 2        C. 4         D. 6             E. None of these

147. Which of the following compound has a cation (positive ion) and anion (negative ion) that is isoelectronic?

A. LiBr   B. H₂O₂      CaO       CaCl₂      BeO

148 Elevation of boiling point of the solutions

A. P^o_A - P_A/P^o_A = X_B        B. ΔT_b = k_bm   C. π = nRT/V; π = CRT

D. pH=-log[H⁺]                 E. v=k[A]^a[B]^b

149. Calculate the mass percent of oxygen in C₄H₁₀O.

A. 18.57%    B. 20.3%    C. 50.3%      D. 9.2%    E. 15.2%

150. What is the mass percent of potassium in K₃Fe(CN)₆?

A. 66.62%   B. 35.62%    C. 26.25%  D. 85.62%   E. 29.25%