FINAL EXAM 2013 Mrs. McNamara Accelerated Chemistry SCANTRON

Name___________________________________ No-Calculators Allowed [1 pts. each]

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) A reaction which forms a gaseous product is an example of a(n)________. 1)A) gas evolution reaction B) combustion reactionC) precipitation reaction D) oxidation-reduction reaction

2) A reaction in which a substance reacts with oxygen, emitting heat and formingoxygen-containing compounds is an example of a(n)

2)

A) precipitation reaction. B) combustion reaction.C) acid-base reaction. D) gas evolution reaction.

3) Which of the following is NOT a sign of a chemical reaction? 3)A) absorbing light when chemicals are contacted with each otherB) emission of light when chemicals are contacted with each otherC) absorbing heat when chemicals are contacted with each otherD) All of the above are signs of a chemical reaction.

4) Which of the following statements about balancing reactions is FALSE? 4)A) If there is no coefficient or subscript, a one is implied.B) Subscripts are multiplied by the coefficients to determine the number of atoms in a

compound.C) Coefficients are added to compounds to ensure both sides of the reaction have equal

numbers of each atom.D) When coefficients are added the type of compounds is changed in the chemical reaction.

5) When the equation, ___O2 + ___C5H12 ___CO2 + ___H2O is balanced, the coefficient: of O2 is:

5)

A) 3 B) 5 C) 4 D) 8

6) What are the coefficients for the following reaction when it is properly balanced?

___O2 + ___CH4 ___CO2 + ___H2O

6)

A) 2, 1, 3, 1 B) 2, 1, 1, 2 C) 1, 3, 2, 1 D) 2, 3, 2, 2

7) What are the coefficients for the following reaction when it is properly balanced?

___Na3PO4 + ___Ba(NO3)2 ___NaNO3 + ___Ba3(PO4)2

7)

A) 2, 1, 1, 3 B) 2, 3, 6, 1 C) 2, 3, 1, 6 D) 6, 1, 3, 2

1

8) What are the coefficients for the following reaction when it is properly balanced?

___potassium iodide + ___lead (II) acetate ___lead (II) iodide +___potassium acetate

8)

A) 3, 2, 2, 1 B) 2, 1, 1, 1 C) 2, 1, 1, 2 D) 1, 1, 2, 2

9) When the equation __Ca3N2 + __H2O __Ca(OH)2 + __NH3 is balanced, the coefficient ofH2O is:

9)

A) 3 B) 6 C) 2 D) 12

10) Which of the following equations is NOT balanced properly? 10)A) 4NH3 + 14O2 4NO2 + 6H2O B) 2Cr + 6HCl 2CrCl3 + 3H2C) 2NaHCO3 Na2CO3 + CO2 + H2O D) none of the above

11) An aqueous solution is: 11)A) an ionic compound with water dissolved in it.B) water with a molecular compound dissolved in it.C) water with another compound dissolved in it.D) any liquid with another compound dissolved in it.

12) Which of the following compounds is INSOLUBLE? 12)A) magnesium iodide B) magnesium nitrateC) magnesium sulfate D) magnesium phosphate

13) Which of the following compounds is SOLUBLE? 13)A) aluminum sulfate B) aluminum carbonateC) aluminum sulfide D) aluminum hydroxide

14) The compound sodium sulfate is soluble in water. When this compound dissolves in water,which ion listed below would be present in solution?

14)

A) Na22+ B) S2- C) O2- D) SO42-

15) If you had an aqueous mixture that contained Ag+, K+, and Pb+2 cations, how many differentsolids could precipitate if a chloride solution was added?

15)

A) 4 B) 2 C) 1 D) 3

16) What type of a reaction occurs when a potassium nitrate solution is mixed with a bariumacetate solution?

16)

A) gas evolution B) acid-base neutralizationC) precipitation D) no reaction

17) What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq)are mixed?

17)

A) H2O B) PbSO4C) PbK2 D) none of the above

2

18) Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

Which ion would NOT be present in the complete ionic equation?

18)

A) K+ B) I- C) Pb2+ D) NO32-

19) Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

Which ion(s) would NOT be spectator ions?

19)

A) NO3-, Pb2+ B) Pb2+, I - C) K+, I- D) Pb2+, NO3-

20) Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

What is the correct net ionic equation?

20)

A) Pb2+ + 2I- PbI2(s)B) Pb2+ + I2- PbI2(s)C) 2NO3- + 2K+ 2KNO3

D) Pb2+ + 2NO3- + 2K+ + 2I- PbI2(s) + 2K+ + 2NO3-

21) Which is a spectator ion from the following complete ionic equation:Ag+(aq) + NO3-(aq) + K+ (aq) + Br-(aq) AgBr(s) + K+(aq) + NO3- (aq)

21)

A) AgBr B) K+ C) Ag+ D) Br-

22) What type of a reaction occurs when a silver nitrate solution is mixed with sodium chloridesolution?

22)

A) oxidation-reduction B) gas evolutionC) acid-base neutralization D) precipitation

23) What is the net ionic equation for the reaction of hydrochloric acid with potassium hydroxide? 23)A) HCl + KOH H2O + KClB) H+ + OH- H2OC) 2H+ +2Cl- + K2+ + 2OH- H2O + K2+ +2 Cl-

D) H+ + Cl- + K+ + OH- H2O + K+ + Cl-

24) What is the complete ionic equation for the reaction of hydrochloric acid with potassiumhydroxide?

24)

A) H+ + Cl- + K+ + OH- H2O + K+ + Cl-

B) 2H+ +2Cl- + K2+ + 2OH- H2O + K2+ +2 Cl-

C) H+ + Cl- + K+ + OH- 2H+ + O2- + K+ + Cl-

D) H+ + OH- H2O

3

25) Which of the following types of compounds will NOT undergo a gas evolution reaction whenacid is added?

25)

A) hydroxides B) sulfides C) bisulfites D) carbonates

26) What type of a reaction occurs when a hydrochloric acid solution is mixed with a sodiumbicarbonate solution?

26)

A) gas evolution B) acid-base neutralizationC) precipitation D) oxidation-reduction

27) What type of a reaction occurs when potassium metal reacts with fluorine gas? 27)A) acid-base neutralization B) gas evolutionC) oxidation-reduction D) precipitation

28) Methane gas (CH4), on complete combustion in air, produces:1. CO2 2. H2 3. H2O

28)

A) 1 and 2 only B) 2 and 3 onlyC) 1 and 3 only D) All of 1 and 2 only

29) Which of the following statements about redox reactions is FALSE? 29)A) Oxidation is the loss of electrons.B) A reaction can result in either oxidation or reduction, not both.C) Reduction is the gain of electrons.D) A reaction involving elemental oxygen is a redox reaction.

30) What type of reaction is the generic equation A + B AB? 30)A) decomposition B) double-displacementC) single displacement D) synthesis/combination

31) What type of reaction is the generic equation AB + CD AD + CB? 31)A) single displacement B) decompositionC) synthesis/combination D) double-displacement

32) What must be supplied for most decomposition reactions to happen? 32)A) electrical current B) heatC) energy D) any of the above

33) Which statement about ozone is TRUE? 33)A) Chlorofluorocarbons deplete the ozone layer.B) Ozone normally forms in the upper atmosphere.C) Ozone protects life on Earth from harmful ultraviolet light.D) All the of the first three statements are true.

34) Which of the below statements about global warming is FALSE? 34)A) Greenhouse gases allow sunlight to reach and heat the earth.B) Some greenhouses gases are needed to keep the proper temperature balance.C) Greenhouse gases prevent heat from leaving the earth.D) If the level of greenhouse gases increases, the temperature will decrease.

4

35) Which of the following is TRUE? 35)A) Stoichiometry allows prediction of the amounts of products that form in a chemical

reaction based on the amounts of reactants.B) Stoichiometry shows the numerical relationship between chemical quantities in a

balanced chemical equation.C) Stoichiometry allows prediction of how much of the reactants are necessary to form a

given amount of product.D) All of the above are true.

36) How many moles of water are made from complete reaction of 2.2 moles of oxygen gas withhydrogen gas?Given the reaction: 2H2 + O2 2H2O

36)

A) 4.4 B) 1.1 C) 3.3 D) 2.2

37) How many moles of water are made from complete reaction of 1.4 moles of hydrogen gas?Given the reaction: 2H2 + O2 2H2O

37)

A) 1.4 B) 0.7 C) 2.1 D) 2.8

38) How many moles of aluminum are needed to make 9 moles of molecular hydrogen?Given the reaction: 2 Al + 6 HCl 2 AlCl3 + 3H2

38)

A) 6 moles B) 3 moles C) 2 moles D) 4 moles

39) How many moles of sodium metal are needed to make 3.6 moles of sodium chloride?Given the reaction: 2Na + Cl2 2NaCl

39)

A) 0.9 B) 3.6 C) 7.2 D) 1.8

40) Given the balanced equation CH4 + 2 O2 CO2 + 2 H2O, which of the following is NOT acorrect conversion factor?

40)

A) 2 mole H2O = 18.02 g B) 1 mole CH4 2 mole H2OC) 2 mole O2 1 mole CO2 D) 1 mole O2 = 32.00 g

41) How many grams of water are made from the reaction of 16.0 grams of oxygen gas?Given the reaction: 2H2 + O2 2H2O

41)

A) 16 B) 18 C) 9 D) 36

42) How many grams of sodium metal are needed to make 29.3 grams of sodium chloride?Given the reaction: 2Na + Cl2 2NaCl

42)

A) 11.5 B) 46.0 C) 5.75 D) 23.0

43) Given that 4 NH3 + 5 O2 4 NO + 6 H2O, if 3.00 mol NH3 were made to react with excess ofoxygen gas, the amount of H2O formed would be

43)

A) 2.00 mol. B) 3.00 mol. C) 6.00 mol. D) 4.50 mol.

44) A chemist wishes to perform the following reaction: N2 + 3 H2 2 NH3If only 14.0 g of N2 is available, what is the minimum amount, in grams, of H2 needed tocompletely react with this quantity of N2?

44)

A) 6.06 g B) 1.51 g C) 3.03 g D) 1.01 g

5

45) Which of the following statements is FALSE? 45)

A) The percent yield =Actual Yield

Theoretical Yield × 100%

B) The limiting reactant is completely consumed in a chemical reaction.C) The theoretical yield is the amount of product that can be made based on the amount of

limiting reagent.D) All of the above are true statements.

46) Consider the following generic chemical equation: 2A + 5B C + 3DIf you react 4 units of A with 10 units of B, which statement is TRUE?

46)

A) Substance A will be the limiting reactant.B) There is just enough of A and B so that everything reacts completely.C) Substance C cannot be formed from this reaction.D) Substance B will be the limiting reactant.

47) Determine the theoretical yield of C when 3 units of A and 10 units of B are reacted in thefollowing generic chemical equation: 2A + 5B 4C.

47)

A) 8 B) 4 C) 3 D) 6

48) If the theoretical yield of a reaction is 42.0 grams of product and the percent yield is 75%. Howmany grams were actually produced?

48)

A) 5400 B) 32 C) 56 D) 1.8

49) The theoretical yield of a reaction is 75.0 grams of product and the actual yield is 42.0g. Whatis the percent yield?

49)

A) 31.5 B) 56.0 C) 178 D) 75.0

50) What is the theoretical yield of a reaction if 25.0 grams of product were actually producedfrom a reaction that has a 88% yield?

50)

A) 352 B) 28.4 C) 3.52 D) 22.0

51) What is the limiting reactant for the following reaction given we have 3.4 moles of Ca(NO3)2and 2.4 moles of Li3PO4?Reaction: 3Ca(NO3)2 + 2Li3PO4 6LiNO3 + Ca3(PO4)2

51)

A) Ca3(PO4)2 B) LiNO3 C) Li3PO4 D) Ca(NO3)2

52) What is the excess reactant for the following reaction given we have 3.4 moles of Ca(NO3)2and 2.4 moles of Li3PO4?Reaction: 3Ca(NO3)2 + 2Li3PO4 6LiNO3 + Ca3(PO4)2

52)

A) Li3PO4 B) Ca3(PO4)2 C) LiNO3 D) Ca(NO3)2

53) How many moles of lithium nitrate are theoretically produced if we start with 3.4 moles ofCa(NO3)2 and 2.4 moles of Li3PO4?Reaction: 3Ca(NO3)2 + 2Li3PO4 6LiNO3 + Ca3(PO4)2

53)

A) 6.8 B) 1.1 C) 7.2 D) 1.2

6

54) How many grams of calcium phosphate are theoretically produced if we start with 3.40 molesof Ca(NO3)2 and 2.40 moles of Li3PO4?Reaction: 3Ca(NO3)2 + 2Li3PO4 6LiNO3 + Ca3(PO4)2

54)

A) 310 B) 248 C) 351 D) 1054

55) What is the limiting reactant for the following reaction given we have 2.6 moles of HCl and1.4 moles of Ca(OH)2?Reaction: 2HCl + Ca(OH)2 2H2O + CaCl2

55)

A) HCl B) H2O C) CaCl2 D) Ca(OH)2

56) How many moles of calcium chloride are theoretically produced for the following reactiongiven we have 2.6 moles of HCl and 1.4 moles of Ca(OH)2?Reaction: 2HCl + Ca(OH)2 2H2O + CaCl2

56)

A) 1.0 B) 1.4 C) 0.7 D) 1.3

57) In order to determine the limiting reactant in a particular reaction, one must know each of thefollowing EXCEPT

57)

A) the molar mass of each reactant present.B) the coefficient of each reactant in a balanced equation.C) the mass of each product formed.D) the mass of each reactant present.

58) What is the limiting reactant for the reaction below given that you start with 2.50 grams C and2.50 grams SiO2?Reaction: C + SiO2 SiC + O2

58)

A) SiO2 B) C C) SiC D) O2

59) How many moles of NH3 can be produced by the reaction of 2.00 g of N2 with 3.00 g H2?Reaction: N2(g) + 3 H2(g) 2 NH3(g)

59)

A) 0.0567 B) 0.235 C) 1.00 D) 0.143

60) Calculate the maximum number of grams of NH3 that can be produced by the reaction of2.00 g of N2 with 3.00 g H2.Reaction: N2(g) + 3 H2(g) 2 NH3(g)

60)

A) 0.964 B) 4.00 C) 17.0 D) 2.43

61) Consider the reaction: 2 Al + 3Br2 2 AlBr3Suppose a reaction vessel initially contains 5.0 mole Al and 6.0 mole Br2. What is in thereaction vessel once the reaction has occurred to the fullest extent possible?

61)

A) 2.0 mole Al; 3.0 mole Br2; 2.0 mole AlBr3B) 0 mole Al; 0 mole Br2; 11.0 mole AlBr3C) 0 mole Al; 1.0 mole Br2; 4.0 mole AlBr3D) 1.0 mole Al; 0 mole Br2; 4.0 mole AlBr3

7

62) The reaction of one mole of nitrogen gas with three moles of hydrogen gas releases 92 kJ ofthermal energy to the surroundings. Which of the following is TRUE?

62)

A) This reaction is exothermic.B) Complete reaction of two moles of nitrogen gas would release 184 kJ of thermal

energy in this reaction.C) This reaction has a negative enthalpy of reaction.D) All of the above are true.

63) Consider the following reaction: 2 Mg + O2 2 MgO H rxn = -1203 kJCalculate the amount of heat (in kJ) associated with complete reaction of 4 moles of Mg.

63)

A) -2406 kJ B) -601.5 kJ C) -4812 kJ D) -1203 kJ

64) Consider the following equation: CO + 2 H2 CH3OH H rxn = -128 kJCalculate the amount of heat (in kJ) associated with complete reaction of 8.08 g H2.

64)

A) -512 kJ B) -1034 kJ C) -256 kJ D) -1024 kJ

65) Which of the following statements about Lewis structures is FALSE? 65)A) A covalent bond occurs when electrons are shared.B) An ionic bond occurs when electrons are transferred.C) An octet is when an atom has 8 valence electrons.D) All of the above statements are true.

66) Which Lewis structure below correctly represents KCl? 66)

A) K [:..Cl··

:] B) K [..Cl··

] C) :..K··

: :..Cl··

: D) K :..Cl··

:

67) Which Lewis structure below correctly represents the compound formed between magnesiumand sulfur?

67)

A) Mg [:..S··

:] 2 Mg B) [:..S··

:] Mg 2 [:..S··

:]

C) Mg [:..S··

:] D) Mg 2 [:..S··

:] 2

68) When a nonmetal bonds with a nonmetal 68)A) a covalent bond is involved. B) a molecular compound forms.C) electrons are shared. D) all of the above are true

69) What is the correct Lewis structure for O2? 69)

A)..O··

=

..O··

B) O-O C) :..O··

-

..O··

: D) : O O :

8

70) What is the correct Lewis structure for N2? 70)

A) : N N : B) :..N··

-

..N··

: C) N-N D)..N··

=

..N··

71) The Lewis structure for carbon monoxide is : C O : This structures shows 71)A) 4 lone pairs and 3 bonding pairs. B) 2 lone pairs and 1 bonding pair.C) 2 lone pairs and 3 bonding pairs. D) 4 lone pairs and 1 bonding pair.

72) Which sequence below represents the proper order of increasing bond strength? 72)A) single < triple < double B) double < single < tripleC) single < double < triple D) triple < double < single

73) The central atom in the chlorate anion, ClO3- is surrounded by 73)A) three bonding and one unshared pair of electrons.B) two bonding and two unshared pairs of electrons.C) one bonding and three unshared pairs of electrons.D) two double bonds and no unshared pairs of electrons.

74) What is the correct Lewis structure for CO2? 74)

A) :..O··

= C=

..O··

: B) :..O··

=

..C··

=

..O··

: C) :..O··

-

..C··

-

..O··

: D) : O··

= C= O··

:

75) What is the correct Lewis structure for CN ? 75)

A) [C-N] B) [..C··

=

..N :] C) [: C N :] D) [:

..C··

-

..N··

:]

76) The correct Lewis structure for BF3 would have exactly: 76)A) 1 double bond. B) 1 triple bond.C) 2 double bonds. D) no double bonds.

77) Which symbol should be used between two structures that represent resonance structures? 77)A) B) C) D)

9

78) Which set shows the correct resonance structures for SeO2? 78)

A) : O··

=Se=

..O··

: O Se-

..O··

: :..O··

-Se O :

B)..O··

=

..Se -

..O··

: :..O··

-

..Se =

..O··

C) :..O··

-

..Se··

-

..O··

:..O··

=

..Se··

=

..O··

D) :..O··

=

..Se··

-

..O··

: :..O··

-

..Se··

=

..O··

:

79) Which of the following compounds have resonance structures? 79)A) O3 B) H2O C) CH4 D) NH3

80) What is the angle between electron groups in the linear electron geometry? 80)A) 90° B) 180° C) 109.5° D) 120°

81) What is the angle between electron groups in the trigonal planar electron geometry? 81)A) 109.5° B) 180° C) 90° D) 120°

82) What is the angle between electron groups in the tetrahedral geometry? 82)A) 90° B) 180° C) 120° D) 109.5°

83) What is the electron geometry if you have 4 electron groups around the center atom? 83)A) tetrahedral B) trigonal bipyramidalC) linear D) trigonal planar

84) What is the electron geometry if you have 3 electron groups around the center atom? 84)A) linear B) trigonal planarC) trigonal bipyramidal D) tetrahedral

85) What is the molecular geometry if you have 3 single bonds and 1 lone pair around the centralatom?

85)

A) linear B) bentC) trigonal pyramidal D) tetrahedral

86) What is the molecular geometry if you have a double bond, a single bond and 1 lone pairaround the central atom?

86)

A) bent B) tetrahedralC) trigonal pyramidal D) linear

87) Which of the following compounds would have a linear molecular geometry?1. N2 2. H2S 3. CO2

87)

A) 1 and 2 only B) 2 and 3 only C) 1,2 and 3 D) 1 and 3 only

10

88) What is the molecular geometry of carbon dioxide, CO2? 88)A) linear B) bentC) tetrahedral D) trigonal pyramidal

89) What is the molecular geometry of PH3? 89)A) tetrahedral B) trigonal pyramidalC) linear D) bent

90) What is the molecular geometry of SiH4? 90)A) trigonal pyramidal B) tetrahedralC) linear D) bent

91) What is the molecular geometry of NH4+? 91)A) tetrahedral B) linearC) trigonal pyramidal D) bent

92) Which of the following has a tetrahedral electron geometry and a trigonal pyramidalmolecular geometry?

92)

A) PF3 B) GeH4 C) SO2 D) Br2O

93) The elements with the highest electronegativity values tend to be found in the: 93)A) lower right-side of the periodic table. B) upper left-side of the periodic table.C) lower left-side of the periodic table. D) upper right-side of the periodic table.

94) Which molecule listed below has a nonpolar covalent bond? 94)A) NaCl B) H2C) H2O D) all of the compounds

95) Which molecule listed below is a polar molecule? 95)A) HCN B) H2OC) NH3 D) all of the compounds

96) Which molecule listed below is a nonpolar molecule? 96)A) BH3 B) CO2C) CCl4 D) all of the compounds

97) Which compound listed below will dissolve in water? 97)A) SiO2 B) CCl4C) NH3 D) all of the compounds

98) Which compound listed below will dissolve in carbon tetrachloride, CCl4? 98)A) NH3 B) NaClC) CS2 D) all of the compounds

11

99) Which of the following statements about the water molecule is TRUE? 99)A) The electronegativities of hydrogen and oxygen are equal and therefore a water molecule

is nonpolar.B) A water molecule is symmetrical and therefore is nonpolar.C) A water molecule has two dipole moments and they cancel each other.D) A water molecule is asymmetric and therefore is polar.

100) Which of the following statements are TRUE about the BF3 molecule? 100)A) BF3 violates the octet rule for the central atom.B) BF3 has a trigonal planar molecular geometry.C) BF3 is nonpolar.D) All of the above statements are true.

101) The electronegativity value for N is 3.0 and that for O is 3.5. Based on these values, which ofthe following statements is TRUE about the compound NO?

101)

A) NO is an ionic compound.B) NO is a polar covalent compound.C) NO is a pure covalent compound.D) There is not enough enough information to determine the nature of NO.

102) The electronegativity value for Mg is 1.2 and the value for O is 3.5. Based on these values,what type of bond is expected for a compound formed between Mg and O?

102)

A) Pure covalent B) IonicC) Polar covalent D) not enough information

103) Which of the following is NOT part of the Kinetic Molecular Theory? 103)A) Gas particles do not repel each other.B) The average energy of the particles is dependent on the molecular mass of the particle.C) There is a large distance between gas particles as compared to their relative size.D) The size of the actual gas particles is small compared to the volume of the whole gas.

104) Which of following statements are consistent with the Kinetic Molecular Theory? 104)A) Gases are compressible because the volume of atoms is almost entirely open space.B) Gases have a low density because there is so much empty space between the particles.C) Gas particles collide with each other and surfaces without losing any energy.D) All of the above statements are consistent with the Kinetic Molecular Theory.

105) All of the following statements are consistent with the kinetic molecular theory of gasesEXCEPT

105)

A) The gas molecules collide with each other and with the surfaces around them.B) The size of the gas molecules is negligible compared to the total volume of the gas.C) Strong attractive forces hold the gas molecules together.D) The average kinetic energy of the molecules of a gas is proportional to the temperature of

the gas in kelvins.

106) 1 atm is equal to: 106)A) 760 mm Hg. B) 101,325 Pa. C) 760 torr. D) all of the above

12

107) 1 torr is equal to: 107)A) 14.7 psi. B) 1 Pa. C) 1 mm Hg. D) 760 mm Hg.

108) What is the equivalent pressure of 0.905 atm in units of mm Hg? 108)A) 840 B) 0.905 C) 13.3 D) 688

109) What is the equivalent pressure of 1520 torr in units of atm? 109)A) 2.00 B) 203,000 C) 380. D) 1520

110) What is the equivalent pressure of 760 torr in units of mm Hg? 110)A) 14.7 B) 1 C) 760 D) 29.92

111) Which of the following statements is TRUE for gases?1. The temperature of a gas is inversely proportional to its pressure.2. The volume of a gas is directly proportional to the pressure in torr.3. The pressure of a gas is due to collisions of the gas molecules.

111)

A) 2 only B) 1 only C) 3 only D) 1 and 2 only

112) To solve problems using Boyle's Law, which mathematical equation should be used? 112)

A)V1P1

=V2P2

B)P1V1

=P2V2

C) P2V1 = P1V2 D) P1V1 = P2V2

113) One liter of a gas is in a sealed chamber containing a moveable piston. If the piston is movedso that the volume of the gas is compressed to a volume of one-half liter, what will happen tothe pressure on the gas? (Assume the temperature is constant and no gas particles are lost.)

113)

A) The pressure will remain the same.B) The pressure will be twice the original value.C) It would be impossible to move the piston since gases are not compressible.D) The pressure will be half of the original value.

114) Divers often inflate heavy duty balloons attached to salvage items on the sea floor. If a balloonis filled to a volume of 3.00 L at a pressure of 2.50 atm, what is the volume of the balloon whenit reaches the surface?

114)

A) 7.50 L B) 5.50 L C) 0.833 L D) 1.20 L

115) Charles's Law is expressed as: 115)

A) V is proportional to T B) V is proportional to 1T

C) V is proportional to 1P

D) P is proportional to V

116) Which one of the following is impossible for an ideal gas? 116)

A) V1T1 = V2T2 B) V2 = ( T2T1

) V1 C) 1V2

=T1T2

( 1V1

) D)V1T1

=V2T2

13

117) A gas sample occupies 3.50 liters of volume at 20.°C. What volume will this gas occupy at100.°C (reported to three significant figures)?

117)

A) 4.46 L B) 2.75 L C) 0.224 L D) 17.5 L

118) What is the initial temperature of a gas if the volume changed from 1.00 L to 1.10 L and thefinal temperature was determined to be 255.0°C?

118)

A) 480°C B) 232°C C) 207°C D) -41°C

119) Gas density can be calculated by dividing the mass of gas by its volume. If you took a balloonof gas and then warmed the balloon in a sunny window, what can now be said about thedensity of the gas in the balloon?

119)

A) The gas density will remain the same.B) The gas density will decrease.C) The gas density will increase.D) The density of gases is independent of temperature.

120) What is the proper form of the combined gas law? 120)

A) V1T1P1

=V2T2

P2B) P1V1T1 = P2V2T2

C) P1V1T1

=P2V2

T2D) P1T1

V1=

P2T2V2

121) A certain volume of gas was confined in a rigid container. If the pressure of the gas sample inthe container was doubled, what happened to the temperature?

121)

A) The temperature became one half. B) The temperature increased four times.C) The temperature doubled. D) The temperature decreased one-third.

122) Suppose a balloon was released from the ground and rose to such a height that both theatmospheric pressure and atmospheric temperature decreased. Which statement is TRUE?

122)

A) Both the temperature and pressure changes act to decrease the balloon's volume.B) The temperature change acts to increase the balloon's volume.C) Both the temperature and pressure changes act to increase the balloon's volume.D) none of the above

123) If the initial pressure of a system was 1.00 atm and the volume was halved and thetemperature was tripled, what is the final pressure?

123)

A) 6.00 atm B) 2.00 atm C) 1.50 atm D) 0.667 atm

124) What is the initial temperature (°C) of a system that has the pressure decreased by 10 timeswhile the volume increased by 5 times with a final temperature of 150 K?

124)

A) -198 B) 27 C) 300 D) 75

125) Avogadro's Law is expressed as: 125)

A) V is proportional to 1n

B) V is proportional to n

C) P is proportional to n D) n is proportional to 1T

14

126) What happens to the volume of a gas when you double the number of moles of gas whilekeeping the temperature and pressure constant?

126)

A) The volume increases, but more information is needed.B) The volume decreases, but more information is needed.C) The volume doubles.D) The volume is halved.

127) If each of the following gas samples have the same temperature and pressure, which samplehas the greatest volume?

127)

A) 1 gram of Ar B) 1 gram of O2C) all have the same volume D) 1 gram of H2

128) The ideal gas law is: 128)

A) T =PVnR

B) V =nRT

PC) PV = nRTD) All of the above are forms of the ideal gas law.

129) Which conditions can cause nonideal gas behavior by 1) decreasing the space between gasparticles or 2) by slowing gas particles so that interactions are significant?

129)

A) 1) high pressure; 2) low temperature B) 1) low pressure ; 2) low temperatureC) 1) low pressure; 2) high temperature D) 1) high pressure; 2) high temperature

130) What is the major component of the air we breathe? 130)A) smog B) argon C) oxygen D) nitrogen

131) If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxideat 345 torr, what is the total pressure of the system?

131)

A) 1,329 atm B) 639 torr C) 17.5 cm Hg D) 1.75 atm

132) A gas cylinder contains only the gases radon, nitrogen, and helium. The radon has a pressureof 222 torr while the nitrogen has a pressure of 446 torr. If the total pressure inside the cylinderis 771 torr, what is the pressure that is due to the helium?

132)

A) 771 torr B) 668 torr C) 103 torr D) 549 torr

133) What problem could happen if deep sea divers used pure oxygen in their tanks? 133)A) nitrogen narcosis B) oxygen toxicityC) rapture of oxygen D) hypoxia

134) Human lungs have evolved to breathe oxygen at a pressure as that in the atmosphere, 0.21atm. If a particular heliox mixture to be carried by a scuba diver is at a pressure of 7.00 atm,what should be the partial pressure due to helium in order to maintain the pressure due tooxygen at 0.21 atm?

134)

A) 7.00 atm B) 6.79 atm C) 0.21 atm D) 7.21 atm

15

135) Which set of conditions reflect STP? 135)A) 273 K, 1 Pa B) 373 K, 760 torrC) 298 K, 1 atm D) 273 K, 760 mm Hg

136) Suppose you had a balloon containing 1 mole of helium at STP and a balloon containing 1mole of oxygen at STP. Which statement is TRUE?

136)

A) The balloons will have the same volume.B) The balloons will have the same mass.C) Both A) and B) are true.D) Neither A) nor B) are true.

137) Ammonia gas decomposes according to the equation:2NH3(g) N2(g) + 3H2(g)

If 15.0 L of nitrogen is formed at STP, how many liters of hydrogen will be produced (alsomeasured at STP)?

137)

A) 90.0 L B) 15.0 L C) 30.0 L D) 45.0 L

138) Water can be formed according to the equation:2H2 (g) + O2 (g) 2H2O (g)

If 8.0 L of hydrogen is reacted at STP, exactly how many liters of oxygen at STP would beneeded to allow complete reaction?

138)

A) 4.0 L B) 1.0 L C) 2.0 L D) 8.0 L

139) How many liters of O2 (g) are needed to react completely with 56.0 L of CH4 (g) at STP toproduce CO2 (g) and H2O (g)?Given: CH4 (g) + 2O2 (g) CO2 (g) + H2O (g)

139)

A) 112. L B) 56.0 L C) 84.0 L D) 28.0 L

140) Intermolecular forces are responsible for: 140)A) the function of DNA. B) the shape of protein molecules.C) the existence of liquids and solids. D) all of the above

141) Which state of matter has a high density and an indefinite shape? 141)A) gases B) solidsC) liquids D) both solids and liquids

142) Which state of matter has a high density and a definite volume? 142)A) gases B) liquidsC) solids D) both solids and liquids

143) Which state of matter has a low density and is easily compressed? 143)A) liquids B) solidsC) gases D) both solids and liquids

144) The tendency of a liquid to minimize its surface area is called: 144)A) vaporization. B) viscosity.C) capillary action. D) surface tension.

16

145) The measure of the resistance to the flow of a liquid is called: 145)A) sublimation. B) vapor pressure.C) condensation. D) viscosity.

146) A situation where two opposite processes are occurring at equal rates, and no net change istaking place, is called:

146)

A) condensation. B) evaporation.C) vaporization. D) dynamic equilibrium.

147) Increasing the intermolecular forces of a liquid will do which of the following? 147)A) decrease the evaporation rate B) increase the surface tensionC) decrease the vapor pressure D) all of the above

148) The rate of vaporization of a liquid can be increased by1. increasing the surface area2. increasing the temperature3. increasing the strength of the intermolecular forces

148)

A) 1 only B) 2 only C) 3 only D) 1 and 2 only

149) The amount of heat required to melt one mole of a solid is called the: 149)A) heat of vaporization. B) cooling curve.C) heating curve. D) heat of fusion.

150) What happens as you start to add heat to a solid substance? 150)A) Heating of the now formed liquid results in increasing the liquid temperature.B) Increasing the rate of heating of a substance at its melting point only causes more rapid

melting.C) Thermal energy causes the components of the solid to vibrate faster.D) all of the above

151) When you make ice cubes: 151)A) it is an exothermic process.B) it is an endothermic process.C) the heat of vaporization must be removed.D) the process is referred to scientifically as sublimation.

152) Which statement is TRUE in describing what occurs when a solid melts to a liquid? 152)A) The process is endothermic and the heat of fusion is positive.B) The process is exothermic and the heat of fusion is positive.C) The process is endothermic and the heat of fusion is negative.D) The process is exothermic and the heat of fusion is negative.

17

153) In northern climates, it is common to have a layer of frost form on cars that have been outovernight in the winter. During the day the frost layer disappears despite its temperatureremaining below freezing. How?

153)

A) The frost evaporates due to the sun heating the solid.B) The frost melts due to the sun heating the surface of the car above the melting point.C) The frost sublimes directly from solid ice to water vapor.D) The frost cycles as does the saturation level of moisture in the winter air does from night

to day.

154) A mothball can change directly from its solid phase to its gaseous phase. This process isknown as:

154)

A) melting. B) sublimation. C) condensation. D) deposition.

155) Which intermolecular force is present in all molecules and atoms? 155)A) X-forces B) dipole-dipole forcesC) hydrogen bonding D) dispersion forces

156) Which intermolecular force is due to the formation of an instantaneous dipole? 156)A) dispersion forces B) X-forcesC) hydrogen bonding D) dipole-dipole forces

157) Which intermolecular force increases with increasing molar mass? 157)A) dipole-dipole forces B) dispersion forcesC) hydrogen bonding D) X-forces

158) Assuming that the molecules carbon monoxide (CO) and nitrogen (N2) have similar electronclouds, which statement below is TRUE?

158)

A) The N2 has the higher boiling point because it has greater dispersion forces.B) Both CO and N2 must have the same boiling point.C) CO has the higher boiling point because it experiences dipole-dipole forces.D) N2 has the higher boiling point because it experiences dipole-dipole forces.

159) Which intermolecular force is common to all polar molecules but NOT nonpolar molecules? 159)A) dispersion forces B) X-forcesC) dipole-dipole forces D) hydrogen bonding

160) Which statement below is FALSE? 160)A) A hydrogen bond is the strongest of the intermolecular forces.B) A hydrogen atom must be bonded directly to fluorine, oxygen, or nitrogen to exhibit

hydrogen bonding.C) The large electronegativity difference between hydrogen and an F, O, or N atom is

essential for the formation of a hydrogen bond.D) none of the above

161) Which molecule below has hydrogen bonding? 161)A) H2O B) CH3OH C) HF D) all of the above

18

162) Which compound will have the highest boiling point? 162)A) CH3CH2OH B) CH3C(O)CH3 C) CH4 D) CH3CH3

163) Which substance would be expected to have the highest boiling point? 163)A) CO B) N2 C) O2 D) CO2

164) Which intermolecular force is the strongest? 164)A) dispersion forces B) X-forcesC) dipole-dipole forces D) hydrogen bonding

165) Which intermolecular forces are found in CCl4? 165)A) dipole-dipole forces B) X-forcesC) dispersion forces D) hydrogen bonding

166) Rank the compounds NH3, CH4, and PH3 in order of increasing boiling point. 166)A) NH3 < CH4< PH3 B) CH4 < PH3 < NH3C) NH3 < PH3< CH4 D) CH4< NH3 < PH3

167) What types of forces exist between I2 molecules? 167)A) dispersion forces B) ion-dipole forcesC) hydrogen bonding D) dipole-dipole forces

168) Dry ice (solid CO2) is which type of solid? 168)A) covalent atomic solid B) metallic atomic solidC) nonbonding atomic solid D) molecular solid

169) NaCl is which type of solid? 169)A) molecular solid B) covalent atomic solidC) nonbonding atomic solid D) ionic solid

170) Silicon is which type of solid? 170)A) nonbonding atomic solid B) molecular solidC) ionic solid D) covalent atomic solid

171) Why is water considered an unusual molecule? 171)A) Water can dissolve many polar and ionic compounds.B) No molecule of similar size is a liquid at room temperature.C) No molecule of similar size has as high a boiling point.D) all of the above

172) The reason for many of the unique properties of water is: 172)A) moderate viscosity and expanding upon freezing.B) dispersion forces.C) high surface tension and low volatility.D) the ability to form hydrogen bonds.

19

173) Which of the following is NOT a property of acids? 173)A) Acids have a slippery feel. B) Acids dissolve many metals.C) Acids have a sour taste. D) Acids turn litmus paper red.

174) Which of the following statements about acids are TRUE?1. An acid is used in car batteries.2. The active ingredient of vinegar is an acid.3. Acids are used for cleaning metals.

174)

A) 2 and 3 only B) 1 and 2 onlyC) 1 and 3 only D) All of 1, 2, and 3

175) Which of the following is NOT a property of bases? 175)A) Bases have a slippery feel. B) Bases turn litmus paper blue.C) Bases have a bitter taste. D) Bases dissolve many metals.

176) Which of the following statements about a base are TRUE?1. Bases are used in the manufacturing of soap.2. Bases have a sour taste.3. Fertilizer manufacture and cotton processing use bases.

176)

A) 1 and 3 only B) 2 and 3 onlyC) 1 and 2 only D) All of 1, 2, and 3

177) Which of the following common bases is commonly used for manufacturing fertilizer? 177)A) NH3 B) KOH C) NaHCO3 D) NaOH

178) The Arrhenius definition of an acid is: 178)A) produces H in solution. B) a proton donor.C) produces OH in solution. D) a proton acceptor.

179) The Bronsted-Lowry definition of a base is: 179)A) produces OH in solution. B) produces H in solution.C) a proton acceptor. D) a proton donor.

180) The Bronsted-Lowry definition of an acid is: 180)A) a proton donor. B) produces OH in solution.C) produces H in solution. D) a proton acceptor.

181) Which of the following is NOT true? 181)A) The Arrhenius Model of acids and bases applies toward substances that are nonaqueous.B) The Bronsted-Lowry Model can apply to bases that do not contain hydroxide ions.C) The Arrhenius Model of acids and bases was developed before the Bronsted-Lowry

Model.D) The Bronsted-Lowry Model applies to a wider range of acid-base phenomena than does

the Arrhenius Model.

20

182) In the following reaction:HCO3- (aq) + H2O (aq) H2CO3 (aq) + OH- (aq)

182)

A) HCO3- is an acid and H2CO3 is its conjugate base.B) H2O is an acid and HCO3- is its conjugate base.C) H2O is an acid and H2CO3 is its conjugate base.D) H2O is an acid and OH- is its conjugate base.

183) In the following reaction: NH4+ (aq) + H2O (aq) NH3 (aq) + H3O+ (aq) 183)A) NH4+ is a base and H2O is its conjugate acid.B) H2O is a base and H3O+ is its conjugate acid.C) NH4+ is an acid and H2O is its conjugate base.D) NH4+ is an acid and H3O+ is its conjugate base.

184) What is the conjugate acid of OH ? 184)A) OH B) H2O C) NaOH D) O2-

185) What is the conjugate base of H2O? 185)

A) OH B) NaOH C) O2- D) H3O+

186) A substance that acts as an acid or a base is called 186)A) hydrophillic. B) isoprotic. C) a salt. D) amphoteric.

187) When an acid reacts with a metal, what is one of the usual products? 187)A) salt B) carbon dioxide C) water D) hydrogen gas

188) A neutralization reaction between an acid and sodium hydroxide formed water and the saltnamed sodium sulfate. What was the formula of the acid that was neutralized?

188)

A) H2S B) HCl C) H2SO4 D) Na2SO4

189) Which of the following acids is diprotic? 189)A) HClO4 B) H2SO4 C) HNO3 D) HI

190) Which of the following acids is a diprotic, weak acid? 190)A) phosphoric acid B) carbonic acidC) sulfuric acid D) hydrobromic acid

191) A 0.10 M solution of an electrolyte has a pH of 4.5. The electrolyte is: 191)A) a weak acid. B) a weak base. C) a strong acid. D) a strong base.

192) What is the concentration of H in 2.0 M acetic acid, HC2H3O2? 192)A) >2.0 M B) 1.0 M C) < 2.0 M D) 2.0 M

193) Which of the following is a weak base? 193)A) potassium hydroxide B) calcium hydroxideC) sodium fluoride D) ammonia

21

194) Consider a 1.6 × 10-3 M solution of HNO3. Which of the following statements is NOT true? 194)A) This solution could neutralize a base. B) This solution has a pH of 11.20.C) This solution could dissolve metal. D) This solution would turn litmus to red.

195) What is the concentration of the hydronium ions in a neutral solution? 195)A) > 1.0 × 10-7 M B) < 1.0 × 10-7 M C) 1.0 × 10-7 M D) 1.0 × 10-14 M

196) What is the concentration of the hydroxide ions in an acidic solution? 196)A) 0.0 M B) 1.0 × 10-7 M C) > 1.0 × 10-7 M D) < 1.0 × 10-7 M

197) What is the concentration of the hydronium ions in an acidic solution? 197)A) 1.0 × 10-14 M B) > 1.0 × 10-7 M C) 1.0 × 10-7 M D) < 1.0 × 10-7 M

198) What is the value of the ion product constant for water (Kw)? 198)A) 1.0 × 107 B) 1.0 × 1014 C) 1.0 × 10-14 D) 1.0 × 10-7

199) Which solution below has the highest concentration of hydroxide ions? 199)A) pH = 12.49 B) pH = 10.12 C) pH = 7.00 D) pH = 3.21

200) The pH of a solution is 5.00. Which of the following is TRUE about the solution? 200)A) Its [H3O+] is 1.0 × 10-9 MB) Its [H3O+] is 1.0 × 105 MC) Its [H3O+] is 1.0 × 10-5 MD) It is more acidic than a solution whose pH is 4.00.

201) In order for a solution to be acidic, 201)A) [H3O+] > [OH-] B) [H3O+] = [OH-]C) pH = pOH D) [H3O+] < [OH-]

202) In order for a solution to be basic, 202)A) [H3O+] < [OH-] B) [H3O+] > [OH-]C) [H3O+] = [OH-] D) pH = pOH

203) In a solution that has a pH = 7.0, 203)A) [H3O+] + [OH-] = Kw B) [H3O+] > [OH-]

C) [H3O+] < [OH-] D) [H3O+] = [OH-]

204) A solution at 25°C has a hydrogen ion concentration of 2.6 × 10-5 M. Which of the following isTRUE?

204)

A) [H3O+] < [OH-] B) [H3O+] = [OH-]

C) [H3O+] > [OH-] D) [H3O+] =[OH-]

Kw

22

205) Which solution below is considered to have basic character? 205)A) pOH = 4 B) pOH = 13 C) pOH = 7 D) pH = 2

206) If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydroniumion concentration?

206)

A) It increased. B) It became zero.C) It decreased. D) It became less than zero.

207) Which of the following is TRUE of alkaloid compounds? 207)A) Alkaloids occur naturally in many plants.B) Some narcotic drugs are alkaloids.C) Alkaloids are organic bases.D) All of the above are true.

208) A buffer solution is all of the following EXCEPT: 208)A) a solution that contains both a weak acid and its conjugate base.B) a solution that resists a change in pH when a base is added.C) a solution that resists a change in pH when an acid is added.D) a solution that regulates pH by the addition of a strong acid or base.

209) Which of the following statements are TRUE of buffer solutions?1. A buffer solution can be made by mixing equal concentrations of

acetic acid and sodium acetate.2. A buffer solution can be made by mixing equal concentrations of

hydrochloric acid and sodium chloride.3. A buffer solution resists changes in pH when small quantities of acid

or base are added.

209)

A) 1 and 2 only B) 1 and 3 onlyC) 2 and 3 only D) All of 1, 2, and 3

210) Which combination below will be a buffer solution? 210)A) HC2H3O2 and NaC2H3O2 B) HCl and ClC) NaBr and NaOH D) HNO3 and NaNO3

211) Acid rain legislation targeted the release of which compound by industry? 211)A) benzene B) CO2 C) SO2 D) dioxin

212) According to the collision theory of chemical reactions: 212)A) high energy collisions lead to the successful formation of products.B) low energy collisions do not occur in the gas phase.C) low energy collisions result in many successful reactions as there is sufficient time for the

reactants to form products.D) high energy collisions result in few successful reactions as there isn't sufficient time for

the products to react.

23

213) Which of the following changes will increase the reaction rate? 213)A) an increase in the concentration of reactantsB) an increase in the concentration of the productsC) a decrease of the reaction temperatureD) allowing more time for the reaction

214) Which of the following changes will increase reaction rate?1. An increase in the concentration of reactants2. An increase in temperature3. Higher-energy collisions between reacting molecules

214)

A) 2 and 3 only B) 1 and 3 onlyC) 1 and 2 only D) All of 1, 2, and 3

215) Which of the following is TRUE for a system that is in dynamic equilibrium? 215)A) The reaction rate of the forward reaction approaches zero.B) Both the forward and reverse reactions come to a halt.C) The forward reaction goes to 100% completion.D) none of the above

216) A chemical equilibrium exists when 216)A) there are equal amounts of reactants and products.B) the sum of reactant and product concentrations equals one mole.C) the rate at which reactants form products is the same as the rate at which products form

reactants.D) the rate at which reactants form products becomes zero.

217) A system is said to be in dynamic equilibrium when: 217)A) the forward and reverse reactions come to a halt.B) the sum of the concentrations of the reactants is equal to the sum of the concentrations of

the products.C) you have let the reaction proceed for approximately 30 minutes and can assume there

will be no more changes.D) there is no longer any net change in the concentrations of products or reactants.

218) For the reaction 2A + B 2C + 3D, the equilibrium expression is: 218)

A) Keq =[2C][3D][2A][B]

B) Keq =[A]2[B]

[C]2[D]3C) Keq =

[C]2[D]3

[A]2[B]D) Keq =

[2][1][2][3]

219) The chemical equation that would generate the equilibrium expression Keq =[B]2 [C]

[A]3 is

________. (Assume all substances are gases in this reaction.)

219)

A) C + 2B 3A B) 1/2 B + C 1/3 AC) A B + C D) 3A 2B + C

24

220) For the reaction S2F6 2SF2 + F2, the equilibrium expression is: 220)

A) Keq =[S2F6]

[SF2][F2]B) Keq =

[SF2][F2][S2F6]

C) Keq =[SF2]2[F2]

[S2F6]D) Keq =

[S2F6]

[SF2]2[F2]

221) Which equilibrium constant represents a reaction that favors the formation of the products tothe greatest extent?

221)

A) Keq = 1.0 × 10-18 B) Keq = 100C) Keq = 1.0 × 108 D) Keq = 1.0 × 10-3

222) Which equilibrium constant represents a reaction that favors the reactants to the greatestextent?

222)

A) Keq = 1.0 × 108 B) Keq = 1.0 × 10-3

C) Keq = 1.0 × 10-18 D) Keq = 100

223) Which of the following is TRUE of a system for which Keq << 1? 223)A) It will take a long time to reach equilibrium.B) The equilibrium favors the reverse reaction.C) It will take a short time to reach equilibrium.D) The equilibrium favors the forward reaction.

224) Which of the following is TRUE of a system for which Keq >> 1? 224)A) It will take a short time to reach equilibrium.B) The equilibrium favors the reverse reaction.C) The equilibrium favors the forward reaction.D) It will take a long time to reach equilibrium.

225) What must be TRUE for a reaction possessing a large equilibrium constant? 225)A) The reverse reaction is favored. B) The forward reaction is favored.C) The reaction rate is fast. D) The reaction rate is slow.

226) When writing the expression for an equilibrium constant, which type of substance ISincluded?

226)

A) pure liquids B) gases C) solids D) all of the above

227) For the reaction 2 H2O (l) 2H2 (g) + O2 (g), the equilibrium expression is: 227)

A) Keq = [H2]2 [O2] B) Keq =[H2]2 [O2]

[H2O]2

C) Keq =[H2]2 [O]2

[H2O]2D) Keq = [H2O]2

25

228) For the reaction Cu2S(s) 2Cu+(aq) + S2-(aq), the equilibrium expression is: 228)

A) Keq = [Cu2S] B) Keq =[Cu+][ S2-]

[Cu2S]

C) Keq = [Cu+]2[ S2-] D) Keq =[Cu+]2[ S2-]

[Cu2S]

229) Le Chatelier's Principle states that: 229)A) when a system at equilibrium is disturbed, a new equilibrium constant is established.B) a disturbing force must be applied to a system in order for it to reach equilibrium.C) when a chemical system at equilibrium is disturbed, the system shifts in order to

minimize the effect.D) when a chemical system is at equilibrium it is no longer possible to alter the system.

230) For the reaction Ag2S(s) 2Ag+(aq) + S2-(aq), what happens to the equilibrium position ifaqueous ammonium sulfide is added?

230)

A) doubles B) shifts to the leftC) shifts to the right D) does nothing

231) For the reaction Ag2S(s) 2Ag+(aq) + S2-(aq), what happens to the equilibrium position ifammonium sulfate is added?

231)

A) doubles B) shifts to the leftC) shifts to the right D) does nothing

232) For the reaction Ag2S(s) 2Ag+(aq) + S2-(aq), what happens to the equilibrium position ifthe amount of solid silver sulfide is doubled?

232)

A) doubles B) shifts to the rightC) shifts to the left D) does nothing

233) For the reaction Ag2S(s) 2Ag+(aq) + S2-(aq), what happens to the equilibrium position ifthe amount of silver ion is halved?

233)

A) shifts to the left B) shifts to the rightC) doubles D) does nothing

234) Consider the reaction: 2N2O(g) O2(g) + 2N2(g). Which of the following will cause a shift inthe equilibrium to the right?

1. Add more N2O2. Remove O23. Remove N2

234)

A) 1 and 3 only B) 1 and 2 onlyC) 2 and 3 only D) All of 1, 2, and 3

26

235) Consider the reaction: 2N2O(g) O2(g) + 2N2(g). Which of the following will cause a shift inthe equilibrium to the left?

1. Remove N2O2. Remove O23. Add N2

235)

A) 1 and 2 only B) 2 and 3 onlyC) 1 and 3 only D) All of 1, 2, and 3

236) We have the following reaction at equilibrium in a flask,CaSO4(s) Ca2+(aq) + SO42+(aq)

What will happen to [Ca2+] if additional CaSO4 is added to the flask?

236)

A) It will increase.B) It will decrease.C) It will not change.D) Cannot tell with the information provided.

237) For the reaction 2N2O(g) O2(g) + 2N2(g), what happens to the equilibrium position if thepressure increases?

237)

A) shifts to the right B) doublesC) does nothing D) shifts to the left

238) For the reaction H2 (g) + Cl2 (g) 2 HCl (g), what happens to the equilibrium position if thepressure increases?

238)

A) shifts to the left B) shifts to the rightC) doubles D) does nothing

239) For the reaction 2N2O(g) O2(g) + 2N2(g), what happens to the equilibrium position if thepressure decreases?

239)

A) does nothing B) shifts to the leftC) doubles D) shifts to the right

240) For the reaction 2N2O(g) O2(g) + 2N2(g), what happens to the equilibrium position if thevolume decreases?

240)

A) shifts to the left B) doublesC) does nothing D) shifts to the right

241) For the reaction 2N2O(g) O2(g) + 2N2(g), what happens to the equilibrium position if thevolume increases?

241)

A) does nothing B) shifts to the rightC) doubles D) shifts to the left

242) What happens to the equilibrium position of an exothermic reaction when you add heat? 242)A) does nothing B) shifts to the rightC) shifts to the left D) doubles

27

243) What happens to the equilibrium position of an exothermic reaction when you remove heat? 243)A) shifts to the left B) doublesC) shifts to the right D) does nothing

244) What happens to the equilibrium position of an endothermic reaction when you add heat? 244)A) shifts to the right B) does nothingC) doubles D) shifts to the left

245) What happens to the equilibrium position of an endothermic reaction when you remove heat? 245)A) doubles B) shifts to the rightC) does nothing D) shifts to the left

246) Which compound is the most soluble? 246)A) AgCl, Ksp = 1.77 × 10-10 B) AgI, Ksp = 8.51 × 10-17

C) PbS, Ksp = 9.04 × 10-29 D) CuS, Ksp = 1.27 × 10-36

247) What is the Ksp expression for the ionic compound Li2CO3? 247)

A) Ksp = [Li+]2 [CO32-] B) Ksp = [Li2CO3]3

C) Ksp = 2[Li+] [CO32-] D) Ksp = [Li+] [CO32-]

248) Which statement about activation energy is FALSE? 248)A) Increasing the temperature lowers the activation energy.B) The higher the activation energy, the slower the reaction rate.C) Activation energy is an energy hump that normally exists between reactants and

products.D) The lower the activation energy, the faster the reaction rate.

249) Comparing a reaction with a catalyst to the same reaction without the catalyst, each of thefollowing statements is true EXCEPT

249)

A) The rate for the reaction with a catalyst is faster.B) Both reactions would have the same value for the equilibrium constant.C) The activation energy is the same for both the catalyzed and uncatalyzed reaction.D) The products are the same.

250) Which statement below is FALSE? 250)A) The rate of a reaction can be increased by increasing concentrations of reactants.B) A catalyst alters the equilibrium constant.C) The rate of a reaction can be increased by altering the temperature.D) The rate of a reaction can be increased by adding a catalyst.

28