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

Transcription

1 General Chemistry PHS 1015 Practice Exam 3 Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following equations has 1:1:1:1 as the coefficient ratio when balanced? 1) A) H2SO4 + KOH K2SO4 + H2O B) Zn + HCl H2 + ZnCl2 C) CH4 + O2 CO2 + H2O D) NaOH + HCl NaCl + H2O 2) Which of the following equations has 1:2:1:1 as the coefficient ratio when balanced? 2) A) H2SO4 + KOH K2SO4 + H2O B) Zn + HCl H2 + ZnCl2 C) CH4 + O2 CO2 + H2O D) NaOH + HCl NaCl + H2O 3) Which of the following balanced reactions does not have at least one 6 as a coefficient? 3) A) H2SO4 + Al(OH)3 Al2(SO4)3 + H2O B) H3PO4 + Ba(OH)2 Ba3(PO4)2 + H2O C) C6H12O6 + O2 CO2 + H2O D) C2H2 + O2 CO2 + H2O 4) The coefficients are respectively for the following equation. Fe2O3 + Al Al2O3 + Fe A) 1: 2: 1: 2 B) 2: 3: 2: 3 C) 1: 2: 2: 1 D) 2: 3: 3: 4 5) The coefficients are respectively for the following equation. C4H10 + O2 CO2 + H2O A) 1: (13/2): 4: 5 B) 2: 13: 8: 10 C) 1: 13: 4: 5 D) either A or B 4) 5) 6) Which of the following equations does not have 1:2:1:2 as the coefficient ratio when balanced? 6) A) H2SO4 + KOH K2SO4 + H2O B) Ca(OH)2 + HCl CaCl2 + H2O C) CH4 + O2 CO2 + H2O D) K + H2O H2 + KOH 7) Which of the following has 6 as one of the coefficients when the equation is balanced? 7) A) H2SO4 + Al(OH)3 Al2(SO4)3 + H2O B) C2H6O +O2 CO2 + H2O C) Mg + HCl H2 + MgCl2 D) Al(OH)3 + HCl AlCl3 + H2O 8) What is the coefficient for iron after the following reaction is balanced? Fe + O2 Fe2O3 A) 1 B) 3 C) 4 D) 6 9) What is the sum of all coefficients after the following equation is balanced? C8H18 + O2 CO2 + H2O A) 4 B) 18 C) 32 D) 61 10) What is the sum of all coefficients after the following equation is balanced? K2CrO4 + Al(NO3)3 Al2(Cr O4)3 + KNO3 A) 4 B) 8 C) 12 D) 15 8) 9) 10) 1

2 11) Which of the following reactions is a single replacement reaction? 11) A) HCl + NaOH NaCl + H2O B) Mg + HCl H2 + MgCl2 C) CaCl2 + H2O CaCl2 2H2O D) KClO3 KCl + O2 12) Which of the following reactions is a double replacement reaction? 12) A) HCl + NaOH NaCl + H2O B) Mg + HCl H2 + MgCl2 C) CaC12 + H2O CaCl2 2H2O D) KClO3 KCl + O2 13) Which of the following reactions is a decomposition reaction? 13) A) HCl + NaOH NaCl + H2O B) Mg + HCl H2 + MgCl2 C) CaCl2 + H2O CaCl2 2H2O D) KClO3 KCl + O2 14) Which of the following is an example of a combination reaction? 14) A) HCl + NaOH NaCl + H2O B) Mg + HCl H2 + MgCl2 C) 2 Na + Cl2 2NaCl D) KClO3 KCl + O2 15) Which of the following equations is not a combustion reaction? 15) A) C2H6O + O2 H2O + CO2 B) CH4 + O2 CO + H2O C) KClO3 KCl +O2 D) Fe + O2 FeO 16) The following equation is an example of a reaction. NaClO3 NaCl + O2 A) combination B) combustion C) decomposition D) double replacement 17) The following equation is an example of a reaction. Zn + CuCl2 Cu + ZnCl2 A) combination B) single replacement C) double replacement D) decomposition 18) The following equation is an example of a reaction. K2SO4 + BaCl2 BaSO4 + KCl A) combination B) single replacement C) double replacement D) decomposition 16) 17) 18) 19) Which of the following equations is not a single replacement reaction? 19) A) H2SO4 + Mg(OH)2 H2O + MgSO4 B) Zn + HCl H2 + ZnCl2 C) Al + Fe2O3 Al2O3 + Fe D) Na + H2O NaOH + H2 20) Which of the following equations is not a double replacement reaction? 20) A) H2SO4 + Mg(OH)2 H2O + MgSO4 B) Mg + HCl H2 + MgCl2 C) AlCl3 + H2O Al(OH)3 + HCl D) AgNO3 + NaCl AgCl + NaNO3 21) Which of the following equations is not a decomposition reaction? 21) A) CaSO4 2H2O CaSO4 + 2 H2O B) NaClO3 NaCl + O2 C) H2O2 H2O + O2 D) K + H2O KOH + H2 2

3 22) Which of the following equations is not a combination reaction? 22) A) H2 + O2 H2O B) C2H4 + Br2 C2H4Br2 C) CH4 + O2 CO2 + H2O D) Fe + O2 Fe3O4 23) Which of the following equations is a combustion reaction? 23) A) MgO + HCl MgCl2 + H2O B) Al + Fe2O3 Al2O3 + Fe C) KClO3 KCl + O2 D) CH4 + O2 CO2 + H2O 24) The following equation is an example of a reaction. C8H18 + O2 CO2 + H2O A) synthesis B) decomposition C) double displacement D) combustion 25) The spectator ions in the following precipitation equation are AgNO3 + NaCl AgCl + NaNO3 A) Ag+ and NO3 - B) Na+ and NO3 - C) Ag+ and Cl- D) Na+ and Cl- 24) 25) 26) Which ions are not spectator ions in the following precipitation equation? AgNO3 + NaCl AgCl + NaNO3 A) Ag+ and NO3 - B) Na+ and NO3 - C) Ag+ and Cl- D) Na+ and Cl- 26) 27) The following equation is an example of a reaction. Pb(NO3 )2+ 2KI PbI2 + 2KNO3 A) synthesis B) precipitation C) single replacement D) decomposition 28) The spectator ions in the following precipitation equation are Pb(NO3)2+ 2KI PbI2 + 2KNO3 A) Pb2+ and I- B) K+ and NO3 - C) K+ and I- D) Pb2+ and NO3-27) 28) 29) Which of the following is the least soluble in water? 29) A) sodium sulfate B) lead (II) nitrate C) potassium chloride D) calcium sulfate 30) Which of the following salts is insoluble in water? 30) A) K2SO4 B) AgNO3 C) CaCO3 D) Na3PO4 31) Which of the following salts is soluble in water? 31) A) AgCl B) BaCO3 C) Ca(SO4) D) NaNO3 32) Which hydroxide is insoluble in water? 32) A) sodium hydroxide B) barium hydroxide C) aluminum hydroxide D) calcium hydroxide 3

4 33) Which hydroxide is soluble in water? 33) A) lead (II) hydroxide B) magnesium hydroxide C) calcium hydroxide D) strontium hydroxide 34) Which chloride is soluble in water? 34) A) lead (II) chloride B) calcium chloride C) mercury (I) chloride D) silver chloride 35) Which sulfate is insoluble in water? 35) A) ammonium sulfate B) strontium sulfate C) sodium sulfate D) potassium sulfate 36) Which sulfate is soluble in water? 36) A) calcium sulfate B) barium sulfate C) lithium sulfate D) lead (II) sulfate 37) Which sulfide is insoluble in water? 37) A) lead (II) sulfide B) potassium sulfide C) ammonium sulfide D) sodium sulfide 38) Which phosphate is soluble in water? 38) A) ammonium phosphate B) cobalt (II) phosphate C) aluminum phosphate D) barium phosphate 39) Which lead (II) compound is soluble in water? 39) A) lead (II) sulfate B) lead (II) carbonate C) lead (II) chloride D) lead (II) nitrate 40) Which of the following equations is not a precipitation reaction? 40) A) Na2SO4 + CaCl2 CaSO4 + NaCl B) MgCl2 + AgNO3 Mg(NO3)2 + AgCl C) NaOH + HCl NaCl + H2O D) NaCl+ AgC2H3O2 AgCl + NaC2H3O2 41) The following equation is an example of a reaction. AgNO3 + NaCl AgCl + NaNO3 A) combination B) precipitation C) single replacement D) decomposition 42) Which ions are not spectator ions in the following precipitation equation? Pb(NO3)2+ 2KI PbI2 + 2KNO3 A) Pb2+ and I- B) K+ and NO3 - C) K+ and I- D) Pb2+ and NO3-41) 42) 43) When aqueous solutions of sodium phosphate and calcium nitrite are mixed, the spectator ions are A) calcium and nitrite B) sodium and phosphate C) calcium and phosphate D) sodium and nitrite 43) 4

5 44) When aqueous solutions of calcium hydroxide and hydrobromic acid are mixed, the spectator ions are A) calcium and bromide B) hydrogen and hydroxide C) calcium and hydroxide D) hydrogen and bromide 45) When aqueous solutions of sodium nitrate and potassium chloride are mixed, the spectator ions are A) potassium and nitrate B) sodium and chloride C) both A and B D) no spectator ions are present 46) The net ionic equation for the following reaction is AgNO3 + NaCl AgCl + NaNO3 A) Ag+ (aq) + NO3 - (aq) AgNO3 B) Ag+ (aq) + Cl- (aq) AgCl (s) C) Na+ (aq) + NO3 - (aq) NaNO3 D) NaCl + AgNO3 AgCl (s) 44) 45) 46) 47) If the following ions Ca2+, NO3 -, Na+ and SO4 2- are placed in a test tube, the precipitate formed is A) NaNO3 B) CaSO4 C) Ca(NO3)2 D) Na2SO4 47) 48) If the following ions Ba2+, Cl-, K+ and SO4 2- are placed in a test tube, the precipitate formed is A) BaSO4 B) KCl C) BaCl2 D) K2SO4 48) 49) If the following ions Ca2+, Cl-, Na+ and CO3 2- are placed in a test tube, the precipitate formed is A) CaCO3 B) NaCl C) CaCl2 D) No precipitate will be formed. 49) 50) The precipitate formed when sodium chloride and lead (II) nitrate are placed in a test tube is A) lead (II) chloride B) sodium nitrate C) lead (II) hydroxide D) No precipitate will be formed. 51) The precipitate formed when barium nitrate and potassium chromate are placed in a test tube is A) barium nitrate B) barium chromate C) potassium nitrate D) potassium chromate 52) The precipitate formed when hydrochloric acid and sodium hydroxide are placed in a test tube is A) sodium hydroxide B) sodium chloride C) hydrochloric acid D) No precipitate will be formed. 53) The net ionic equation for the following reaction is H2SO4 + KOH K2SO4 + H2O A) K+ (aq) + SO4 2- (aq) K2SO4 B) H+ (aq) + OH- (aq) H2O C) K+ (aq) + OH-(aq) KOH D) H+ (aq) + SO4 2- (aq) H2SO4 50) 51) 52) 53) 5

6 54) It takes mole(s) of potassium hydroxide to neutralize moles of sulfuric acid. 54) A) 1; 1 B) 1; 2 C) 2; 1 D) 3; 1 55) It takes mole(s)of calcium hydroxide to neutralize moles of sulfuric acid. 55) A) 1; 1 B) 1; 2 C) 2; 1 D) 1; 3 56) It takes mole(s) of sulfuric acid to neutralize moles of aluminum hydroxide. 56) A) 2; 3 B) 3; 2 C) 1; 2 D) 1; 1 57) The number of moles of sodium hydroxide needed to neutralize one mole of nitric acid is 57) A) 1 B) 2 C) 3 D) ) What is the mass in grams of mole of P2O5? 58) A) g B) g C) g D) g 59) What is the mass in grams of mole of a compound whose formula is C3H7O2? 59) A) g B) g C) g D) g 60) Which of the following has the least number of atoms? 60) A) (NH4)3PO4 B) Na2P2O3 C) (NH4)2Cr2O7 D) K4Fe(CNO)6 61) Which of the following has the greatest number of atoms? 61) A) (NH4)3PO4 B) Na2P2O3 C) (NH4)2Cr2O7 D) K4Fe(CNO)6 62) The correct sequence of decreasing number of atoms per formula unit in the following is 62) A) (NH4)3PO4 > Na2P2O3 > Na3PO4 B) Na3PO4 > (NH4)3PO4 > Na2P2O3 C) Na2P2O3 > Na3PO4 > (NH4)3PO4 D) (NH4)3PO4 > Na3PO4 > Na2P2O3 63) The number of oxygen atoms in 1 mole of Al2(SO4)3 is 63) A) 3 B) 4 C) 12 D) none of the above 64) The molar mass of Ca3(PO4)2 is 64) A) 310 B) 279 C) 246 D) ) The molar mass for Pb(CO3)4 is 65) A) 447 B) 409 C) 327 D) ) Which of the following has a molar mass equal to 133? 66) A) (NH4)3PO3 B) Ca3(PO4)2 C) Al2(SO3)3 D) Co2(CO3)2 67) Which of the following has the highest molar mass? 67) A) (NH4)3PO3 B) Ca3(PO4)2 C) Al2(SO3)3 D) Co2(CO3)2 6

7 68) Which of the following pairs does not share the same molecular mass when rounded to the nearest whole number? A) CH3OH and oxygen gas B) CO and nitrogen gas C) C2H6O and C2H4O2 D) C4H10O and C3H6O2 68) 69) The molar mass of a compound XClO3 is The molar mass (rounded to the nearest whole number) of X is, which is A) 39; K B) 23; Na C) 7; Li D) 1; H 70) The molar mass of a compound X(HCO3)2 is 146. The atomic weight of X when rounded to the nearest whole number is, which is A) 24; Mg B) 40; Ca C) 51; V D) 56; Fe 71) The molecular mass of a compound X(NO3)3 is 213. The atomic mass of X is, which is A) 27; Al B) 51; V C) 56; Fe D) 59; Co 72) The molar mass of a compound Ca(MO3)2 is 160. The atomic mass of M is, which is A) 12; C B) 14; N C) 32; S D) 35; Cl 73) The molar mass of a compound Al2(XO4)3 is 342. The atomic mass of X is, which is A) 31; P B) 32; S C) 52; Cr D) 55; Mn 74) Alkanes have the general molecular formula CnH2n+2. Thus, when n = 1, the alkane is CH4, when n = 2, the alkane is C2H6 etc. If an alkane has a molar mass between 140 and 150, this alkane is A) C9H20 B) C12H26 C) C10H22 D) C11H24 69) 70) 71) 72) 73) 74) 75) Alkenes have the general molecular formula CnH2n. Thus, when n = 2, the alkene is C2H4. If an alkene has a molecular mass between 65 and 75, this alkene is A) C5H12 B) C5H10 C) C6H3 D) C6H12 75) 76) Alkynes have the general molecular formula CnH2n-2. Thus, when n = 2, the alkyne is C2H2 etc. If an alkyne has a molecular mass between 75 and 85, this alkyne is A) C6H10 B) C6H12 C) C5H16 D) C7H12 76) 77) Which of the following quantities does not share the same molar mass as the others when rounded to the nearest whole number? A) Al2(SO4)3 B) C12H22O11 C) C24H38O D) Pb3(PO4)4 77) 78) Which of the following contains the least number of atoms? 78) A) 1.0 mole C6H14 B) 3.0 moles N2O5 C) 12.0 moles silver D) 3.0 moles water 7

8 79) Which of the following contains the greatest number of atoms? 79) A) 1.0 mole C6H14 B) 3.0 moles N2O5 C) 12.0 moles silver D) 3.0 moles water 80) 12 g of carbon is equal to 80) A) the mass of one atom B) the mass of one molecule C) the mass of one mole D) the mass of half a mole 81) 16 g of oxygen gas is equal to 81) A) the mass of one atom B) the mass of one molecule C) the mass of one mole D) the mass of half a mole 82) A sample of calcium that contains Avogadro's number of atoms has a mass of 82) A) 20 g B) 40 g C) 80 g D) 160 g 83) A sample of calcium that contains one-half Avogadro's number of atoms has a mass of 83) A) 20 g B) 40 g C) 80 g D) 160 g 84) A sample of calcium that contains four times Avogadro's number of atoms has a mass of 84) A) 20 g B) 40 g C) 80 g D) 160 g 85) A sample of calcium that contains twice Avogadro's number of atoms has a mass of 85) A) 20 g B) 40 g C) 80 g D) 160 g 86) A sample of oxygen gas that contains Avogadro's number of molecules has a mass of 86) A) 8.0 g B) 16.0 g C) 32.0 g D) 64.0 g 87) A sample of oxygen gas that contains Avogadro's number of atoms has a mass of 87) A) 8.0 g B) 16.0 g C) 32.0 g D) 64.0 g 88) A sample of oxygen gas that contains one-half of Avogadro's number of molecules has a mass of A) 8.0 g B) 16.0 g C) 32.0 g D) 64.0 g 89) A sample of oxygen gas that contains twice Avogadro's number of molecules has a mass of A) 8.0 g B) 16.0 g C) 32.0 g D) 64.0 g 88) 89) 90) A sample of methane gas that contains Avogadro's number of molecules has a mass of 90) A) 8.0 g B) 16.0 g C) 32.0 g D) 64.0 g 91) A sample of methane gas that contains Avogadro's number of atoms has a mass of 91) A) 3.2 g B) 6.4 g C) 16.0 g D) 80.0 g 92) Which of the following does not have the same number atoms as the other three choices? 92) A) three moles Na2SO3 B) six moles of water C) nine moles NaCl D) five moles CH4 8

9 93) What is the mass of moles aluminum sulfate? 93) A) 6.15 g B) g C) 17.1 g D) 19.8 g 94) What is the molar mass of a compound X if moles weigh 21.6 g? 94) A) 540 B) 185 C) 216 D) ) 0.3 moles of a certain calcium compound weigh 93 g. This compound may be 95) A) calcium nitrate B) calcium chromate C) calcium phosphate D) calcium sulfate 96) 0.02 moles of a certain aluminum compound has a mass of 1.56 g. This compound may be A) aluminum hydroxide B) aluminum nitrate C) aluminum cyanide D) aluminum permanganate 96) 97) 0.05 moles of a certain compound has a mass of 17.1 g. This compound may be 97) A) aluminum sulfate B) lead (II) chloride C) cobalt (III) oxide D) magnesium carbonate 98) Which of the following will not have the same number atoms as the other three choices? 98) A) K2Cr2O7 B) (NH4)2S C) Al(ClO2)3 D) Ba(HCO3)2 99) Which of the following has 14 atoms per formula unit? 99) A) (NH4)2SO3 B) Al(ClO4)3 C) Pb(CrO4)2 D) Mg3(PO4)2 100) The number of atoms in 2.4 g of magnesium metal is 100) A) B) C) D) ) A certain food contains 60 mg of table salt. This is approximately equal to formula units. 101) A) B) C) D) ) The number of oxygen atoms present in 32.4 g of N2O5 is 102) A) 5.00 B) C) D) ) Which is the correct statement about one mole of ammonia, NH3? 103) A) It contains 14 g nitrogen and 3 g hydrogen. B) It contains molecules. C) It contains atoms of hydrogen. D) all of the above 104) The number of phosphorus atoms in one molecule of H3PO4 is 104) A) 1 B) 8 C) D) ) The total number of atoms in two moles SO3 is 105) A) 4 B) 8 C) D)

10 106) The mass of one formula unit of Al2(SO4)3 is g. 106) A) 342 B) C) D) ) Which of the following does not contain atoms? 107) A) 60 g of carbon B) one mole of methane C) two moles of water D) 160 g sulfur 108) Which contains more carbon? 108) A) 24 g methane B) 140 g sodium carbonate C) 40 g carbon monoxide D) 15 g octane, C8H18 109) One molecule of water contains 109) A) one mole of hydrogen B) one mole of oxygen C) one atom of oxygen D) 16 g of oxygen 110) The ingredients to make 50 servings of fruit punch are: 2-1/2 cups white sugar 6 cups water 2 (3-ounce) packages strawberry flavored gelatin mix 1 (46-fluid-ounce) can pineapple juice 2/3 cup lemon juice 1 quart orange juice 2 (2-liter) bottles lemon-lime flavored carbonated beverage How many servings of punch can you make using the above recipe, if you have 2 gallons of pineapple juice, 8 (2-liter) bottles of lemon-lime flavored soda and 2 gallons of orange juice? Assume you have plenty of all the other ingredients. A) 125 servings B) 200 servings C) 278 servings D) 375 servings E) 400 servings 110) 111) The mass of CaCl2 that contains 17.8 g of chlorine is 111) A) 35.6 g B) 53.4 g C) 27.9 g D) 20.5 g 112) The number of moles of chlorine atoms in 12.5 g of carbon tetrachloride is 112) A) B) C) D) ) The mass of oxygen present in 11.7 g of Al2(CO3)3 is 113) A) 7.20 g B) 14.4 g C) 8.10 g D) 4.05 g 114) Which has more ions 2.0 moles of Al2(SO4)3 or 3.0 moles of Na3PO4? 114) A) 2.0 moles of Al2(SO4)3 B) 3.0 moles of Na3PO4 C) There are equal number of ions in both ionic compounds. D) It cannot be determined based on the information given. 115) moles of an element has a mass of 2.56 g. This element is 115) A) Pb B) V C) Ac D) Th 10

11 116) What is the mass of hydrogen that will react with g of Li to form LiH? 116) A) g B) g C) g D) g 117) What is the mass of sulfur that will react with g of copper metal to yield copper (I) sulfide? 117) A) g B) g C) g D) g 118) g chlorine will combine with g of sulfur to produce SCl2. 118) A) B) C) D) ) Two moles of hydrogen react with excess nitrogen to produce moles of ammonia.. N2 + 3 H2 2 NH3 A) 1.3 B) 2.0 C) 1.0 D) ) If 4 moles of nitrogen produces 2 moles of nitrogen dioxide, then the percent yield is N2 + 2 O2 2 NO2 A) 100% B) 50% C) 25% D) 12.5% 121) If 14 kg of nitrogen yields 23 kg of nitrogen dioxide, then the percent yield for the reaction is N2 + 2 O2 2 NO2 A) 100% B) 50% C) 25% D) 12% 122) The maximum number of moles of water that can be produced from 0.5 moles of C3H8O is 2 C3H8O + 9 O2 6 CO2 + 8 H2O A) 0.5 B) 2 C) 4 D) 8 123) If 5.0 moles of ammonia is produced, then the number of hydrogen molecules consumed is N2 + 3 H2 2 NH3 A) 5.0 B) 7.5 C) 3.2 D) ) What is the percent yield for a given process, if 4.0 kg of a product is recovered from a reaction whose theoretical yield is 5.6 kg? A) 41% B) 62% C) 71% D) 89% 125) The balanced equation involves the corresponding coefficients NaHCO3 Na2CO3 + CO2 + H2O A) 1: 1: 1: 1 B) 1: 2: 1: 1 C) 2: 1: 1: 1 D) 2: 1: 2: 1 126) The balanced equation involves the corresponding coefficients H2SO4 + Cu SO2 + H2O + CuSO4 A) 2: 1: 1: 2: 1 B) 1: 1: 2: 2: 1 C) 2: 1: 2: 1: 1 D) 2: 1: 1: 2: 2 127) The balanced equation involves the corresponding coefficients NH3 + O2 NO + H2O A) 2: 3: 2: 3 B) 2: 5: 2: 3 C) 4: 5: 4: 6 D) 2: 2: 3: 3 119) 120) 121) 122) 123) 124) 125) 126) 127) 11

12 128) The balanced equation involves the corresponding coefficients C2H6O + O2 CO2 + H2O A) 1: 2: 2: 3 B) 1: 3: 2: 3 C) 2: 7: 4: 6 D) 2: 9: 4: 6 129) The balanced equation involves the corresponding coefficients C6H14 + O2 CO2 + H2O A) 1: 9: 6: 7 B) 1: 10: 6: 7 C) 2: 19: 12:14 D) 2: 21: 6: 7 130) The balanced equation involves the corresponding coefficients NaN3 Na + N2 A) 2: 2: 3 B) 1: 2: 3 C) 2: 1: 3 D) 3: 3: 2 131) The maximum number of moles of carbon dioxide that can be produced from four moles of C3H8O is 2 C3H8O + 9 O2 6 CO2 + 8 H2O A) 4 B) 6 C) 8 D) ) Which reactant is present in excess if 10.0 g of CaO react with 3.0 mol of H2O? CaO + H2O Ca(OH)2 A) Ca(OH)2 B) CaO C) H2O D) None of the above, the amounts exactly balance. 133) Which of the following abides by the principle of mass conservation according to the balanced reaction? 4 K + O2 2 K2O A) 39.0g K g O2 94.0g K2O B) g K g O g K2O C) 156.0g K g O g K2O D) 78.0g K g O g K2O 128) 129) 130) 131) 132) 133) 134) The theoretical number of carbon dioxide moles produced from 3 moles of C2H6O is C2H6O + O2 CO2 + H2O A) 3 B) 4 C) 6 D) 9 135) The theoretical number of carbon dioxide moles produced from 6 moles of NaHCO3 is ' NaHCO3 Na2CO3 + CO2 + H2O A) 1 B) 3 C) 6 D) ) The theoretical number of moles of water produced from 8 moles of NaHCO3 is NaHCO3 Na2CO3 + CO2 + H2O A) 2 B) 4 C) 8 D) ) What is the theoretical mass of carbon dioxide produced from 4.0 moles of NaHCO3? NaHCO3 Na2CO3 + CO2 + H2O A) 1.0 g B) 22 g C) 44 g D) 88 g 134) 135) 136) 137) 12

13 138) What is the theoretical mass of water produced from 10 moles of NaHCO3? NaHCO3 Na2CO3 + CO2 + H2O A) 180 g B) 90 g C) 45 g D) 18 g 139) Determine the percent yield of an experiment in which 1.00 mole of NaHCO3 was consumed and 22.0 g of carbon dioxide was isolated. NaHCO3 Na2CO3 + CO2 + H2O A) 100.% B) 50.0% C) 37.5% D) 25% 140) The theoretical number of moles of water produced from 2 moles of C2H6O is C2H6O + O2 CO2 + H2O A) 2 B) 3 C) 6 D) 9 141) What is the theoretical mass of carbon dioxide produced from one mole of C2H6O? C2H6O + O2 CO2 + H2O A) 6 g B) 44 g C) 88 g D) 176 g 142) Determine the percent yield of an experiment in which 1 mole of C2H6O was consumed and 22 g of carbon dioxide was isolated. C2H6O + O2 CO2 + H2O A) 100% B) 50% C) 37.5% D) 25% 143) The theoretical number of moles of carbon dioxide produced from 3.0 moles of C6H14 is C6H14 + O2 CO2 + H2O A) 3.0 B) 6.0 C) 9.0 D) ) The theoretical number of water moles produced from two moles of C6H14 is C6H14 + O2 CO2 + H2O A) 1 B) 6 C) 7 D) ) What is the theoretical mass of carbon dioxide produced from one mole of C6H14? C6H14 + O2 CO2 + H2O A) 6 g B) 44 g C) 132 g D) 264 g 146) The % yield of an experiment in which 1.0 mole of C6H14 was used and 22 g of carbon dioxide was isolated is C6H14 + O2 CO2 + H2O A) 100% B) 50% C) 17.5% D) 8.3% 147) The theoretical number of moles of sodium produced from 4 moles of NaN3 is NaN3 Na + N2 A) 1 B) 2 C) 4 D) 8 148) The theoretical number of moles of nitrogen produced from 6 moles of NaN3 is NaN3 Na + N2 A) 2 B) 6 C) 9 D) ) 139) 140) 141) 142) 143) 144) 145) 146) 147) 148) 13

14 149) The theoretical mass of sodium produced from 2.0 moles of NaN3 is NaN3 Na + N2 A) 11.5 g B) 23 g C) 34.5 g D) 46 g 150) The percent yield of an experiment in which 2.0 moles of NaN3 was used and 21 g of nitrogen was isolated is NaN3 Na + N2 A) 100% B) 50% C) 37.5% D) 25% 151) The minimum number of moles of oxygen needed to completely consume 4 moles of C3H8O is 2 C3H8O + 9 O2 6 CO2 + 8 H2O A) 4 B) 9 C) 13.5 D) ) The theoretical yield of water produced from of 2.0 moles of C3H8O is g. 2 C3H8O + 9 O2 6 CO2 + 8 H2O A) 8 B) 18 C) 36 D) ) If 36 g of water are produced from two moles of C3H8O, the percent yield of the reaction is 2 C3H8O + 9 O2 6 CO2 + 8 H2O A) 100% B) 50% C) 25% D) 10% 154) The theoretical number of moles of copper that will react with 4 moles of sulfuric acid is H2SO4 + Cu SO2 + H2O + CuSO4 A) 2 B) 4 C) 6 D) 8 155) The theoretical number of moles of sulfur dioxide produced from 4 moles of sulfuric acid is H2SO4 + Cu SO2 + H2O + CuSO4 A) 2 B) 4 C) 6 D) 8 156) The theoretical number of moles of water produced from 4 moles of sulfuric acid is H2SO4 + Cu SO2 + H2O + CuSO4 A) 2 B) 4 C) 6 D) 8 157) The theoretical mass of sulfur dioxide produced from 2.0 moles of sulfuric acid is H2SO4 + Cu SO2 + H2O + CuSO4 A) 8.0 g B) 16.0 g C) 32.0 g D) 64.1 g 158) The percent yield of an experiment in which 2.0 moles of copper was used and 18 g of water was isolated is H2SO4 + Cu SO2 + H2O + CuSO4 A) 100% B) 50% C) 37.5% D) 25% 159) How many grams of oxygen will react with 20 g of ammonia? NH3 + O2 NO + H2O A) 71 g B) 94 g C) 24 g D) 47 g 149) 150) 151) 152) 153) 154) 155) 156) 157) 158) 159) 14

15 160) How many grams of NO will form when 40 g of oxygen are used? NH3 + O2 NO + H2O A) 30 g B) 15 g C) 45 g D) 60 g 161) How many grams of ammonia are consumed if 45.0 g of NO are formed in a 100% yield? NH3 + O2 NO + H2O A) 6.51 g B) 13.0 g C) 26.0 g D) 39.0 g 162) What is the percent yield if 52 g of ammonia produce 45 g of NO? NH3 + O2 NO + H2O A) 100% B) 49% C) 25% D) 18% 163) What is the mass of NO expected if 104 g of ammonia are consumed in a 100% yield? NH3 + O2 NO + H2O A) 45.7 g B) 91.5 g C) 183 g D) 366 g 164) 14 g of nitrogen will react with g of oxygen. N2 + 2 O2 2 NO2 A) 8 B) 16 C) 32 D) ) 14 g of nitrogen will yield g of nitrogen dioxide. N2 + 2 O2 2 NO2 A) 23 B) 46 C) 92 D) ) 64 g of oxygen will yield g of nitrogen dioxide. N2 + 2 O2 2 NO2 A) 23 B) 46 C) 92 D) ) The maximum amount of IF7 that can be obtained from 25.0 g is fluorine is I2 + F2 IF7 A) 63 g B) 48.9 g C) 24.5 g D) 12.3 g 168) How many moles of aluminum chloride can be obtained from 4.5 moles of aluminum and excess chlorine? Al + Cl2 AlCl3 A) 1.5 B) 3.0 C) 4.5 D) ) Which reactant is the limiting reagent if 6 mol of H2 and 4 mol of O2 are used? 2H2 + O2 2H2O A) O2 B) H2 C) neither H2 nor O2 D) both H2 and O2 160) 161) 162) 163) 164) 165) 166) 167) 168) 169) 170) Which reagent will be used up first if 78.1 g of O2 is reacted with 62.4 g of C4H10? 2 C4H O2 8 CO H2O A) C4H10, butane B) oxygen C) water D) carbon dioxide 170) 15

16 171) How many grams of CO2 can be made from reacting 78.1 g of O2 and 62.4 g of C4H10? 2 C4H O2 8 CO H2O A) 66.1 g CO2 B) 141 g CO2 C) 189 g CO2 D) 378 g CO2 E) 430 g CO2 171) 172) The reaction was performed in the lab and 50.1 g of CO2 was collected from the reaction of 78.1 g of O2 with 62.4 g of C4H10. The percent yield of this reaction is 2 C4H O2 8 CO H2O A) 11.7 % B) 13.3 % C) 26.5 % D) 35.7 % E) 75.8 % 173) The reaction was performed in the lab and 50.1 g of CO2 was collected from the reaction of 78.1 g of O2 with 62.4 g of C4H10. How many grams of the excess reactant are left over. 2 C4H O2 8 CO H2O A) 15.7 g B) 21.8 g C) 28.0 g D) 40.6 g E) 45.8 g 172) 173) 174) Which statement is true about the empirical formula? 174) A) The empirical formula is always different than the molecular formula. B) The empirical formula is always the same as the molecular formula. C) The empirical formula may be different than the molecular formula. D) The empirical formula cannot be determined solely by the % composition. 175) Which statement is true about the molecular formula? 175) A) The molecular formula is always different than the empirical formula. B) The molecular formula is always the same as the empirical formula. C) The empirical formula may be different than the molecular formula. D) The empirical formula can be determined solely by the % composition. 176) Which statement is true when comparing acetic acid C2H4O2 and formaldehyde CH2O? 176) A) Their empirical formulas are identical. B) Their molecular formulas are identical. C) Their molecular formulas are different. D) both A and C 177) If the empirical formula of a compound is CH2O and the molecular weight is 180, the molecular formula is A) CH2O B) C2H4O2 C) C3H6O3 D) C6H12O6 177) 178) Which of the following has its empirical formula different than its molecular formula? 178) A) CH2S B) C2H7N3 C) C3H6N3 D) C5H7O3 179) Which of the following pairs does not share the same empirical formula? 179) A) CH2O and C3H6O3 B) C6H6 and C2H2 C) C2H6O and CH3O D) C3H4Br2 and C9H12O6 180) Which of the following does not share the same empirical formula as the other three? 180) A) CH2O B) C6H12O6 C) C8H16O8 D) C12H22O11 16

17 181) What is the empirical formula of C8H6O3? 181) A) CHO B) C4H3O C) C4H3O2 D) C8H6O3 182) A certain compound has the following composition: C= 40.0% and H= 6.7%. The empirical formula is A) CH B) CH2O C) C6H6O D) CHO 182) 183) An independent experiment showed that the molecular weight of isopropyl alcohol is approximately 62. The molecular formula therefore is A) C2H6O2 B) C3H8O2 C) C3H8O D) C3H10O2 183) 184) 5.82 g isopropyl alcohol yield g of water and 12.6 g of carbon dioxide upon combustion. The empirical formula is A) CH2O B) C3H8O C) C2H6O D) C3H9O 184) 185) Combustion of 6.51 mg of a compound produces mg of carbon dioxide and 8.36 mg of water. The empirical formula is A) CH2O B) C2H3 C) C2H3O D) CH2 185) 186) Combustion of 5.00 mg of a compound produces 15.2 mg of carbon dioxide and 7.80 mg of water. The empirical formula is A) CH2 B) C2H5 C) C3H7 D) C4H10 186) 187) Combustion of 5.00 mg of a compound produces 9.60 mg of carbon dioxide and 5.90 mg of water. The empirical formula is A) CH2O B) C2H5 C) C2H6O D) C4H10O 187) 188) What is the molecular formula of a compound that weighs 46 g/mol and analyzes to 52.2% C, 34.8% O, and 13% H? A) C3H2O2 B) C2H6O C) CH3O D) C2H5O2 188) 189) A compound is found to be 43.7% phosphorus and 56.3% oxygen. Given the molecular mass as 285 ± 10, calculate the empirical and molecular formulas. A) PO2; P4O8 B) P2O5; P4O10 C) P2O3; P6O9 D) P4O10; P4O10 189) 190) A sample is composed of 2.78 g of iron and 1.19 g of oxygen. The empirical formula is 190) A) FeO2 B) Fe2O5 C) Fe2O3 D) FeO 191) Which compound has the percent composition of 15.8% Al, 28.1% S and 56.1% O? 191) A) Al2(SO4)3 B) Al2(SO3)3 C) Al2S3 D) Al2(S2O3)3 192) A chromium-silicon compound contains 73.52% chromium. The empirical formula is 192) A) CrSi B) CrSi2 C) Cr2Si D) Cr3Si2 193) An iron oxide is 72.4% in iron. Its empirical formula is 193) A) FeO B) Fe2O C) Fe2O3 D) Fe3O4 17

18 194) An iron oxide is 77.7% in iron. Its empirical formula is 194) A) FeO B) Fe2O C) Fe2O3 D) Fe3O4 195) An iron oxide is 70.0% in iron. Its empirical formula is 195) A) FeO B) Fe2O C) Fe2O3 D) Fe3O4 196) Which of the following compounds is expected to have oxygen? 196) A) compound W: %C= 40.2% ; H= 6.8%; N= 10.3%; S= 19.2% B) compound X: %C= 52.3% ; H= 4.1%; Br= 30.4%; S= 13.2% C) compound Y: %C= 25.6% ; H= 8.8%; I= 45.3%; N= 20.2% D) compound Z: %C= 48.1% ; H= 8.6%; F= 28.2%; P= 15.0% 197) A certain compound is found to contain 1.45 g of Na, 2.05 g of S and 1.5 g of O. Its empirical formula is A) Na2SO B) NaS2O C) Na2S2O3 D) NaSO2 197) 198) g of bromine combine with g of iodine to yield a compound X. The empirical formula of the compound described above is A) Br2I B) BrI2 C) Br2I3 D) BrI 198) 199) A compound has the following elemental composition: C = 58.8%, H= 13.8%, N = 27.4%. The empirical formula of this compound is A) C5H14N B) C5H10N2 C) C5H14N2 D) C5H15N2 199) 200) The empirical formula for a compound that is 48.7% C, 13.6% H and 37.8% N is 200) A) C4H9N2 B) C3H8N C) C3H10N2 D) C4H10N 201) If the empirical formula is CH2, and the molecular weight is equal to 180 ±10, then the molecular formula is A) C6H12O6 B) C14H21 C) C8H12O4 D) C13H26 201) 202) Hydrazine contains 87.5% nitrogen and 12.5% hydrogen. If the molecular mass is 32 ± 6, the molecular formula is A) N2H B) N2H2 C) N2H3 D) N2H4 202) 203) A g sample of a certain cobalt oxide contains g of cobalt. The empirical formula is A) CoO B) CoO2 C) Co2O D) Co3O4 203) 204) A selenium-chlorine compound is 35.7% in selenium. Its empirical formula is 204) A) SeCl B) SeCl2 C) SeCl3 D) SeCl4 205) 0.68 g of sulfur combine with 1.51 g of chlorine. The empirical formula of this compound is A) SCl B) SCl2 C) SCl4 D) SCl6 205) 206) The element in C7H5NO3 whose % composition is 31.8% is 206) A) carbon B) hydrogen C) nitrogen D) oxygen 18

19 207) What is the percentage by mass of iron (Fe) in the mineral hematite (Fe2O3)? 207) A) 40% B) 60% C) 70% D) 30% 208) What is the percentage by mass of hydrogen in ordinary water (H2O)? 208) A) 20% B) 11% C) 60% D) 40% 209) Methanol (CH4O) weighs 32 g/mol. What is the mass percentage of carbon in methanol? 209) A) 63% B) 50% C) 20% D) 38% 210) Ilmenite (FeTiO3) is the primary ore from which the element titanium (Ti) is isolated. What is the percentage of titanium by mass in this mineral? A) 20% B) 32% C) 80% D) 68% 210) 211) Which contains the highest percentage of oxygen? 211) A) H2O2 B) Na2O2 C) HgO D) CO2 212) Which contains the least percentage of oxygen? 212) A) H2O2 B) Na2O2 C) HgO D) CO2 213) Which contains the highest percentage of hydrogen? 213) A) HCl B) H2SO4 C) H3PO4 D) H2O 214) Which contains the lowest percentage of hydrogen? 214) A) HCl B) H2SO4 C) H3PO4 D) H2O 215) Which of the following compounds has its carbon composition equal to 52.1%? 215) A) C2H6O B) CH3Cl C) C4H8O2N2S D) C10H20O4N2S 216) Which of the following compounds has its hydrogen composition equal to 2.4%? 216) A) C4H7Cl B) CH2Cl2 C) C2H3NO2 D) C10H20ONS 217) Which of the following compounds has its oxygen composition equal to 50.0%? 217) A) (NH4)2CO3 B) CH2O2 C) C2H3NO2 D) C10H20ONS 218) Which of the following compounds has its nitrogen composition equal to 29.2%? 218) A) C2H3NO2 B) C10H20ONS C) (NH4)2CO3 D) N2H4 219) Which of the following compounds has its chlorine composition equal to 83.5%? 219) A) C2H3ClO2 B) C10H17ClS C) CCl4 D) CH2Cl2 220) Which of the following compounds has its sulfur composition equal to 18.6%? 220) A) C6H8SO2N2 B) C7H14S C) CH2SO2 D) COS 221) Which of the following compounds has its combined carbon and hydrogen composition equal to 37.0%? A) C4H7Cl B) CH2O2 C) C2H3NO2 D) C10H20ONS 221) 19

20 222) Which of the following compounds has its combined carbon and oxygen composition equal to 76.7%? A) C4H7Cl B) CH2O2 C) C2H3NO2 D) C10H20ONS 222) 223) Which of the following has the highest percent of oxygen? 223) A) N2O B) Al2O3 C) K2CO3 D) KMnO4 224) Which of the following has the lowest percent of oxygen? 224) A) N2O B) Al2O3 C) K2CO3 D) KMnO4 225) Which of the following percent compositions does not correspond to one of the elements of NaNO3? A) 56.4% B) 19.4% C) 16.5 % D) 27.1% 226) Which of the following percentage compositions does not correspond to one of the elements of C6H12O6? A) 43.4% B) 40.0% C) 6.7% D) 53.3% 227) Which of the following percentage compositions does not correspond to one of the elements of C9H8O4? A) 4% B) 26% C) 36% D) 60% 228) g of bromine combine with g of iodine to yield a compound X. Its percent composition is A) Br = 38.6%, I = 61.4% B) Br = 61.3%, I = 38.6% C) Br = 32.8%, I = 67.2% D) Br = 67.2%, I = 32.8% 225) 226) 227) 228) 229) What is the mass percent of Sn in tin (IV) oxide? 229) A) 26.96% B) 64.97% C) 78.77% D) 93.69% E) 96.73% 230) What is the molarity of 3.68 ml of a solution containing moles of calcium chloride? 230) A) M B) 0.68 M C) 1.5 M D) M 231) The molarity of a solution that contains 5.85 g of NaCl in 2.0 L of solution is 231) A) 2.93 M B) M C) 5.0 M D) 0.29 M 232) To prepare 100 ml of 0.4 M HCl solution from a stock solution of 2 M HCl solution one needs to A) dilute 20 ml of 2 M HCl solution with 100 ml of HCl solution. B) dilute 20 ml of 2 M HCl solution with enough water to make a total volume of 100 ml of solution. C) use 500 ml of 2 M HCl solution and boil it down to a final volume of 100 ml of solution. D) dilute 80 ml of 2 M HCl solution to a total volume of 100 ml of solution. 232) 233) To prepare 500. ml of 0.5 M NaCl from a stock of 2.0 M NaCl one needs to 233) A) dilute 125 ml 2.0 M NaCl with enough water to a total of 500. ml solution B) dilute 125 ml 2.0 M NaCl with 500. ml water C) dilute 375 ml 2.0 M NaCl with enough water to a total of 500. ml solution D) dilute 375 ml 2.0 M NaCl with 500. ml water 20

21 234) 25 ml of a 0.1 M NaCl solution contains g of NaCl. 234) A) B) 0.15 C) 2.5 D) ) 7.5 g of calcium carbonate in 150 ml of aqueous solution will provide a M solution. A) 0.10 B) 0.50 C) 1.0 D) ) 236) 200. ml of a M NaCl solution contains g of NaCl. 236) A) 1.17 B) 11.7 C) 117 D) ) 500 ml of a 0.4 M sodium nitrate contains moles of sodium ions and moles of nitrate ions. A) 0.4; 0.2 B) 0.2; 0.4 C) 0.4; 0.6 D) 0.2; ) 500 ml of a 0.4 M calcium nitrite contains moles of calcium ions and moles of nitrite ions. A) 0.4; 0.2 B) 0.2; 0.4 C) 0.4; 0.6 D) 0.2; ) 500 ml of a 0.4 M potassium dichromate contains moles of potassium ions and moles of dichromate ions. A) 0.4; 0.2 B) 0.2; 0.4 C) 0.4; 0.6 D) 0.2; ) 500 ml 0.4 M aluminum nitrate solution contains moles of aluminum ions and moles of nitrate ions. A) 0.6; 0.2 B) 0.2; 0.4 C) 0.2; 0.6 D) 0.2; ) 238) 239) 240) 241) 10.0 ml of 0.50 M HCl solution neutralizes ml of 0.50 M NaOH solution. 241) A) 5.0 B) 10. C) 20. D) ) 10.0 ml of 0.50 M sulfuric acid neutralizes ml of 0.50 M ammonium hydroxide solution. 242) A) 5.0 B) 10. C) 20. D) ) 10.0 ml of 0.50 M sulfuric acid neutralizes ml of 0.50 M magnesium hydroxide solution. 243) A) 5.0 B) 10. C) 20. D) ) 10.0 ml of 0.50 M hydrochloric acid neutralizes ml of 0.50 M magnesium hydroxide solution. A) 5.0 B) 10. C) 20. D) ) 245) The percent composition of a solution made by dissolving 5.0 g NaOH in 20. g of water is 245) A) 4.0% B) 5.0% C) 20.% D) 25% 246) How many grams of NaCl are in 200 g of a 10 percent-by-mass salt solution? 246) A) 10 g B) 20 g C) 40 g D) 80 g 247) How many grams of water are in 100 g of a 30 percent-by-mass sugar solution? 247) A) 30 g B) 60 g C) 70 g D) 100 g 21

22 248) Which solution is the most basic solution? 248) A) a solution whose [H+] = 100 B) a solution whose [OH-] = C) a solution whose ph = 0 D) All of the above have the same degree of basicity. 249) Which solution is the most acidic solution? 249) A) a solution whose [H+] = 10-1 B) a solution whose [OH-] = C) a solution whose ph = 0 D) All of the above have the same degree of acidity. 250) What is the hydrogen-ion concentration of an aqueous solution having a ph of 4.72? 250) A) mol/l B) 4.72 mol/l C) 0.67 mol/l D) mol/l 251) What is the hydroxide-ion concentration of an aqueous solution having a ph of 4.72? 251) A) mol/l B) mol/l C) mol/l D) mol/l 252) What is the ph of an aqueous solution having a hydrogen-ion concentration of mol/l? 252) A) 6.83 B) 0.83 C) 2.17 D) ) What is the poh of an aqueous solution having a hydrogen-ion concentration of mol/l? A) B) C) 2.17 D) ) The ph of an aqueous solution is What is the poh? (ph + poh = 14 for aqueous acid/base systems). A) 4.65 B) C) D) ) 254) 255) The ph of blood is approximately 255) A) 5.2 B) 7.0 C) 7.4 D) ) The ph of diabetic patients can be as low as 256) A) 3.2 B) 5.8 C) 6.8 D) ) A drop of a full unit in the ph scale 257) A) reduces the acidity 10 B) increases the acidity 10 C) reduces the acidity 2 D) increases the acidity 2 258) A change in ph from 10 to 7 258) A) increases the acidity 1000 B) reduces the acidity 3000 C) increases the acidity 3 D) increases the acidity ) The ph of natural rainwater is close to 259) A) 5.6 B) 6.3 C) 7.0 D)

23 260) Stomach juices have a ph close to 260) A) 1.5 B) 2.8 C) 4.5 D)

24 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 1) D 2) B 3) D 4) A 5) D 6) D 7) A 8) C 9) D 10) C 11) B 12) A 13) D 14) C 15) C 16) C 17) B 18) C 19) A 20) B 21) D 22) C 23) D 24) D 25) B 26) C 27) B 28) B 29) D 30) C 31) D 32) C 33) C 34) B 35) B 36) C 37) A 38) A 39) D 40) C 41) B 42) A 43) D 44) A 45) C 46) B 47) B 48) A 49) A 50) A 24

25 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 51) B 52) D 53) B 54) C 55) A 56) B 57) A 58) C 59) D 60) B 61) D 62) D 63) D 64) A 65) A 66) A 67) C 68) C 69) B 70) A 71) A 72) A 73) B 74) C 75) B 76) A 77) D 78) D 79) B 80) C 81) D 82) B 83) A 84) D 85) C 86) C 87) B 88) B 89) D 90) B 91) A 92) D 93) C 94) A 95) C 96) A 97) A 98) C 99) A 100) A 25

26 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 101) C 102) B 103) D 104) A 105) D 106) C 107) C 108) A 109) C 110) B 111) C 112) C 113) A 114) B 115) D 116) B 117) B 118) D 119) A 120) C 121) B 122) B 123) B 124) C 125) C 126) A 127) C 128) B 129) C 130) A 131) D 132) C 133) C 134) C 135) B 136) B 137) D 138) B 139) A 140) C 141) C 142) D 143) D 144) D 145) D 146) D 147) C 148) C 149) D 150) D 26

27 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 151) D 152) D 153) C 154) A 155) A 156) B 157) D 158) D 159) D 160) A 161) C 162) B 163) C 164) C 165) B 166) C 167) B 168) C 169) B 170) B 171) A 172) E 173) D 174) C 175) C 176) D 177) D 178) C 179) D 180) D 181) D 182) B 183) C 184) B 185) D 186) B 187) C 188) B 189) B 190) C 191) A 192) D 193) D 194) A 195) C 196) A 197) C 198) D 199) C 200) C 27

28 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 201) D 202) D 203) D 204) D 205) B 206) D 207) C 208) B 209) D 210) B 211) A 212) C 213) D 214) B 215) A 216) B 217) A 218) C 219) D 220) A 221) C 222) C 223) B 224) C 225) B 226) A 227) B 228) A 229) C 230) B 231) B 232) B 233) A 234) B 235) B 236) A 237) D 238) B 239) A 240) C 241) B 242) C 243) B 244) A 245) C 246) B 247) C 248) D 249) C 250) D 28

29 Answer Key Testname: GENERAL CHEMISTRY PHS 1015 PRACTICE EXAM 3 251) C 252) C 253) B 254) A 255) C 256) C 257) B 258) A 259) A 260) A 29