Sample Questions - Chapters 1-4

CHAPTERS 1 - 4
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CHAPTER 1

1.: Of the following name/symbol combinations of elements, which one is WRONG?; (a) uranium/U; (b) sulfur/S; (c) nitrogen/N; (d) potassium/K; (e) iron/I
2.: Of the following name/symbol combinations of elements, which one is WRONG?; (a) C/carbon; (b) B/barium; (c) F/fluorine; (d) N/nitrogen; (e) U/uranium
3.: The chemical symbol for manganese is; (a) Mn; (b) Mo; (c) Ma; (d) Ga; (e) Mg
4.: The number 0.005436 has how many significant figures?; (a) 2; (b) 3; (c) 4; (d) 5; (e) 6
5.: The number 10.00 has how many significant figures?; (a) 1; (b) 2; (c) 3; (d) 4; (e) 5
6.: What is the volume of a 2.50 gram block of metal whose density is 6.72 grams per cubic centimeter?; (a) 16.8 cubic centimeters; (b) 2.69 cubic centimeters; (c) 0.0595 cubic centimeters; (d) 0.372 cubic centimeters; (e) 1.60 cubic centimeters
7.: A cube of 1.2 inches on the side has a mass of 36 grams. What is the density in g/cm³?; (a) 21; (b) 2.2; (c) 30.; (d) 1.3; (e) 14
8.: Nitric acid is a very important industrial chemical: 1.612 x 10¹⁰ pounds of it were produced in 1992. If the density of nitric acid is 12.53 pounds/gallon, what volume would be occupied by this quantity? (1 gallon = 3.7854 liters); (a) 7.646 x 10¹¹ liters; (b) 8.388 x 10⁹ liters; (c) 1.287 x 10⁹ liters; (d) 5.336 x 10¹⁰ liters; (e) 4.870 x 10⁹ liters
9.: Identify the INCORRECT statement.; (a) Helium in a balloon: an element; (b) Paint: a mixture; (c) Tap water: a compound; (d) Mercury in a barometer; an element
10.: An unused flashbulb contains magnesium and oxygen. After use, the contents are changed to magnesium oxide but the total mass does not change. This observation can best be explained by the; (a) Law of Constant Composition.; (b) Law of Multiple Proportions.; (c) Avogadro's Law.; (d) Law of Conservation of Mass.
11.: Which answer includes all the following that are chemical changes and not physical changes?; I. freezing of water; II. rusting of iron; III. dropping a piece of iron into hydrochloric acid (H₂ is produced); IV. burning a piece of wood; V. emission of light by a kerosene oil lamp; (a) III and IV; (b) II and V; (c) I, II, III, IV, and V; (d) II, III, and V; (e) II, III, IV, and V
12.: Which response lists all of the following properties of sulfur that are physical properties and not other properties?; I.It reacts with hydrogen when heated.; II. It is a yellow solid at room temperature.; III. It is soluble in carbon disulfide.; IV. Its density is 2.97 g/cubic centimeter; V. It melts at 112°C.; (a) II, III, IV, and V; (b) II, IV, and V; (c) I only; (d) II, III, and IV; (e) III, IV, and V
Answers to Chapter 1: 1. (e) 2. (b) 3. (a) 4. (c) 5. (d) 6. (d) 7. (a) 8. (e) 9. (c) 10. (d) 11. (e) 12. (a)

CHAPTER 2

1.: The formula weight of the compound, Al₂(SO₄)₃^.18H₂O is:; (a) 394.4 g; (b) 666.4 g; (c) 110,900 g; (d) 466.8 g; (e) 561.2 g
2.: The weight of a millimole of (NH₄)₂HPO₄ is:; (a) 132 g; (b) 114 g; (c) 1.14 x 10^-3 g; (d) 0.132 g; (e) 6.02 x 10²⁰ g
3.: How many moles of alanine, C₃H₇NO₂, are there in 159 g of alanine?; (a) 1.42 x 10⁴; (b) 1.78; (c) 0.992; (d) 0.560; (e) 3.31
4.: How many atoms are in one mole of CH₃OH?; (a) 6; (b) 6.0 x 10²³; (c) 12.0 x 10²³; (d) 3.6 x 10²⁴; (e) 3
5.: The mass in grams of 2.6 x 10²² chlorine atoms is:; (a) 4.4; (b) 11; (c) 0.76; (d) 1.5; (e) 3.2
6.: How many aluminum atoms are there in 3.50 grams of Al₂O₃?; (a) 4.13 x 10²²; (b) 4.90 x 10²²; (c) 2.07 x 10²²; (d) 1.68 x 10²²; (e) 2.45 x 10²²
7.: Which one of the samples contains the most atoms?; (a) 1 mol of CO₂(g); (b) 1 mol of UF₆(g); (c) 1 mol of CH₃COCH₃(l); (d) 1 mol of He(g); (e) all contain the same number of atoms
8.: Which one of the samples contains the most molecules?; (a) 1 mol of CO₂(g); (b) 1 mol of UF₆(g); (c) 1 mol of CH₃COCH₃(l); (d) 1 mol of He(g); (e) all contain the same number of molecules
9.: Which one of the samples has the largest mass?; (a) 1 mol of CO₂(g); (b) 1 mol of UF₆(g); (c) 1 mol of CH₃COCH₃(l); (d) 1 mol of He(g); (e) all have the same mass
10.: Which of the following statements is(are) FALSE?; 1. The percent by mass of each element in a compound depends on the amount of the compound.; 2. The mass of each element in a compound depends on the amount of the compound.; 3. The percent by mass of each element in a compound depends on the amount of element present in the compound.; (a) 2 and 3; (b) 1 only; (c) 1 and 2; (d) 1, 2 and 3
11.: Guanidin, HNC(NH₂)₂, is a fertilizer. To three significant figures, what is the percent by mass of nitrogen in the fertilizer?; (a) 45.2%; (b) 49.4%; (c) 54.8%; (d) 65.1%; (e) 71.1%
12.: Calculate the percent, by weight, of carbon in 154 g of C₄H₈O₃?; (a) 46%; (b) 31%; (c) 72%; (d) 27%; (e) 55%
13.: Analysis of a sample of a covalent compound showed that it contained 14.4% hydrogen and 85.6% carbon by mass. What is the empirical formula for the compound?; (a) CH; (b) CH₂; (c) CH₃; (d) C₂H₃; (e) none of these
14.: An oxide of lead contains 90.65% Pb, by weight. The empirical formula is:; (a) Pb; (b) PbO; (c) Pb₃O₄; (d) Pb₂O₃; (e) PbO₂
15.: A 0.500 g sample of a compound containing only antimony and oxygen was found to contain 0.418 g of antimony and 0.082 g of oxygen. What is the simplest formula for the compound?; (a) SbO; (b) SbO₂; (c) Sb₃O₄; (d) Sb₂O₅; (e) Sb₂O₃
16.: A compound contains, by mass, 40.0% carbon, 6.71% hydrogen, and 53.3% oxygen. A 0.320 mole sample of this compound weighs 28.8 g. The molecular formula of this compound is:; (a) C₂H₄O₂; (b) C₃H₆O₃; (c) C₂H₄O; (d) CH₂O; (e) C₄H₇O₂
17.: What mass of cerussite, PbCO₃, would contain 35.0 grams of lead?; (a) 27.1 g; (b) 45.1 g; (c) 42.4 g; (d) 35.6 g; (e) 51.7 g
Answers to Chapter 2: 1. (b) 2. (d) 3. (b) 4. (b) 5. (d) 6. (a) 7. (c) 8. (e) 9. (b) 10. (b) 11. (e) 12. (a) 13. (b) 14. (c) 15. (e) 16. (b) 17. (b)

CHAPTER 3

1.: Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one."
PtCl₄ + XeF₂^___> PtF₆ + ClF + Xe; (a) 16; (b) 22; (c) 24; (d) 26; (e) 32
2.: Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one."
Cr₂(SO₄)₃ + RbOH ^___> Cr(OH)₃ + Rb₂SO₄; (a) 10; (b) 12; (c) 13; (d) 14; (e) 15
3.: Balance the following equation using minimum integral coefficients:
NH₃ + O₂ ^___> NO₂ + H₂O
The stoichiometric coefficient for oxygen gas O₂ is:; (a) 1; (b) 4; (c) 3; (d) 7; (e) 5
4.: When iron pyrite (FeS₂) is heated in air, the process known as "roasting" forms sulfur dioxide and iron(III) oxide. When the equation for this process is completed and balanced, using the smallest whole number coefficients, what is the coefficient for "O₂"?
___ FeS₂ + ___ O₂^___> ___ SO₂ + ___ Fe₂O₃; (a) 2; (b) 4; (c) 7; (d) 8; (e) 11
5.: How many moles of KBrO₃ are required to prepare 0.0700 moles of Br₂ according to the reaction:
KBrO₃ + 5KBr + 6HNO₃ ^___> 6KNO₃ + 3Br₂ + 3H₂O; (a) 0.210; (b) 0.0732; (c) 0.0704; (d) 0.220; (e) 0.0233
6.: Which of the following statements is FALSE for the chemical equation given below in which nitrogen gas reacts with hydrogen gas to form ammonia gas assuming the reaction goes to completion?
N₂ + 3H₂^___> 2NH₃; (a) The reaction of one mole of H₂ will produce 2/3 moles of NH₃.; (b) One mole of N₂ will produce two moles of NH₃.; (c) One molecule of nitrogen requires three molecules of hydrogen for complete reaction.; (d) The reaction of 14 g of nitrogen produces 17 g of ammonia.; (e) The reaction of three moles of hydrogen gas will produce 17 g of ammonia.
7.: Calcium carbide, CaC₂, is an important preliminary chemical for industries producing synthetic fabrics and plastics. CaC₂ may be produced by heating calcium oxide with coke:
CaO + 3C ^___> CaC₂ + CO
What is the amount of CaC₂ which can be produced from the reaction of excess calcium oxide and 10.2 g of carbon? (Assume 100% efficiency of reaction for purposes of this problem.); (a) 18.1 g; (b) 28.4 g; (c) 20.8 g; (d) 19.8 g; (e) 27.2 g
8.: Calculate the mass of hydrogen formed when 25 grams of aluminum reacts with excess hydrochloric acid.
2Al + 6HCl ^___> Al₂Cl₆ + 3H₂; (a) 0.41 g; (b) 1.2 g; (c) 1.8 g; (d) 2.8 g; (e) 0.92 g
9.: When 12 g of methanol (CH₃OH) was treated with excess oxidizing agent (MnO₄^-), 14 g of formic acid (HCOOH) was obtained. Using the following chemical equation, calculate the percent yield. (The reaction is much more complex than this; please ignore the fact that the charges do not balance.)
3CH₃OH + 4MnO₄^- ^___> 3HCOOH + 4MnO₂; (a) 100%; (b) 92%; (c) 82%; (d) 70%; (e) 55%
10.: A commercially valuable paint and adhesive stripper, dimethyl sulfoxide (DMSO), (CH₃)₂SO, can be prepared by the reaction of oxygen with dimethyl sulfide, (CH₃)₂S, using a ratio of one mole oxygen to two moles of the sulfide:
O₂ + 2(CH₃)₂S^___> 2(CH₃)₂SO
If this process is 83% efficient, how many grams of DMSO could be produced from 65 g of dimethyl sulfide and excess O₂?; (a) 68 g; (b) 75 g; (c) 83 g; (d) 51 g; (e) 47 g
11.: The formation of ethyl alcohol (C₂H₅OH) by the fermentation of glucose (C₆H₁₂O₆) may be represented by:
C₆H₁₂O₆ ^___> 2C₂H₅OH + 2CO₂
If a particular glucose fermentation process is 87% efficient, how many grams of glucose would be required for the production of 51 g of ethyl alcohol (C₂H₅OH)?; (a) 68 g; (b) 75 g; (c) 115 g; (d) 229 g; (e) 167 g
12.: The limiting reagent in a chemical reaction is one that:; (a) has the largest molar mass (formula weight).; (b) has the smallest molar mass (formula weight).; (c) has the smallest coefficient.; (d) is consumed completely.; (e) is in excess.
13.: If 5.0 g of each reactant were used for the the following process, the limiting reactant would be:
2KMnO₄ +5Hg₂Cl₂ + 16HCl ^___> 10HgCl₂ + 2MnCl₂ + 2KCl + 8H₂O; (a) KMnO₄; (b) HCl; (c) H₂O; (d) Hg₂Cl₂; (e) HgCl₂
14.: What mass of ZnCl₂ can be prepared from the reaction of 3.27 grams of zinc with 3.30 grams of HCl?
Zn +2HCl ^___> ZnCl₂ + H₂; (a) 6.89 g; (b) 6.82 g; (c) 6.46 g; (d) 6.17 g; (e) 6.02 g
15.: How many grams of NH₃ can be prepared from 77.3 grams of N₂ and 14.2 grams of H₂? (Hint: Write and balance the equation first.); (a) 93.9 g; (b) 79.7 g; (c) 47.0 g; (d) 120.0 g; (e) 13.3 g
16.: Silicon carbide, an abrasive, is made by the reaction of silicon dioxide with graphite. SiO₂ +3C ^___> SiC + 2CO
If 100 g of SiO₂ and 100 g of C are reacted as far as possible, which one of the following statements will be correct?; (a) 111 g of SiO₂ will be left over.; (b) 44 g of SiO₂ will be left over.; (c) 82 g of C will be left over.; (d) 40 g of C will be left over.; (e) Both reactants will be consumed completely, with none of either left over.
17.: Calculate the mass of 6.00% NiSO₄ solution that contains 40.0 g of NiSO₄?; (a) 667 g; (b) 540 g; (c) 743 g; (d) 329 g; (e) none of these
18.: How many grams of water are contained in 75.0 grams of a 6.10% aqueous solution of K₃PO₄?; (a) 75.0 g; (b) 73.2 g; (c) 70.4 g; (d) 68.1 g; (e) 62.8 g
19.: The mass (in grams) of FeSO₄.7H₂O required for preparation of 125 mL of 0.90 M solution is:; (a) 16 g; (b) 25 g; (c) 13 g; (d) 31 g; (e) 43 g
20.: What is the molarity of phosphoric acid in a solution labeled 20.0% phosphoric acid (H₃PO₄) by weight with a density = 1.12 g/mL?; (a) 0.98 M; (b) 2.3 M; (c) 2.7 M; (d) 3.0 M; (e) 3.6 M
21.: How many mL of 17 M NH₃ must be diluted to 500.0 mL to make a 0.75 M solution?; (a) 13 mL; (b) 22 mL; (c) 39 mL; (d) 73 mL; (e) none of these
22.: How many grams of Ag₂CO₃ are required to react with 28.5 mL of 1.00 M NaOH solution?
Ag₂CO₃ +2NaOH ^___> Ag₂O + Na₂CO₃ + H₂O; (a) 7.87 g; (b) 3.93 g; (c) 15.7 g; (d) 10.8 g; (e) 8.16 g
23.: How many milliliters of 0.200 M NH₄OH are needed to react with 12.0 mL of 0.550 M FeCl₃?
FeCl₃ + 3NH₄OH ^___> Fe(OH)₃ + 3NH₄Cl; (a) 99.0 mL; (b) 33.0 mL; (c) 8.25 mL; (d) 68.8 mL; (e) 132 mL
24.: When 250. mL of a 0.15 M solution of ammonium sulfide (NH₄)₂S is poured into 120. mL of a 0.053 M solution of cadmium nitrate CdSO₄, how many grams of a yellow precipitate of cadmium sulfide CdS are formed? The other product is (NH₄)₂SO₄. (Hint: Write out and balance the equation. Is this a limiting reagent problem? ); (a) 5.4 g; (b) 0.92 g; (c) 2.6 g; (d) 1.9 g; (e) 530 g
Answers to Chapter 3: 1. (a) 2. (b) 3. (e) 4. (e) 5. (e) 6. (e) 7. (a) 8. (d) 9. (c) 10. (a) 11. (c) 12. (d) 13. (d) 14. (d) 15. (b) 16. (d) 17. (a) 18. (c) 19. (d) 20. (b) 21. (b) 22. (b) 23. (a) 24. (a)

CHAPTER 4

1.: What alkaline earth metal is located in period 3?; (a) Li; (b) Na; (c) Ca; (d) Mg; (e) Sr
2.: Which of the following is classified as a metal?; (a) Ge; (b) As; (c) F; (d) V; (e) Ar
3.: Which of the following is a weak acid?; (a) H₂SO₄; (b) HClO₃; (c) HF; (d) HCl; (e) HNO₃
4.: Which one of the following is likely to be the most soluble base?; (a) Ca(OH)₂; (b) Ag(OH)₂; (c) Ga(OH)₃; (d) Zn(OH)₂; (e) Zr(OH)₃
5.: Which one of the following statements is TRUE?; (a) One mole of any acid will ionize completely in aqueous solution to produce one mole of H⁺ ions.; (b) Solutions of weak acids always have lower concentrations of H⁺ than solutions of strong acids.; (c) There are several common acids that are insoluble.; (d) The soluble bases are all of the IA and IIA metal hydroxides.; (e) All weak acids are insoluble.
6.: Which one of the following salts is insoluble?; (a) NH₄Cl; (b) Ca(NO₃)₂; (c) BaCO₃; (d) Na₂S; (e) Zn(CH₃COO)₂
7.: What salt is formed in the following acid/base reaction?
HClO₃ + Ba(OH)₂ ^___>; (a) BaCl₂; (b) ClOBa; (c) H₂O; (d) BaClO₃; (e) Ba(ClO₃)₂
7.: The precipitate formed when barium chloride is treated with sulfuric acid is _______ ,; (a) BaS₂O₄; (b) BaSO₃; (c) BaSO₂; (d) BaSO₄
8.: The spectator ion(s) in the following reaction is/are:
Na₂CO₃(aq) + Ba(NO₃)₂(aq)^___> BaCO₃(s) + 2NaNO₃(aq); (a) Na⁺ and Ba²⁺; (b) Ba²⁺ and CO₃^-2; (c) CO₃^2- and NO₃-; (d) Na⁺ only; (e) Na⁺ and NO₃^-
9.: Which one of the following statements is FALSE?; (a) For the reaction of a strong acid with a strong base, the net ionic equation is always
H⁺ + OH^- ^___> H₂O; (b) "Spectator ion" appear in the total ionic equation for a reaction, but not in the net ionic equation.; (c) HF, HCl, and HNO₃ are all examples of strong acids.; (d) Titration is a process which can be used to determine the concentration of a solution.; (e) In a neutralization reaction, an acid reacts with base to produce a salt and H₂O.
10.: What is the net ionic equation for the acid-base reaction that occurs when acetic acid and potassium hydroxide solutions are mixed?; (a) H⁺(aq) + OH^-(aq) ^___> H₂O(l); (b) H⁺(aq) + KOH(s) ^___> K⁺(aq) + H₂O(l); (c) CH₃COOH(aq) + KOH(s) ^___> KCH₃COO(aq) + H₂O(l); (d) CH₃COO^-(aq) + H⁺(aq) + K⁺(aq) + OH^-(aq) ^___> K⁺(aq) + CH₃COO^-(aq) + H₂O(l); (e) CH₃COOH(aq) + OH^-(aq) ^___> CH₃COO^-(aq) + H₂O(l)
11.: What is the net ionic equation for the acid-base reaction that occurs when nitric acid is added to copper(II) hydroxide?; (a) H⁺(aq) + OH^-(aq) ^___> H₂O(l); (b) 2H⁺(aq) + Cu(OH)₂(s) ^___> Cu²⁺(aq) + 2H₂O(l); (c) 2HNO₃(aq) +Cu(OH)₂(s) ^___> Cu(NO₃)₂(s) + 2H₂O(l); (d) 2H⁺(aq) + 2NO₃^-(aq) + Cu²⁺(aq) + 2OH^-(aq) ^___> Cu(NO₃)₂(s) + 2H₂O(l); (e) 2H⁺(aq) + 2NO₃^-(aq) + Cu²⁺(aq) + 2OH^-(aq) ^___> Cu²⁺(aq) + 2NO₃^-(aq) + 2H₂O(l)
12.: Which of the following statements is FALSE given the following net ionic equation?
H₃PO₄(aq) + 3OH^-(aq) ^___> PO₄^3-(aq) + 3H₂O(l); (a) If all the water evaporated away, the salt remaining could possibly be Na₃PO₄.; (b) The acid, H₃PO₄, is a weak electrolyte.; (c) The base involved must be a strong soluble base.; (d) This is classified as a neutralization reaction.; (e)This could be the net ionic equation for H₃PO₄ reacting with Al(OH)₃.
13.: Which of the following statements is FALSE given the following net ionic equation?
2H⁺(aq) + Cu(OH)₂(s) ^___> Cu²⁺(aq) + 2H₂O(l); (a) If all the water evaporated away, the salt remaining could possibly be NaS.; (b) The acid involved must be a strong electrolyte.; (c) The base, Cu(OH)₂, is an insoluble base.; (d) This could be the net ionic equation for HNO₃ reacting with Cu(OH)₂.; (e) This is classified as a neutralization reaction.
14.: Determine the oxidation number of carbon in K₂CO₃.; (a) 0; (b) +2; (c) +4; (d) -2; (e) some other value
14.: Determine the oxidation number of chromium in K₂Cr₂O₇.; (a) 0; (b) +3; (c) +6; (d) +12; (e) some other value
14.: Given that the Activity Series is: Na>Mg>Cu>Ag>Au, which one of the following answers represents the ions that would not be displaced from aqueous solution (reduced) by metallic magnesium?; (a) Na⁺; (b) Cu²⁺; (c) Cu²⁺ and Au⁺; (d) Cu²⁺, Ag⁺ and Au⁺; (e) Na⁺, Cu²⁺, Ag⁺ and Au⁺