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

Transcription

1 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Consider the balanced equation shown, and identify the statement that is not true. 1) Na2SO4 (aq) + BaCl2 (aq) 2 NaCl (aq) + BaSO4 (s) A) Barium sulfate is produced in solid form. B) The products are barium sulfate and sodium chloride. C) Barium chloride is dissolved in water. D) The coefficient of sodium sulfate is one. E) 2 NaCl (aq) could also be correctly written as Na2Cl2 (aq). 2) In a precipitation reaction the insoluble product can be identified by the symbol. A) (aq) B) (g) C) (s) D) (l) E) none of the above 2) 3) Consider the reaction shown and identify the statement that is not true. 3) CaCO3 (s) 825 C CaO (s) + CO 2 (g) A) The reactant must be heated for this reaction to occur. B) The products are a solid and a gas. C) Water must be present for this reaction to occur. D) This reaction is balanced as written. E) There are no solutions used in this reaction. 4) The scientific principle which is the basis for balancing chemical equations is A) the Law of Conservation of Mass. B) the Law of Conservation of Energy. C) the Law of Conservation of Mass and Energy. D) Avogadroʹs Law. E) the Law of Definite Proportions. 4) 1

2 5) Which statement regarding balanced chemical equations is not true? A) When no coefficient is written in front of a formula, the number ʺoneʺ is assumed. B) Reactants are written to the left of the arrow. C) The number of each kind of atoms must be the same on each side. D) Coefficients are used in front of formulas to balance the equation. E) Subscripts may be changed to make an equation simpler to balance. 5) 6) Which is the correct equation for the reaction of magnesium with hydrochloric acid to produce hydrogen and magnesium chloride? 6) A) Mg + HCl H + MgCl B) 2 Mg + 6 HCl 3 H2 + 2 MgCl2 C) Mg + 2 HCl H2 + MgCl2 D) Mg + 2 HCl 2 H + MgCl2 E) Mg + 3 HCl 3 H + MgCl2 7) Which of the following equations is not balanced? 7) A) 2 Al + 6 HCl 2 AlCl3 + 3 H2 B) 2 H2 + O2 2 H2O C) SO2 + O2 SO3 D) C3H8 + 5 O2 3 CO2 + 4 H2O E) 2 Na + 2 H2O 2 NaOH + H2 8) Which of the following equations is not balanced? A) C7H16 + O2 7 CO2 + 8 H2O 8) B) 2 Al2O3 4 Al + 3 O2 C) 4 Fe3O4 + O2 6 Fe2O3 D) K2CrO4 + Pb(NO3)2 2 KNO3 + PbCrO4 E) 3 AgNO3 + (NH4)3PO4 Ag3PO4 + 3 NH4NO3 9) When the reaction shown is correctly balanced, the coefficients are 9) KClO3 KCl + O2 A) 2, 2, 1 B) 4, 4, 6 C) 2, 2, 2 D) 1, 1, 1 E) 2, 2, 3 2

3 10) When the reaction shown is correctly balanced, the coefficients are 10) C6H14 (l) + O2 (g) CO2 (g) + H2O (g) A) 1, 6, 6, 7 B) 2, 16.5, 12, 7 C) 1, 3.5, 6, 7 D) 2, 19, 12, 14 E) 1, 9.5, 6, 7 11) When the reaction shown is correctly balanced, the coefficients are 11) HBr + Ca(OH)2 CaBr2 + H2O A) 2, 2, 1, 1 B) 1, 1, 1, 2 C) 2, 1, 1, 2 D) 2, 1, 1, 1 E) 2, 1, 2, 2 12) When the reaction shown is correctly balanced, the coefficients are 12) Li + Br2 LiBr A) 1, 2, 2 B) 1, 2, 1 C) 2, 2, 1 D) 1, 1, 1 E) 2, 1, 2 13) When the reaction shown is correctly balanced, the coefficients are 13) HNO3 + KOH KNO3 + H2O A) 2, 2, 2, 2 B) 1, 1, 1, 1 C) 3, 1, 1, 3 D) 0, 0, 0, 0 E) 2, 1, 2, 1 14) When the reaction shown is balanced, there are atoms of oxygen and atoms of hydrogen on each side. 14) (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + NH4C2H3O2 (aq) A) 16; 18 B) 8; 14 C) 16; 28 D) 6; 11 E) 4; 7 3

4 15) The balanced equation for the reaction occurring when calcium nitrate solution is mixed with sodium phosphate solution is 15) A) 3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) Ca3(PO4)2 (aq) + 6 NaNO3 (aq). B) Ca(NO3)2 (aq) + 2 NaPO4 (aq) Ca(PO4)2 (s) + 2 NaNO3 (aq). C) 2 Ca(NO3)2 (aq) + 3 Na3PO4 (aq) 2 Ca3(PO4)2 (s) + 6 NaNO3 (aq). D) 3 CaNO3 (aq) + Na3PO4 (aq) Ca3PO4 (aq) + 3 NaNO3 (s). E) 3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) Ca3(PO4)2 (s) + 6 NaNO3 (aq). 16) The balanced equation for the reaction occurring when iron(iii) oxide, a solid, is reduced with pure carbon to produce carbon dioxide and molten iron is 16) A) 2 FeO3 + 3 C (s) 2 Fe (l) + 3 CO2 (g). B) 2 Fe2O3 + 3 C (s) 4 Fe (l) + 3 CO2 (g). C) 2 Fe3O + C (s) 6 Fe (l) + CO2 (g). D) 2 FeO + C (s) 2 Fe (l) + CO2 (g). E) 4 Fe2O3 + 6 C (s) 8 Fe (l) + 6 CO2 (g). 17) The balanced equation for the reaction between aqueous ammonium sulfate and aqueous barium acetate is 17) A) (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) BaSO4 (aq) + 2 NH4C2H3O2 (s). B) (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + NH4C2H3O2 (aq). C) (NH4)2SO4 (aq) + Ba(C2H3O2)2 (aq) BaSO4 (s) + 2 NH4C2H3O2 (aq). D) NH4SO4 (aq) + BaC2H3O2 (aq) BaSO4 (s) + NH4C2H3O2 (aq). E) (NH4)2SO3 (aq) + Ba(C2H3O2)2 (aq) BaSO3 (aq) + NH4C2H3O2 (aq). 18) Which statement concerning the mole is not correct? A) The molar mass of any compound is equal to its molecular weight in grams. B) A mole of a diatomic element contains 2 NA moles of atoms of the element. 18) C) A mole of any compound contains one mole of each kind of atom found in that compound. D) A mole of metal contains NA atoms of that metal. E) All of these statements are correct. 4

5 19) Which statement concerning the mole concept is not true? A) One mole of sodium contains the same number of atoms as one mole of carbon. B) One mole of any compound contains one mole of atoms. C) The molar mass of a metal is its atomic weight expressed in grams. D) One mole of water contains the same number of molecules as one mole of ammonia. E) The mole concept makes a connection between the mass of a substance and the number of particles or units of that substance. 19) 20) Which statement based on the mole concept is not correct? A) The number of atoms in one mole of platinum is the same as the number of atoms in one mole of uranium. B) The molar mass of a diatomic element is its atomic weight times two. C) One mole of methane, CH4, contains the same number of atoms as one mole of carbon dioxide, CO2. 20) D) One mole of sodium chloride, NaCl, contains the same number of ions as one mole of calcium sulfate, CaSO4. E) One mole of bromine, Br2, contains the same number of molecules as one mole of propane, C3H8. 21) Which sample contains the largest number of ions? 21) A) 1.5 mol SnCl2 B) 1.0 mol NaNO3 C) 1.0 mol (NH4)3PO4 D) 1.5 mol AgNO3 E) 1.0 mol Fe(NO3)2 22) How many molecules are present in 4.25 mol of CCl4? 22) A) B) C) D) E) SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 23) Which sample contains more atoms, 1.60 mol of C2H6 or 4.00 mol of CO2? Explain your answer, including a calculation. 23) 24) Which contains more ions, 1 mol of ammonium sulfate or 1 mol of potassium phosphate? 24) 5

6 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 25) The molecular weight of PCl3 is amu. 25) A) B) C) D) E) ) The molar mass of Fe(OH)3 is g. 26) A) B) C) D) E) ) The number of grams in mol of Na is. A) B) 8.05 C) 65.7 D) 11.0 E) ) 28) The formula weight of copper(ii) chloride is g. A) B) C) D) E) ) 29) 42.0 g Cl2 contains molecules Cl2 and atoms of Cl. A) ; B) 1.18; C) ; D) 0.592; 1.18 E) ; ) 30) 50.0 g of Cl2 contains mol Cl2. 30) A) 50.0 B) 1.41 C) 1775 D) 4.24 x 1023 E) ) 105 g of MgCl2 contains mol MgCl2. A) 6.62 x 1023 B) 1.76 C) 1.10 D) 105 E) 1.06 x ) 32) How much Ca(NO3)2 should be weighed out to have mol? 32) A) 107 g B) 97.6 g C) 133 g D) 66.4 g E) 165 g 6

7 33) How many moles of NaHCO3 are present in a 2.00 g sample? 33) A) 2.38 x 10-2 mol B) 85.0 mol C) 2.00 mol D) 1.27 x 10-2 mol E) 168 mol 34) The number of grams in 2.65 mol of SO2 is 34) A) B) 170. C) D) E) 1.60 x ) A student weighed g of lithium chloride, LiCl, to use in a reaction. How many moles is this? A) B) C) D) 5.11 E) ) 36) Which sample contains the largest number of atoms? A) 1.0 mol H2O 36) B) 2.0 mol CH4 C) 1.5 mol NaCl D) 3.0 mol Cl2 E) 2.5 mol Au 37) Which sample contains the smallest number of atoms? A) 1.0 mol H2O 37) B) 2.0 mol CH4 C) 2.5 mol Au D) 1.5 mol NaCl E) 3.0 mol Cl2 38) The formula weight of Al2(SO4)3 is grams. 38) A) B) C) D) E) ) The molar mass of butane, C4H10, is grams. 39) A) B) C) D) E)

8 40) How many molecules are there in 3.00 moles of NH3? 40) A) B) 1.00 C) D) 3.00 E) ) How many molecules are present in 3.25 mol of C2H6O? 41) A) 3.25 B) C) D) E) ) The number of grams in 7.00 moles of N2 is. 42) A) 28.0 B) 14.0 C) 98.0 D) 7 ( ) E) ) The formula weight of ammonium carbonate, (NH4)2CO3, is amu 43) A) B) C) D) E) ) In the balanced reaction shown, the mole ratio of Fe2S3 to O2 is 44) Fe2S3 + 4 O2 2 FeO + 3 SO2 A) 4 to 3. B) 1 to 4. C) 5 to 5. D) 1 to 2. E) 4 to 1. 45) In the reaction shown, how many moles of HCl are needed to react with 2.4 moles of Al? 45) 2 Al + 6 HCl 2 AlCl3 + 3 H2 A) 1.3 B) 7.2 C) 4.8 D) 0.8 E) 6.4 8

9 46) Determine the number of moles of water produced when one mole of NH3 reacts according to the balanced reaction shown. 46) 4 NH3 + 5 O2 4 NO + 6 H2O A) 0.67 B) 1.33 C) 1.50 D) 1.00 E) ) Interpret in words the equation: 47) P4O10 (s) + 6 H2O (l) 4 H3PO4 (aq) A) One mole of phosphorus(x) oxide combines with six moles of water to produce four moles of solution of hydrogen phosphate. B) Zero moles of solid phosphoric oxide dissolve in six moles of water to produce four moles of phosphorous acid. C) One mole of solid tetraphosphorus decaoxide reacts with six moles of liquid water to produce four moles of phosphoric acid solution. D) Four moles of solid phosphorus, five moles of diatomic oxygen gas, and six moles of liquid water react together to produce four moles of phosphoric acid in solution. E) Four atoms of phosphorus, 16 atoms of oxygen, and 12 atoms of hydrogen rearrange to produce four molecules of phosphoric acid. 48) In the reaction shown, what is the mole ratio that would be used to determine the number of moles of H2 that would be produced when 3.5 moles of AlCl3 are produced? 48) 2 Al + 6 HCl 2 AlCl3 + 3 H2 A) 2 moles Al 3 moles HCl B) 2 moles AlCl 3 3 moles H2 C) 3.5 moles AlCl 3 3 moles H2 D) 3 moles AlCl 3 2 moles H2 E) 3 moles H2 2 moles AlCl3 9

10 49) In the reaction shown, what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C4H10? 49) 2 C4H O2 8 CO H2O A) 2 moles C 4HH10 13 moles O2 B) 3.2 moles C 4H10 13 moles O2 C) D) 13 moles O2 2 moles C4H10 13 moles O2 3.2 moles C4H10 E) 2 moles C 4H moles O2 50) The balanced equation given below means? 50) CH4 + 2O2 CO2 + 2H2O A) One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water. B) One gram of methane reacts with two grams of oxygen to produce one gram of carbon dioxide and two grams of water. C) One mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and 2 moles of water. D) A, B and C are correct E) A and C are correct 51) In a chemical reaction A) There are equal numbers of atoms on each side of the reaction arrow. B) There are always the same number of products as there are reactants. C) The number of atoms depends present in a reaction can vary when the conditions change during the reaction. D) There are equal numbers of molecules on each side of the reaction arrow. E) none of the above. 51) 10

11 SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question. 52) Consider the reaction N2 (g) + O2 (g) 2 NO (g). a. How many g NO can be produced when 25.0 g of nitrogen reacts? b. How many g NO can be produced when 25.0 g of oxygen reacts? c. Based on your answers in a and b, predict the amount of NO that can be produced when 25.0 g nitrogen is reacted with 25.0 g of oxygen. d. Explain the reasoning used in part c. 52) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 53) In the reaction 2 C + O2 2 CO, how many moles of carbon are needed to produce 66.0 g of carbon monoxide? A) 2.36 B) 4.71 C) D) 1.18 E) ) 54) How many grams of C will be consumed when 5.00 grams of Na2SO4 react according to the balanced reaction shown? 54) Na2SO4 + 2 C Na2S + 2 CO2 A) g B) 1.69 g C) g D) g E) 17.1 g 55) How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown? 55) 2 Fe + 3 F2 2 FeF3 A) 20.2 g B) 10.1 g C) 6.74 g D) 4.49 g E) 5.05 g 56) The percentage yield of a reaction can best be described as the times 100%. A) amount of product you could make if the reaction went to completion B) amount of product obtained divided by the maximum possible amount of product C) amount of reactants left over divided by the original amounts D) amount of desired product divided by the amount of unwanted product E) total amount of materials involved in a reaction 56) 57) The reaction N2 + 3 H2 2 NH3 is used to produce ammonia. When 450. g of hydrogen was reacted with nitrogen, 1575 g of ammonia were produced. What is the percent yield of this reaction? A) 30.8% B) 41.5% C) 20.7% D) 62.1% E) More information is needed to solve this problem. 57) 11

12 58) A solution containing g AgNO3 is mixed with a CaCl2 solution and 98.4 of AgCl is recovered. Calculate the % yield of the reaction. A) 61.99% B) 61.11% C) 40.16% D) 161.3% E) 80.44% 58) 59) The reaction 2 AgNO3(aq) + K2SO4(aq) 2 KNO3(aq) + Ag2SO4(s) is an example of a(an) reaction. A) acid-base B) combustion C) oxidation-reduction D) precipitation E) none of the above 59) 60) Which reaction is an example of a precipitation reaction? A) 2 Hg (l) + O2 (g) 2 HgO (s) 60) B) H2SO4 (aq) + Ca(OH)2 (aq) CaSO4 (aq) + 2 H2O (l) C) 6 HCl (aq) + 2 Al (s) 2 AlCl3 (aq) + 3 H2 (g) D) FeCl3 (aq) + KOH (aq) Fe(OH)3 (s) + 3 KCl (aq) E) H2CO3 (aq) H2O (l) + CO2 (g) 61) Which reaction is an example of both a precipitation and a neutralization? A) H2SO4 (aq) + Ba(OH)2 (aq) BaSO4 (s) + 2 H2O (l) 61) B) FeCl3 (aq) + KOH (aq) Fe(OH)3 (s) + 3 KCl (aq) C) (NH4)2CO3 (s) 2 NH3 (g) + CO2 (g) + H2O (l) D) 2 C (s) + O2 (g) 2 CO (g) E) 2 H3PO4 (aq) + 3 Ca(OH)2 (aq) Ca3(PO4)2 (aq) + 6 H2O (l) 62) The combination of ions most likely to produce a precipitate is A) NH4 + and SO ) B) Fe3+ and OH-. C) Pb2+ and NO3 -. D) Li+ and PO4 3-. E) Mg2+ and C2H3O

13 63) The combination of ions least likely to produce a precipitate is A) Mg2+ and C2H3O ) B) Ca2+ and PO4 3-. C) Fe3+ and OH-. D) Pb+ and Cl-. E) Ba2+ and SO ) When a solution of iron(iii) nitrate is mixed with a solution of sodium hydroxide, a rust colored precipitate forms. This precipitate is probably 64) A) sodium nitrate. B) iron(iii) nitrate. C) sodium hydroxide. D) iron(iii) hydroxide. E) none of the above 65) Which reaction is an example of an acid-base reaction? A) FeCl3(aq) + 3 KOH(aq) Fe(OH)3(s) + 3 KCl(aq) 65) B) 6 HCl(aq) + 2 Al(s) 2 AlCl3(aq) + 3 H2(g) C) H2CO3(aq) H2O(l) + CO2(g) D) 2 Hg(l) + O2(g) 2 HgO(s) E) H2SO4(aq) + Ca(OH)2(aq) CaSO4(aq) + 2 H2O(l) 66) The oxidation number of iron in the compound FeBr3 is. 66) A) +1 B) +2 C) +3 D) -1 E) -2 67) The oxidation number of sulfur in calcium sulfate, CaSO4, is. 67) A) 0 B) -2 C) +4 D) +6 E) +2 68) The oxidation number of chlorine in the compound FeCl3 is. 68) A) -3 B) -2 C) +3 D) -1 E) +2 13

14 69) As a pure element the oxidation number of zinc is, but in compounds such as ZnC O3 its oxidation number is. A) 0, 0 B) 0, +2 C) 0, +1 D) +1, 0 E) none of the above 69) 70) Fe(s) + CuCl2(aq) Cu(s) + FeCl2(aq) In the redox reaction shown, is oxidized and becomes. A) Fe, Fe+ B) Cu2+, Cu C) Fe, Fe2+ D) Cu, Cu2+ E) none of the above 70) 71) All of the statements regarding redox reactions are true except A) metal ions are produced when pure metals are oxidized. B) a reducing agent causes another substance to be reduced. C) alkali metals often behave as reducing agents because they readily lose electrons. D) halogens usually behave as oxidizing agents because they readily gain electrons. E) when a substance is oxidized its charge (or oxidation number) decreases. 71) 72) Which reaction is not an example of a redox reaction? A) 2 Al2O3 (s) 4 Al (s) + 3 O2 (g) 72) B) 2 Hg (l) + O2 (g) 2 HgO (s) C) 2 (NH4)3PO4 (aq) + 3 Ba(NO3)2 (aq) Ba3(PO4)2 (s) + 6 NH4NO3 (aq) D) CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g) E) 6 HCl (aq) + 2 Al (s) 2 AlCl3 (aq) + 3 H2 (g) 73) All of the reactions shown are oxidation-reduction reactions except A) 2 Fe2O3(s) 4 Fe(s) + 3 O2(g). 73) B) 2 NaI(aq) + Cl2(g) 2 NaCl(aq) + I2. C) N2(g) + O2(g) 2 NO(g). D) K2SO4(aq) + BaCl2(aq) BaSO4(s) + 2 KCl(aq). E) 2 Zn(s) + 2 HCl(aq) ZnCl2(aq) + H2(g). 14

15 74) The element chlorine is very reactive as a(an) agent because it readily electrons to form the chloride ion. 74) A) oxidizing, gains B) oxidizing, loses C) reducing, gains D) reducing, loses E) none of the above 75) When a substance loses electrons it is ; the substance itself is acting as a(an) agent. 75) A) dissolved, neutralizing B) oxidized, oxidizing C) oxidized, reducing D) reduced, oxidizing E) reduced, reducing 76) In the reaction shown, is the oxidizing agent because it. 76) Ni (s) + CuCl2 (aq) Cu (s) + NiCl2 (aq) A) CuCl2; causes reduction B) Ni; causes reduction C) NiCl2; gets reduced D) Ni; gets reduced E) CuCl2; gets reduced 77) Reduction is the process of A) forming an anion from a neutral atom. B) losing oxygen. C) gaining electrons. D) gaining hydrogen. E) all of the above. 77) 15

16 78) 2 AgNO3(aq) + K2SO4(aq) 2 KNO3(aq) + Ag2SO4(s) The net ionic reaction for the balanced equation shown above is 78) A) K+ + NO - 3 KNO 3. B) Ag+ + NO - 3 AgNO 3. C) H+ + OH- H2O. D) 2 Ag+ + SO 2-4 Ag 2SO4. E) 2 K+ + SO 2-4 K 2SO4. 79) The net ionic equation for the reaction between zinc and hydrochloric acid solution is A) ZnCl2 (aq) + H2 (g) ZnS (s) + 2 HCl (aq). 79) B) Zn (s) + 2 HCl (aq) ZnCl2 (aq) + H2 (g). C) Zn2+ (aq) + H2 (g) ZnS (s) + 2 H+ (aq). D) Zn (s) + 2 H+ (aq) Zn2+ (aq) + H2 (g). E) none of these 80) 2 AgNO3(aq) + K2SO4(aq) 2 KNO3(aq) + Ag2SO4(s) The spectator ions in the reaction shown are A) silver ion and sulfate ion. B) potassium ion and sulfate ion. C) potassium ion and nitrate ion. D) silver ion and nitrate ion. E) hydrogen ion and hydroxide ion. 80) 81) Which of the following is always a spectator ion in a chemical reaction? A) Cl- B) S2- C) Mg2+ D) Na+ E) all of these ions 81) 16

17 MATCHING. Choose the item in column 2 that best matches each item in column 1. Match the following. 82) The number of sulfur atoms in 2.00 mole of Al2(SO4)3 83) The number of nitrogen atoms in 1.50 mole of NH4NO3 A) precipitation B) redox C) 225 g 82) 83) 84) The number of hydrogen atoms in 1.00 mole of CH4 85) The molar mass of C15H32 86) The mass of 2.25 moles of CaCO3 87) The mass of 1.22 moles of iron(ii) nitrate D) acid-base E) F) G) H) 219 g 84) 85) 86) 87) 88) The molar mass of BaCl2 I) g 88) 89) M (s) + 2 LX (aq) 2 L (s) + MX2 (aq) J) g 89) 90) LX (aq) + MY (aq) LY (s) + MX (aq) 90) 91) HR (aq) + XOH (aq) XR (aq) + H2O (l) 91) 17

18 Answer Key Testname: UNTITLED5 1) E 2) C 3) C 4) A 5) E 6) C 7) C 8) A 9) E 10) D 11) C 12) E 13) B 14) B 15) E 16) B 17) C 18) C 19) B 20) C 21) A 22) E 23) One molecule of C2H6 contains a total of eight atoms, so one mol of C2H6 contains eight mol of atoms mol C2H6 8 mol atoms / 1 mol C2H6 = 12.8 mol of atoms. Similar reasoning can be used for CO2: 4.00 mol CO2 3 mol atoms / 1 mol CO2 = mol atoms > 12.00, so the sample of C2H6 contains more atoms. 24) One mole of ammonium sulfate, (NH4)2SO4, consists of two mol ammonium ions and one mol sulfate ions, for a total of three moles. One mol of potassium phosphate, K3PO4, consists of three mol potassium ions and one mol phosphate ions, for a total of four moles. Therefore, the potassium phosphate contains more ions. 25) A 26) C 27) B 28) D 29) C 30) E 31) C 32) A 33) A 34) B 35) B 36) B 37) C 38) D 39) E 40) E 41) C 42) E 43) D 18

19 Answer Key Testname: UNTITLED5 44) B 45) B 46) C 47) C 48) E 49) C 50) E 51) A 52) a g N2 1 mol N g N2 2 mol NO 1 mol N g NO 1 mol NO = g NO b g O2 1 mol N 2 32 g O2 2 mol NO 1 mol O g NO 1 mol NO = g NO c g NO d. There is only enough oxygen to produce g NO. Even though there is enough N 2 to produce more NO, there is not enough O2 to react with all the N2 available. Therefore, O2 is the limiting reactant. 53) A 54) A 55) B 56) B 57) D 58) E 59) D 60) D 61) A 62) B 63) A 64) D 65) E 66) C 67) D 68) D 69) B 70) C 71) E 72) C 73) D 74) A 75) C 76) E 77) E 78) D 79) D 80) C 81) D 82) G 83) E 84) F 19

20 Answer Key Testname: UNTITLED5 85) I 86) C 87) H 88) J 89) B 90) A 91) D 20