Deck 4: Chemical Quantities and Aqueous Reactions

Question 1

Consider the following balanced reaction.What mass (in g)of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present.
C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A)0.396 g CO₂
B)0.209 g CO₂
C)0.792 g CO₂
D)0.126 g CO₂
E)0.198 g CO₂

Answer 1

0.198 g CO₂

Question 2

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂.
2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2H₂O(l)

A)1.48 × 10²⁴ molecules H₂S
B)9.89 × 10²³ molecules H₂S
C)5.06 × 10²⁵ molecules H₂S
D)3.17 × 10²⁵ molecules H₂S
E)2.44 × 10²³ molecules H₂S

Answer 2

9.89 × 10²³ molecules H₂S

Question 3

Determine the theoretical yield of HCl if 60.0 g of BCl₃ and 37.5 g of H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl₃ = 117.16 g/mol.
BCl₃(g)+ 3 H₂O(l)→ H₃BO₃(s)+ 3 HCl(g)

A)75.9 g HCl
B)132 g HCl
C)187 g HCl
D)56.0 g HCl
E)25.3 g HCl

Answer 3

56.0 g HCl

Question 4

Consider the following reaction.How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C₃H₇SH present.
C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A)1.55 moles O₂
B)3.50 moles O₂
C)2.33 moles O₂
D)4.14 moles O₂
E)6.21 moles O₂

Question 5

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃).If it is the only product,what mass of PCl₃ is formed?

A)30.15 g
B)54.93 g
C)140.01 g
D)79.71 g
E)91.86 g

Question 6

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄.Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g/mol,N₂H₄ = 32.05 g/mol.
N₂O₄(l)+ 2 N₂H₄(l)→ 3 N₂(g)+ 4 H₂O(g)

A)LR = N₂H₄,59.0 g N₂ formed
B)LR = N₂O₄,105 g N₂ formed
C)LR = N₂O₄,45.7 g N₂ formed
D)LR = N₂H₄,13.3 g N₂ formed
E)No LR,45.0 g N₂ formed

Question 7

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.
6 Li(s)+ N₂(g)→ 2 Li₃N(s)

A)18.3 g Li₃N
B)20.3 g Li₃N
C)58.3 g Li₃N
D)61.0 g Li₃N
E)15.1 g Li₃N

Question 8

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃.
2 ICl₃ + 3 H₂O → ICl + HIO₃ + 5 HCl

A)2.78 × 10²⁴ molecules HCl
B)1.67 × 10²⁴ molecules HCl
C)5.02 × 10²⁵ molecules HCl
D)6.09 × 10²⁵ molecules HCl
E)3.65 × 10²⁴ molecules HCl

Question 9

Consider the following balanced reaction.How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present.The molar masses are as follows: H₂O = 18.02 g/mol,HNO₃ = 63.02 g/mol.
3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A)38.0 g H₂O
B)21.7 g H₂O
C)43.4 g H₂O
D)10.9 g H₂O
E)26.5 g H₂O

Question 10

How many grams of oxygen are formed when 6.21 moles of KOH are formed?
4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

A)19.9 g O₂
B)27.9 g O₂
C)49.7 g O₂
D)3.59 g O₂
E)11.7 g O₂

Question 11

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol.
4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

A)23.2 mol O₂
B)0.580 mol O₂
C)18.5 mol O₂
D)0.724 mol O₂
E)1.73 mol O₂

Question 12

According to the following balanced reaction,how many moles of NO are formed from 8.44 moles of NO₂ if there is plenty of water present?
3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A)2.81 moles NO
B)25.3 moles NO
C)8.44 moles NO
D)5.50 moles NO
E)1.83 moles NO

Question 13

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed?
2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2H₂O(l)

A)99.8 g S
B)66.6 g S
C)56.1 g S
D)44.4 g S
E)14.0 g S

Question 14

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃).If ammonia is the only product,what mass of ammonia is formed?

A)17.01 g
B)1.10 g
C)14.01 g
D)3.02 g
E)23.07 g

Question 15

According to the following balanced reaction,how many moles of KO are required to exactly react with 5.44 moles of H₂O?
4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

A)2.72 moles H₂O
B)16.7 moles H₂O
C)10.9 moles H₂O
D)8.33 moles H₂O
E)4.87 moles H₂O

Question 16

Carbonic acid can form water and carbon dioxide upon heating.How much carbon dioxide is formed from 6.20 g of carbonic acid?
H₂CO₃ → H₂O + CO₂

A)4.40 g
B)8.80 g
C)2.20 g
D)6.20 g

Question 17

According to the following reaction,what amount of Al₂S₃ remains when 20.00 g of Al₂S₃ and 2.00 g of H₂O are reacted? A few of the molar masses are as follows: Al₂S₃ = 150.17 g/mol,H₂O = 18.02 g/mol.
Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

A)28.33 g
B)14.00 g
C)8.33 g
D)19.78 g
E)17.22 g

Question 18

Determine the theoretical yield of H₂S (in moles)if 4.0 mol Al₂S₃ and 4.0 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃ = 150.17 g/mol.
Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

A)12 mol H₂S
B)4.0 mol H₂S
C)18 mol H₂S
D)6.0 mol H₂S
E)2.0 mol H₂S

Question 19

Give the theoretical yield,in moles,of CO₂ from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂.
2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A)0.640 moles
B)64.0 moles
C)2.56 moles
D)16.0 moles

Question 20

Give the theoretical yield,in grams,of CO₂ from the reaction of 4.000 moles of C₈H₁₈ with 4.000 moles of O₂.
2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A)112.7 g
B)102.4 g
C)176.0 g
D)704.0 g

Question 21

How many chloride ions are present in 65.5 mL of 0.210 M AlCl₃ solution?

A)4.02 × 10²³ chloride ions
B)5.79 × 10²⁴ chloride ions
C)2.48 × 10²² chloride ions
D)8.28 × 10²¹ chloride ions
E)1.21 × 10²² chloride ions

Question 22

What is the concentration of ions in a 0.25 M Al₂(CO₃)₃ solution?

A)0.25 M
B)1.00 M
C)1.25 M
D)0.50 M
E)0.75 M

Question 23

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO₃)₂ solution to 150.0 mL.

A)1.13 M
B)0.0887 M
C)0.0313 M
D)0.0199 M
E)0.0501 M

Question 24

How many milliliters of a 0.266 M LiNO₃ solution are required to make 150.0 mL of 0.075 M LiNO₃ solution?

A)53.2 mL
B)42.3 mL
C)18.8 mL
D)23.6 mL
E)35.1 mL

Question 25

How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution?

A)58.40 g
B)175.3 g
C)14.60 g
D)43.83 g

Question 26

How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl?

A)3.37 L
B)1.48 L
C)8.97 L
D)2.96 L
E)1.12 L

Question 27

How many milliliters of a 0.184 M NaNO₃ solution contain 0.113 moles of NaNO₃?

A)543 mL
B)163 mL
C)614 mL
D)885 mL
E)326 mL

Question 28

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield
750.0 mL of solution.

A)1.50 M
B)1.18 M
C)0.130 M
D)0.768 M
E)2.30 M

Question 29

How many moles of NaCl are required to make 250 mL of a 3.00 M solution?

A)750 moles
B)0.750 moles
C)3 moles
D)0.250 moles

Question 30

According to the following reaction,how many moles of Fe(OH)₂ can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl₂.
FeCl₂(aq)+ 2 LiOH(aq)→ Fe(OH)₂(s)+ 2 LiCl(aq)

A)3.97 × 10^-2 moles
B)2.52 × 10^-2 moles
C)1.99 × 10^-2 moles
D)5.03 × 10^-2 moles
E)6.49 × 10^-2 moles

Question 31

How many moles of CH₃CH₂OH are contained in 548 mL of 0.0788 M CH₃CH₂OH solution?

A)4.32 × 10^-2 mol
B)2.32 × 10^-2 mol
C)6.95 × 10^-2 mol
D)1.44 × 10^-2 mol
E)5.26 × 10^-2 mol

Question 32

How many molecules of sucrose (C₁₂H₂₂O₁₁,molar mass = 342.30 g/mol)are contained in 14.3 mL of 0.140 M sucrose solution?

A)8.29 × 10²² molecules C₁₂H₂₂O₁₁
B)1.21 × 10²¹ molecules C₁₂H₂₂O₁₁
C)6.15 × 10²² molecules C₁₂H₂₂O₁₁
D)1.63 × 10²³ molecules C₁₂H₂₂O₁₁
E)5.90 × 10²⁴ molecules C₁₂H₂₂O₁₁

Question 33

Which of the following solutions will have the highest concentration of chloride ions?

A)0.10 M NaCl
B)0.10 M MgCl₂
C)0.10 M AlCl₃
D)0.05 M CaCl₂
E)All of these solutions have the same concentration of chloride ions.

Question 34

What is the concentration of nitrate ions in a 0.125 M Mg(NO₃)₂ solution?

A)0.125 M
B)0.0625 M
C)0.375 M
D)0.250 M
E)0.160 M

Question 35

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction.
Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)

A)61.03%
B)28.65%
C)57.30%
D)20.02%
E)81.93%

Question 36

What volume (in mL)of 0.0887 M MgF₂ solution is needed to make 275.0 mL of 0.0224 M MgF₂ solution?

A)72.3 mL
B)91.8 mL
C)10.9 mL
D)69.4 mL
E)14.4 mL

Question 37

Give the percent yield when 28.16 g of CO₂ are formed from the reaction of 4.000 moles of C₈H₁₈ with 4.000 moles of O₂.
2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A)20.00%
B)25.00%
C)88.90%
D)22.20%

Question 38

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution?

A)1.31 × 10^-3 mol
B)8.74 × 10^-3 mol
C)1.14 × 10^-3 mol
D)3.67 × 10^-3 mol
E)7.65 × 10^-3 mol

Question 39

Determine the molarity of a solution formed by dissolving 468 mg of MgI₂ in enough water to yield 50.0 mL of solution.

A)0.0297 M
B)0.0337 M
C)0.0936 M
D)0.0107 M
E)0.0651 M

Question 40

Which of the following solutions will have the highest electrical conductivity?

A)0.045 M Al₂(SO₄)₃
B)0.050 M (NH₄)₂CO₃
C)0.10 M LiBr
D)0.10 M NaI
E)0.10 M KF

Question 41

What volume of 0.305 M AgNO₃ is required to react exactly with 155.0 mL of 0.274 M Na₂SO₄ solution? Hint: you will want to write a balanced reaction.

A)581 mL
B)173 mL
C)345 mL
D)139 mL
E)278 mL

Question 42

Which of the following is not a strong electrolyte?

A)LiOH
B)CaCl₂
C)MgCO₃
D)NaC₂H₃O₂
E)Li₂SO₄

Question 43

What precipitate is most likely formed from a solution containing Ba⁺²,Na⁺¹,OH^-1,and CO₃^-2.

A)NaOH
B)BaCO₃
C)Na₂CO₃
D)Ba(OH)₂

Question 44

Choose the statement below that is true.

A)A weak acid solution consists of mostly nonionized acid molecules.
B)The term "strong electrolyte" means that the substance is extremely reactive.
C)A strong acid solution consists of only partially ionized acid molecules.
D)The term "weak electrolyte" means that the substance is inert.
E)A molecular compound that does not ionize in solution is considered a strong electrolyte.

Question 45

According to the following reaction,what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO₃)₂ solution?
2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A)97.4 mL
B)116 mL
C)43.0 mL
D)86.1 mL
E)58.1 mL

Question 46

Which of the following is considered a strong electrolyte?

A)NH₄NO₃
B)C₁₂H₂₂O₁₁
C)PbCl₂
D)HC₂H₃O₂
E)CH₃OH

Question 47

How many of the following compounds are insoluble in water?
KC₂H₃O₂ CaSO₄ SrS AlPO₄

A)0
B)1
C)2
D)3
E)4

Question 48

Which of the following is a precipitation reaction?

A)Zn(s)+ 2 AgNO₃(aq)→ 2 Ag(s)+ Zn(NO₃)₂(aq)
B)NaCl(aq)+ LiI(aq)→ NaI(aq)+ LiCl(aq)
C)2 LiI(aq)+ Hg₂(NO₃)₂(aq)→ Hg₂I₂(s)+ 2 LiNO₃(aq)
D)HCl(aq)+ KOH(aq)→ KCl(aq)+ H₂O(l)
E)None of the above are precipitation reactions.

Question 49

According to the following reaction,what mass of PbCl₂ can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO₃)₂.
2 KCl(aq)+ Pb(NO₃)₂(aq)→ PbCl₂(s)+ 2 KNO₃(aq)

A)7.19 g
B)3.59 g
C)1.80 g
D)5.94 g
E)1.30 g

Question 50

Which of the following pairs of aqueous solutions will react to produce a precipitate?

A)LiOH + Na₂S
B)(NH₄)₂SO₄ + LiCl
C)Sr(C₂H₃O₂)₂ + Na₂SO₄
D)KNO₃ + NaOH
E)None of the above solution pairs will produce a precipitate.

Question 51

Which of the following is not a strong electrolyte?

A)CaS
B)LiSO₄
C)NH₄OH
D)CH₃CH₂CH₃
E)Na₂CO₃

Question 52

Which of the following compounds is insoluble in water?

A)Hg₂I₂
B)MgSO₄
C)(NH₄)₂CO₃
D)BaS
E)All of these compounds are soluble in water.

Question 53

What mass,in g,of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC₂H₃O₂ solution with 55.0 mL of 0.109 M MgCl₂ solution?
2 AgC₂H₃O₂(aq)+ MgCl₂(aq)→ 2 AgCl(s)+ Mg(C₂H₃O₂)₂(aq)

A)0.838 g
B)1.72 g
C)0.859 g
D)2.56 g
E)1.70 g

Question 54

Identify the spectator ions in the following molecular equation.
KBr(aq)+ AgNO₃(aq)→ AgBr(s)+ KNO₃(aq)

A)Ag⁺ & Br^-
B)K⁺ & NO₃^-
C)K⁺ & Br^-
D)Ag⁺ & NO₃^-
E)There are no spectator ions in this reaction.

Question 55

Which of the following pairs of aqueous solutions will produce a precipitate when mixed?

A)HCl + LiOH
B)Li₂S + HCl
C)K₂CO₃ + HNO₃
D)MgCl₂ + KOH
E)All of these solution pairs will produce a precipitate.

Question 56

How many of the following compounds are soluble in water?
Cu(OH)₂ LiNO₃ NH₄Br K₂S

A)0
B)1
C)2
D)3
E)4

Question 57

Which of the following compounds is soluble in water?

A)CaS
B)MgCO₃
C)PbCl₂
D)BaSO₄
E)None of these compounds is soluble in water.

Question 58

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of lithium sulfide and copper (II)nitrate are mixed.

A)Li⁺(aq)+ SO₄^2-(aq)+ Cu⁺(aq)+ NO₃^-(aq)→ CuS(s)+ Li⁺(aq)+ NO₃^-(aq)
B)Li⁺(aq)+ S^-(aq)+ Cu⁺(aq)+ NO₃^-(aq)→ CuS(s)+ LiNO₃(aq)
C)2 Li⁺(aq)+ S^2-(aq)+ Cu²⁺(aq)+ 2 NO₃^-(aq)→ Cu²⁺(aq)+ S^2-(aq)+ 2 LiNO₃(s)
D)2 Li⁺(aq)+ S^2-(aq)+ Cu²⁺(aq)+ 2 NO₃^-(aq)→ CuS(s)+ 2 Li⁺(aq)+ 2 NO₃^-(aq)
E)No reaction occurs.

Question 59

Determine the number of grams H₂ formed when 250.0 mL of 0.743 M HCl solution reacts with
3.41 × 10²³ atoms of Fe according to the following reaction.
2 HCl(aq)+ Fe(s)→ H₂(g)+ FeCl₂(aq)

A)0.374 g
B)1.33 g
C)1.14 g
D)0.187 g
E)1.51 g

Question 60

Which of the following pairs of aqueous solutions will react to produce a precipitate?

A)NH₄NO₃ + Li₂CO₃
B)Hg₂(NO₃)₂ + LiI
C)NaCl + Li₃PO₄
D)AgC₂H₃O₂ + Cu(NO₃)₂
E)None of the above solution pairs will produce a precipitate.

Question 61

Determine the oxidation state of Sn in Sn(SO₄)₂.

A)+2
B)+4
C)+6
D)0
E)-2

Question 62

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Al(C₂H₃O₂)₃ and LiNO₃ are mixed.

A)Al³⁺(aq)+ 3 NO₃^-(aq)→ Al(NO₃)₃(s)
B)Li⁺(aq)+ C₂H₃O₂^-(aq) _→ LiC₂H₃O₂(s)
C)Al³⁺(aq)+ 3 NO₃^-(aq)+ Li⁺(aq)+ C₂H₃O₂^-(aq)→ Al(NO₃)₃(aq)+ LiC₂H₃O₂(s)
D)3 Li⁺(aq)+ (C₂H₃O₂)₃^3-(aq)→ Li₃(C₂H₃O₂)_3(s)
E)No reaction occurs.

Question 63

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of H₂SO₄ and KOH are mixed.

A)H⁺(aq)+ OH^-(aq)→ H₂O(l)
B)2 K⁺(aq)+ SO₄^2-(aq)→ K₂SO₄(s)
C)H⁺(aq)+ OH^-(aq)+ 2 K⁺(aq)+ SO₄^2-(aq)→ H₂O(l)+ K₂SO₄(s)
D)H₂²⁺(aq)+ OH^-(aq)→ H₂(OH)₂(l)
E)No reaction occurs.

Question 64

Which of the following is a gas-evolution reaction?

A)2 C₂H₆(l)+ 7 O₂(g)→ 4 CO₂(g)+ 6 H₂O(g)
B)2 H₂(g)+ O₂(g)→ 2 H₂O(g)
C)LiCl(aq)+ NaNO₃(aq)→ LiNO₃(aq)+ NaCl(g)
D)NH₄Cl(aq)+ KOH(aq)→ KCl(aq)+ NH₃(g)+ H₂O(l)
E)None of the above are gas-evolution reactions.

Question 65

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H₂SO₄ solution (in M)?

A)0.20 M
B)0.40 M
C)0.10 M
D)0.36 M
E)0.25 M

Question 66

Match the following.
CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g)

A)combustion
B)acid base
C)oxidation reduction
D)gas evolution
E)precipitation

Question 67

Which of the following is an acid base reaction?

A)C(s)+ O₂(g)→ CO₂(g)
B)2 HClO₄(aq)+ Ca(OH)₂(aq)→ 2 H₂O(l)+ Ca(ClO₄)₂(aq)
C)Fe(s)+ 2 AgNO₃(aq)→ 2 Ag(s)+ Fe(NO₃)₂(aq)
D)MgSO₄(aq)+ Ba(NO₃)₂(aq)→ Mg(NO₃)₂(aq)+ BaSO₄(s)
E)None of the above are acid base reactions.

Question 68

Determine the oxidation state of P in PO₃^3-.

A)+3
B)+6
C)+2
D)0
E)-3

Question 69

What element is undergoing reduction (if any)in the following reaction?
Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

A)Zn
B)N
C)O
D)Ag
E)This is not an oxidation-reduction reaction.

Question 70

Determine the reducing agent in the following reaction.
2 Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2 LiC₂H₃O₂(aq)+ Fe(s)

A)O
B)H
C)C
D)Fe
E)Li

Question 71

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.

A)2 H⁺(aq)+ CO₃^2-(aq)→ H₂CO₃(s)
B)2 Na⁺(aq)+ CO₃^2-(aq)+ 2 H⁺(aq)+ 2 Cl^-(aq)→ H₂CO₃(s)+ 2 NaCl(aq)
C)2 H⁺(aq)+ CO₃^2-(aq)→ H₂O(l)+ CO₂(g)
D)2 Na⁺(aq)+ CO₃^2-(aq)+ 2 H⁺(aq)+ 2 Cl^-(aq)→ H₂CO₃(s)+ 2 Na⁺(aq)+ 2 Cl^-(aq)
E)No reaction occurs.

Question 72

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of K₂S and Fe(NO₃)₂ are mixed.

A)K⁺(aq)+ NO₃^-(aq)→ KNO₃(s)
B)Fe²⁺(aq)+ S^2-(aq)+ 2 K⁺(aq)+ 2 NO₃^-(aq)→ FeS(s)+ 2 K⁺(aq)+ 2 NO₃^-(aq)
C)Fe²⁺(aq)+ S^2-(aq)+ 2 K⁺(aq)+ 2 NO₃^-(aq)→ Fe²⁺(aq)+ S^2-(aq)+ 2 KNO₃(s)
D)Fe²⁺(aq)+ S^2-(aq)→ FeS(s)
E)No reaction occurs.

Question 73

Give the oxidation state for S in SO₃^-2.

A)+4
B)+6
C)-2
D)+2
E)+5

Question 74

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H₃PO₄ solution (in M)?

A)1.03 M
B)0.343 M
C)0.114 M
D)0.138 M
E)0.0461 M

Question 75

What element is undergoing oxidation (if any)in the following reaction?
CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g)

A)O
B)H
C)C
D)both C and H
E)None of the elements is undergoing oxidation.

Question 76

Choose the reaction that represents the combustion of C₆H₁₂O₂.

A)C₆H₁₂O₂(l)+ 8 O₂(g)→ 6 CO₂(g)+ 6 H₂O(g)
B)Mg(s)+ C₆H₁₂O₂(l)→ MgC₆H₁₂O₂(aq)
C)6 C(s)+ 6 H₂(g)+ O₂(g)→ C₆H₁₂O₂(l)
D)C₆H₁₂O₂(l)→ 6 C(s)+ 6 H₂(g)+ O₂(g)
E)None of the above represent the combustion of C₆H₁₂O₂.

Question 77

Give the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO₃ and HI are mixed.

A)2 H⁺(aq)+ SO₃^2-(aq)→ H₂SO₃(s)
B)Mg²⁺(aq)+ 2 I^-(aq)→ MgI₂(s)
C)2 H⁺(aq)+ SO₃^2-(aq)+ Mg²⁺(aq)+ 2 I^-(aq)→ H₂SO₃(s)+ MgI₂(aq)
D)2 H⁺(aq)+ SO₃^2-(aq)→ H₂O(l)+ SO₂(g)
E)No reaction occurs.

Question 78

Determine the oxidation state of Cl in NaClO₃.

A)+6
B)+4
C)+3
D)+2
E)+5

Question 79

Which of the following is an oxidation-reduction reaction?

A)HCl(aq)+ LiOH(aq)→ LiCl(aq)+ H₂O(l)
B)NaI(aq)+ AgNO₃(aq)→ AgI(s)+ NaNO₃(aq)
C)Pb(C₂H₃O₂)₂(aq)+ 2 NaCl(aq)→ PbCl₂(s)+ 2 NaC₂H₃O₂(aq)
D)Mg(s)+ 2 HCl(aq)→ MgCl₂(aq)+ H₂(g)
E)All of the above are oxidation-reduction reactions.

Question 80

Determine the oxidizing agent in the following reaction.
Ni(s)+ 2 AgClO₄(aq)→ Ni(ClO₄)₂(aq)+ 2 Ag(s)

A)Ag
B)Ni
C)Cl
D)O
E)This is not an oxidation-reduction reaction.