Question 1

Identify gasoline.

Accepted Answer

A)  strong electrolyte, weak acid 
B)  weak electrolyte, weak acid 
C)  strong electrolyte, strong acid 
D)  weak electrolyte, strong acid 
E)  nonelectrolyte 
A)  strong electrolyte, weak acid 
B)  weak electrolyte, weak acid 
C)  strong electrolyte, strong acid 
D)  weak electrolyte, strong acid 
E)  nonelectrolyte

Question 2

Give the theoretical yield,in moles,of CO2 from the reaction of 3.00 moles of C8H18 with 3.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Accepted Answer

A)  4.80 moles 
B)  48.0 moles 
C)  1.92 moles 
D)  12.0 moles 
E)  6.00 moles 
A)  4.80 moles 
B)  48.0 moles 
C)  1.92 moles 
D)  12.0 moles 
E)  6.00 moles

Question 3

Which of the following is NOT a strong electrolyte?

Accepted Answer

A)  LiOH 
B)  CaI2 
C)  MgCO3 
D)  KC2H3O2 
E)  K2SO4 
A)  LiOH 
B)  CaI2 
C)  MgCO3 
D)  KC2H3O2 
E)  K2SO4

Question 4

How many moles of BCl3 are needed to produce 25.0 g of HCl(aq)in the following reaction? BCl3(g)+ 3 H2O(l)→ 3 HCl(aq)+ B(OH)3(aq)

Accepted Answer

A)  0.229 mol 
B)  0.686 mol 
C)  2.06 mol 
D)  4.38 mol 
A)  0.229 mol 
B)  0.686 mol 
C)  2.06 mol 
D)  4.38 mol

Question 5

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 4.00 g of K3PO4 in enough water to make 350.mL of solution?

Accepted Answer

A)  0.0135 M 
B)  0.0539 M 
C)  0.215 M 
D)  0.431 M 
A)  0.0135 M 
B)  0.0539 M 
C)  0.215 M 
D)  0.431 M

Question 6

Identify the combustion reaction.

Accepted Answer

A)  2 C3H7OH(l) + 9 O2(g) → 6 CO2(g) + 8 H2O(g) 
B)  2 H2(g) + O2(g) → 2 H2O(g) 
C)  C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O 
D)  C(s) + O2(g) → CO2(g) 
E)  All of the reactions are examples of combustion reactions. 
A)  2 C3H7OH(l) + 9 O2(g) → 6 CO2(g) + 8 H2O(g) 
B)  2 H2(g) + O2(g) → 2 H2O(g) 
C)  C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O 
D)  C(s) + O2(g) → CO2(g) 
E)  All of the reactions are examples of combustion reactions.

Question 7

Which one of the following compounds is insoluble in water?

Accepted Answer

A)  Na2SO4 
B)  KNO3 
C)  Ba SO4 
D)  Rb2CO3 
A)  Na2SO4 
B)  KNO3 
C)  Ba SO4 
D)  Rb2CO3

Question 8

Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l)+ 6 O2(g)→ 3 CO2(g)+ SO2(g)+ 4 H2O(g)

Accepted Answer

A)  2.67 moles O2 
B)  6.00 moles O2 
C)  4.00 moles O2 
D)  16.0 moles O2 
E)  1.00 moles O2 
A)  2.67 moles O2 
B)  6.00 moles O2 
C)  4.00 moles O2 
D)  16.0 moles O2 
E)  1.00 moles O2

Question 9

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)

Accepted Answer

A)  0.290 mol O2 
B)  0.580 mol O2 
C)  18.5 mol O2 
D)  0.724 mol O2 
E)  1.73 mol O2 
A)  0.290 mol O2 
B)  0.580 mol O2 
C)  18.5 mol O2 
D)  0.724 mol O2 
E)  1.73 mol O2

Question 10

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

Accepted Answer

A)  Li+(aq) + NO3-(aq) → LiNO3(s) 
B)  S2-(aq) + Cu2+(aq) → CuS(s) 
C)  2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) 
D)  2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) 
E)  No reaction occurs. 
A)  Li+(aq) + NO3-(aq) → LiNO3(s) 
B)  S2-(aq) + Cu2+(aq) → CuS(s) 
C)  2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) 
D)  2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) 
E)  No reaction occurs.

Question 11

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)?

Accepted Answer

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

Question 12

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)

Accepted Answer

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

Question 13

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

Accepted Answer

A)  H+(aq) + OH-(aq) → H2O(l) 
B)  2 K+(aq) + SO42-(aq) → K2SO4(s) 
C)  H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + 2 K+(aq) + SO42-(aq) 
D)  H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H+(aq) + OH-(aq) + K2SO4(s) 
E)  No reaction occurs. 
A)  H+(aq) + OH-(aq) → H2O(l) 
B)  2 K+(aq) + SO42-(aq) → K2SO4(s) 
C)  H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + 2 K+(aq) + SO42-(aq) 
D)  H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H+(aq) + OH-(aq) + K2SO4(s) 
E)  No reaction occurs.

Question 14

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

Accepted Answer

A)  K+(aq) + NO3-(aq) → KNO3(s) 
B)  Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) 
C)  Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) 
D)  Fe2+(aq) + S2-(aq) → FeS(s) 
E)  No reaction occurs. 
A)  K+(aq) + NO3-(aq) → KNO3(s) 
B)  Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) 
C)  Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) 
D)  Fe2+(aq) + S2-(aq) → FeS(s) 
E)  No reaction occurs.

Question 15

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)

Accepted Answer

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 
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 16

Give the spectator ions for the reaction that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

Accepted Answer

A)  H+ and CO32- 
B)  Na+ and CO32- 
C)  H+ and Cl- 
D)  Na+ and Cl- 
E)  No spectator ions are present. 
A)  H+ and CO32- 
B)  Na+ and CO32- 
C)  H+ and Cl- 
D)  Na+ and Cl- 
E)  No spectator ions are present.

Question 17

Determine the oxidation state of magnesium in MgO.

Accepted Answer

A)  -5 
B)  +3 
C)  +1 
D)  +2 
E)  -4 
A)  -5 
B)  +3 
C)  +1 
D)  +2 
E)  -4

Question 18

Two samples of calcium fluoride are decomposed into their constituent elements.The first sample produced 0.154 g of calcium and 0.146 g of fluorine.If the second sample produced 294 mg of fluorine,how many g of calcium were formed?

Accepted Answer

A)  0.280 g 
B)  3.09 × 102 g 
C)  3.13 g 
D)  0.309 g 
E)  2.80 × 102 g 
A)  0.280 g 
B)  3.09 × 102 g 
C)  3.13 g 
D)  0.309 g 
E)  2.80 × 102 g

Question 19

Identify the diprotic acid.

Accepted Answer

A)  H2SO4 
B)  HCl 
C)  NaCl 
D)  NaOH 
E)  Mg(OH)2 
A)  H2SO4 
B)  HCl 
C)  NaCl 
D)  NaOH 
E)  Mg(OH)2

Question 20

Define an Arrhenius acid.

Accepted Answer

A)  an electron pair donor 
B)  an electron pair receiver 
C)  produces H+ ions in aqueous solution 
D)  accepts H+ ions 
E)  produces OH- ions in aqueous solution 
A)  an electron pair donor 
B)  an electron pair receiver 
C)  produces H+ ions in aqueous solution 
D)  accepts H+ ions 
E)  produces OH- ions in aqueous solution

Exam 4: Chemical Quantities and Aqueous Reactions

Identify gasoline.

Give the theoretical yield,in moles,of CO2 from the reaction of 3.00 moles of C8H18 with 3.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Which of the following is NOT a strong electrolyte?

How many moles of BCl3 are needed to produce 25.0 g of HCl(aq)in the following reaction? BCl3(g)+ 3 H2O(l)→ 3 HCl(aq)+ B(OH)3(aq)

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 4.00 g of K3PO4 in enough water to make 350.mL of solution?

Identify the combustion reaction.

Which one of the following compounds is insoluble in water?

Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l)+ 6 O2(g)→ 3 CO2(g)+ SO2(g)+ 4 H2O(g)

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)

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

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)?

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)

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

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

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)

Give the spectator ions for the reaction that occurs when aqueous solutions of Na2CO3 and HCl are mixed.

Determine the oxidation state of magnesium in MgO.

Two samples of calcium fluoride are decomposed into their constituent elements.The first sample produced 0.154 g of calcium and 0.146 g of fluorine.If the second sample produced 294 mg of fluorine,how many g of calcium were formed?

Identify the diprotic acid.

Define an Arrhenius acid.

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Give the theoretical yield,in moles,of CO₂from the reaction of 3.00 moles of C₈H₁₈ with 3.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

How many moles of BCl₃ are needed to produce 25.0 g of HCl(aq)in the following reaction? BCl₃(g)+ 3 H₂O(l)→ 3 HCl(aq)+ B(OH)₃(aq)

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 4.00 g of K₃PO₄ in enough water to make 350.mL of solution?

Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C₃H₇SH present. C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

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)

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)?

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)

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

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

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)

Give the spectator ions for the reaction that occurs when aqueous solutions of Na₂CO₃ and HCl are mixed.