Question 1

How many mL of 0.024 M solution can be produced from 14.1 mL of 3.0 M solution?

Accepted Answer

A)  (14.1)(0.024)(3.0) mL 
B)  14.1(0.024/3.0) mL 
C)  14.1(3.0/0.024) mL 
D)  (14.1/0.024)/3.0 mL 
E)  (0.024×3)/14.1 mL 
A)  (14.1)(0.024)(3.0) mL 
B)  14.1(0.024/3.0) mL 
C)  14.1(3.0/0.024) mL 
D)  (14.1/0.024)/3.0 mL 
E)  (0.024×3)/14.1 mL

Question 2

What is the molarity of methanol, CH3OH (d = 0792 g/mL), if 150.0 mL is dissolved in enough water to make 4.00 L of solution?

Accepted Answer

A)  3.71 M 
B)  1.17 M 
C)  1.48 M 
D)  0.927 M 
E)  0.734 M 
A)  3.71 M 
B)  1.17 M 
C)  1.48 M 
D)  0.927 M 
E)  0.734 M

Question 3

The reactant that is in excess determines the amount of products formed.

Accepted Answer

A) True 
 B)False

Question 4

When the equation CS2 + Cl2 → CCl4 + S2Cl2 is balanced with the smallest integer coefficients, the sum of the coefficients is:

Accepted Answer

A)  5 
B)  6 
C)  4 
D)  3 
E)  7 
A)  5 
B)  6 
C)  4 
D)  3 
E)  7

Question 5

Given the reaction: 2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O
How many moles of I2 are produced by reacting 28.0 g KMnO4, 18.0 g KI, and 46.0 g H2SO4?

Accepted Answer

A)  0.108 mol 
B)  0.0542 mol 
C)  0.293 mol 
D)  0.443 mol 
E)  0.886 mol 
A)  0.108 mol 
B)  0.0542 mol 
C)  0.293 mol 
D)  0.443 mol 
E)  0.886 mol

Question 6

If an aqueous solution containing 46 g of sodium carbonate per liter is mixed with an equal volume of 0.20 M aqueous hydrochloric acid, what would be the molarity of sodium chloride in the final solution, assuming volumes were additive?

Accepted Answer

A)  0.10 M 
B)  0.20 M 
C)  0.22 M 
D)  0.43 M 
E)  0.50 M 
A)  0.10 M 
B)  0.20 M 
C)  0.22 M 
D)  0.43 M 
E)  0.50 M

Question 7

If 85.6 mL of a 6.75 M solution are diluted to 6.20 L with water, what is the concentration of the final solution?

Accepted Answer

A)  6.75 (6.20/85.6) M 
B)  6.75 (8.56/6.20) M 
C)  6.75 (6200/85.6) M 
D)  6.75 (85.6/6200) M 
E)  8.56 (6.20/6.75) M 
A)  6.75 (6.20/85.6) M 
B)  6.75 (8.56/6.20) M 
C)  6.75 (6200/85.6) M 
D)  6.75 (85.6/6200) M 
E)  8.56 (6.20/6.75) M

Question 8

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? CH3OH → CO + H2

Accepted Answer

A)  3 
B)  8 
C)  5 
D)  4 
E)  7 
A)  3 
B)  8 
C)  5 
D)  4 
E)  7

Question 9

Potassium superoxide (KO2) can simulate a plant-type action by consuming carbon dioxide (CO2) gas and releasing oxygen (O2) gas. The other product is potassium carbonate (K2CO3). When the equation for this process is balanced, it shows that:

Accepted Answer

A)  3 mol oxygen is produced per mol KO2 consumed 
B)  2 mol KO2 is consumed per mol carbon dioxide 
C)  moles of reactants equals moles of product 
D)  3 g of oxygen is produced per 2 g CO2 consumed 
E)  moles of products exceed moles of reactants 
A)  3 mol oxygen is produced per mol KO2 consumed 
B)  2 mol KO2 is consumed per mol carbon dioxide 
C)  moles of reactants equals moles of product 
D)  3 g of oxygen is produced per 2 g CO2 consumed 
E)  moles of products exceed moles of reactants

Question 10

Cryolite is a compound needed for the Hall-Heroult process for producing aluminum. Cryolite is produced by the following reaction: 6 HF + Al(OH)3 + 3 NaOH → Na3AlF6 + 6 H2O
How many grams of cryolite are produced if the reaction has a 94.3% yield and a limiting reagent of 27.8 grams of HF?

Accepted Answer

A)  275 g 
B)  48.6 g 
C)  45.9 g 
D)  15.0 g 
E)  15.9 g 
A)  275 g 
B)  48.6 g 
C)  45.9 g 
D)  15.0 g 
E)  15.9 g

Question 11

What is the sum of the coefficients when the following equation is balanced with the smallest integer coefficients? H2SO3 + Al(OH)3 → Al2(SO3)3 + H2O

Accepted Answer

A)  4 
B)  5 
C)  11 
D)  12 
E)  14 
A)  4 
B)  5 
C)  11 
D)  12 
E)  14

Question 12

A chemical equation is a shorthand way of representing a chemical reaction.

Accepted Answer

A) True 
 B)False

Question 13

A 1.900 g sample of C6H12 is burned in an excess of oxygen. What mass of CO2 and H2O should be obtained?

Accepted Answer

A)  0.994 g CO2, 0.407 g H2O 
B)  2.98 g CO2, 1.22 g H2O 
C)  5.96 g CO2, 2.44 g H2O 
D)  10.45 g CO2, 4.27 g  H2O 
E)  5.23 g CO2, 2.38 g H2O 
A)  0.994 g CO2, 0.407 g H2O 
B)  2.98 g CO2, 1.22 g H2O 
C)  5.96 g CO2, 2.44 g H2O 
D)  10.45 g CO2, 4.27 g  H2O 
E)  5.23 g CO2, 2.38 g H2O

Question 14

Chromium in its +VI oxidation state is considered a hazardous, carcinogenic species, destruction of which may be accomplished by the process symbolized as: 4 Zn + K2Cr2O7 + 7 H2SO4 → 4 ZnSO4 + 2 CrSO4 + K2SO4 + 7 H2O
If 1.0 mol of each reactant is mixed, what is the limiting reagent, and what is the theoretical yield of chromium(II) sulfate?

Accepted Answer

A)  Zn, 0.50 mol 
B)  K2Cr2O7, 2.0 mol 
C)  H2SO4, 0.29 mol 
D)  H2, 1.0 mol 
E)  no limiting reagent, 1.0 mol 
A)  Zn, 0.50 mol 
B)  K2Cr2O7, 2.0 mol 
C)  H2SO4, 0.29 mol 
D)  H2, 1.0 mol 
E)  no limiting reagent, 1.0 mol

Question 15

Iron metal reacts with chlorine gas as follows: 2 Fe(s) + 3 Cl2(g) → 2 FeCl3(s)
How many moles of FeCl3 are obtained when 4.6 mol of Cl2 reacts with excess Fe?

Accepted Answer

A)  3.1 mol 
B)  4.6 mol 
C)  1.5 mol 
D)  2.3 mol 
E)  6.9 mol 
A)  3.1 mol 
B)  4.6 mol 
C)  1.5 mol 
D)  2.3 mol 
E)  6.9 mol

Question 16

In the following reaction: 2 KClO3(s) → 2 KCl(s) + 3 O2(g)
14.0 g KClO3 yielded 1.40 g KCl. What is the percent yield?

Accepted Answer

A)  6.08% 
B)  16.4% 
C)  11.0% 
D)  32.9% 
E)  10.0% 
A)  6.08% 
B)  16.4% 
C)  11.0% 
D)  32.9% 
E)  10.0%

Question 17

Our task is to measure the volume of blood in an elephant. One way to do this would be to drain its blood into a suitable container. Aside from harmful side effects which this method has on the elephant, it will not be successful, as blood will still remain behind in the tissues. Hence, we will inject 2.00 ml of a 2.00 M solution of a dye which the elephant will not appreciably metabolize or excrete in one hour and then measure the concentration of this dye in the bloodstream (our sample being taken from another leg than the point of injection) after 30 minutes, a sufficient time to thoroughly mix the dye in the bloodstream. The concentration of dye at this point is 1.25 x 10-5 M. What is the volume of blood in the elephant?

Accepted Answer

A)  320. L 
B)  320000 L 
C)  3.2 L 
D)  80 L 
E)  800 L 
A)  320. L 
B)  320000 L 
C)  3.2 L 
D)  80 L 
E)  800 L

Question 18

Gases emitted during volcanic activity often contain high concentrations of hydrogen sulfide and sulfur dioxide. These gases may react to produce deposits of sulfur according to the equation: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g)
For the complete reaction of 6.41 mol of hydrogen sulfide:

Accepted Answer

A)  308 g of sulfur is formed 
B)  410 g of sulfur dioxide is consumed 
C)  231 g of water vapor is produced 
D)  320 g of total products result 
E)  628 g of total reactants are consumed 
A)  308 g of sulfur is formed 
B)  410 g of sulfur dioxide is consumed 
C)  231 g of water vapor is produced 
D)  320 g of total products result 
E)  628 g of total reactants are consumed

Question 19

One source of iodine is sodium iodate. Iodine is produced by a series of reactions. The first reaction is a reduction reaction with sodium hydrogen sulfite. IO3- (aq) + 3 HSO3- (aq) → I- (aq) + 3 SO42- (aq) + 3 H+ (aq)
5 I- (aq) + IO3- (aq) + 6 H+ (aq) → 3 I2(s) + 3 H2O
How many grams of iodine are produced from 1.00 × 102 grams of NaHSO3?

Accepted Answer

A)  81.3 g 
B)  243 g 
C)  62.6 g 
D)  48.8 g 
E)  205 g 
A)  81.3 g 
B)  243 g 
C)  62.6 g 
D)  48.8 g 
E)  205 g

Question 20

How much Cl2, in g, is required to produce 12.0 g CCl4 according to the following reaction? CH4 + 4 Cl2 → CCl4 + 4 HCl

Accepted Answer

A)  12.0 g 
B)  5.52 g 
C)  22.1 g 
D)  1.38 g 
E)  11.0 g 
A)  12.0 g 
B)  5.52 g 
C)  22.1 g 
D)  1.38 g 
E)  11.0 g

Exam 4: Chemical Reactions

How many mL of 0.024 M solution can be produced from 14.1 mL of 3.0 M solution?

What is the molarity of methanol, CH3OH (d = 0792 g/mL), if 150.0 mL is dissolved in enough water to make 4.00 L of solution?

The reactant that is in excess determines the amount of products formed.

When the equation CS2 + Cl2 → CCl4 + S2Cl2 is balanced with the smallest integer coefficients, the sum of the coefficients is:

Given the reaction: 2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O How many moles of I2 are produced by reacting 28.0 g KMnO4, 18.0 g KI, and 46.0 g H2SO4?

If an aqueous solution containing 46 g of sodium carbonate per liter is mixed with an equal volume of 0.20 M aqueous hydrochloric acid, what would be the molarity of sodium chloride in the final solution, assuming volumes were additive?

If 85.6 mL of a 6.75 M solution are diluted to 6.20 L with water, what is the concentration of the final solution?

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? CH3OH → CO + H2

Potassium superoxide (KO2) can simulate a plant-type action by consuming carbon dioxide (CO2) gas and releasing oxygen (O2) gas. The other product is potassium carbonate (K2CO3). When the equation for this process is balanced, it shows that:

Cryolite is a compound needed for the Hall-Heroult process for producing aluminum. Cryolite is produced by the following reaction: 6 HF + Al(OH)3 + 3 NaOH → Na3AlF6 + 6 H2O How many grams of cryolite are produced if the reaction has a 94.3% yield and a limiting reagent of 27.8 grams of HF?

What is the sum of the coefficients when the following equation is balanced with the smallest integer coefficients? H2SO3 + Al(OH)3 → Al2(SO3)3 + H2O

A chemical equation is a shorthand way of representing a chemical reaction.

A 1.900 g sample of C6H12 is burned in an excess of oxygen. What mass of CO2 and H2O should be obtained?

Iron metal reacts with chlorine gas as follows: 2 Fe(s) + 3 Cl2(g) → 2 FeCl3(s) How many moles of FeCl3 are obtained when 4.6 mol of Cl2 reacts with excess Fe?

In the following reaction: 2 KClO3(s) → 2 KCl(s) + 3 O2(g) 14.0 g KClO3 yielded 1.40 g KCl. What is the percent yield?

Gases emitted during volcanic activity often contain high concentrations of hydrogen sulfide and sulfur dioxide. These gases may react to produce deposits of sulfur according to the equation: 2 H2S(g) + SO2(g) → 3 S(s) + 2 H2O(g) For the complete reaction of 6.41 mol of hydrogen sulfide:

How much Cl2, in g, is required to produce 12.0 g CCl4 according to the following reaction? CH4 + 4 Cl2 → CCl4 + 4 HCl

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

What is the molarity of methanol, CH₃OH (d = 0792 g/mL), if 150.0 mL is dissolved in enough water to make 4.00 L of solution?

When the equation CS₂ + Cl₂ → CCl₄ + S₂Cl₂ is balanced with the smallest integer coefficients, the sum of the coefficients is:

Given the reaction: 2 KMnO₄ + 10 KI + 8 H₂SO₄ → 6 K₂SO₄ + 2 MnSO₄ + 5 I₂ + 8 H₂O How many moles of I2 are produced by reacting 28.0 g KMnO₄, 18.0 g KI, and 46.0 g H₂SO₄?

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? CH₃OH → CO + H₂

Potassium superoxide (KO₂) can simulate a plant-type action by consuming carbon dioxide (CO₂) gas and releasing oxygen (O₂) gas. The other product is potassium carbonate (K₂CO₃). When the equation for this process is balanced, it shows that:

What is the sum of the coefficients when the following equation is balanced with the smallest integer coefficients? H₂SO₃ + Al(OH)₃ → Al₂(SO₃)₃ + H₂O

A 1.900 g sample of C₆H₁₂ is burned in an excess of oxygen. What mass of CO₂ and H₂O should be obtained?

Iron metal reacts with chlorine gas as follows: 2 Fe(s) + 3 Cl₂(g) → 2 FeCl₃(s) How many moles of FeCl₃ are obtained when 4.6 mol of Cl₂ reacts with excess Fe?

In the following reaction: 2 KClO₃(s) → 2 KCl(s) + 3 O₂(g) 14.0 g KClO₃ yielded 1.40 g KCl. What is the percent yield?

Gases emitted during volcanic activity often contain high concentrations of hydrogen sulfide and sulfur dioxide. These gases may react to produce deposits of sulfur according to the equation: 2 H₂S(g) + SO₂(g) → 3 S(s) + 2 H₂O(g) For the complete reaction of 6.41 mol of hydrogen sulfide:

How much Cl₂, in g, is required to produce 12.0 g CCl₄ according to the following reaction? CH₄ + 4 Cl₂ → CCl₄ + 4 HCl