Question 1

How many moles of HCl are represented by 1.0 * 1019 HCl molecules

Accepted Answer

A)  1.7 * 10-5 mol 
B)  1.5 * 10-3 mol 
C)  1.0 * 1019 mol 
D)  37 mol 
E)  6.0 * 104 mol 
A)  1.7 * 10-5 mol 
B)  1.5 * 10-3 mol 
C)  1.0 * 1019 mol 
D)  37 mol 
E)  6.0 * 104 mol

Question 2

A sample of aluminum metal is placed in a graduated cylinder. It is noted that 5.50 mL of water is displaced by the aluminum. The aluminum is then reacted with excess nitric acid to produce aluminum nitrate and hydrogen gas. Given the density for aluminum is 2.702 g/mL, how many grams of aluminum nitrate are produced in the reaction
2Al(s) + 6HNO3(aq) $\rarr$ 2Al(NO3)3(aq) + 3H2(g)

Accepted Answer

A)  161 g 
B)  11.0 g 
C)  14.9 g 
D)  117 g 
E)  235 g 
A)  161 g 
B)  11.0 g 
C)  14.9 g 
D)  117 g 
E)  235 g

Question 3

The mineral orpiment, having the empirical formula As2S3, was used in ancient times as a cosmetic. What mass of arsenic is present in 5.0 g of orpiment [Given: naturally occurring arsenic is all arsenic-75; assume that all naturally occurring sulfur is sulfur-32 (only approximately true)]

Accepted Answer

A)  0.61 g 
B)  3.0 g 
C)  1.5 g 
D)  2.0 g 
E)  3.5 g 
A)  0.61 g 
B)  3.0 g 
C)  1.5 g 
D)  2.0 g 
E)  3.5 g

Question 4

Ammonia reacts with oxygen to form nitric oxide and water vapor: 
4NH3 + 5O2 $\rarr$ 4NO + 6H2O
When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent

Accepted Answer

A)  NH3 
B)  O2 
C)  NO 
D)  H2O 
E)  No reagent is limiting. 
A)  NH3 
B)  O2 
C)  NO 
D)  H2O 
E)  No reagent is limiting.

Question 5

Calculate the number of moles of xenon in 12.0 g of xenon.

Accepted Answer

A)  1.00 mol 
B)  0.0457 mol 
C)  0.183 mol 
D)  7.62 * 10-3 mol 
E)  0.0914 mol 
A)  1.00 mol 
B)  0.0457 mol 
C)  0.183 mol 
D)  7.62 * 10-3 mol 
E)  0.0914 mol

Question 6

The reaction of 44.1 g of Cr2O3 with 35.0 g of Al produced 25.6 g of Cr. What is the percent yield for this reaction
2Al + Cr2O3 $\rarr$Al2O3 + 2Cr

Accepted Answer

A)  37.9 % 
B)  58.0 % 
C)  73.1 % 
D)  84.9% 
E)  100. % 
A)  37.9 % 
B)  58.0 % 
C)  73.1 % 
D)  84.9% 
E)  100. %

Question 7

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 moles of V2O5 with 6.0 moles of calcium based on the chemical reaction below
V2O5(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

Accepted Answer

A)  1.0 mol 
B)  1.6 mol 
C)  2.0 mol 
D)  2.4 mol 
E)  4.0 mol 
A)  1.0 mol 
B)  1.6 mol 
C)  2.0 mol 
D)  2.4 mol 
E)  4.0 mol

Question 8

Washing soda is a hydrate of sodium carbonate. Elemental analysis of a sample of washing soda gave 4.20% C and 7.05% H. What is the formula for washing soda

Accepted Answer

A)  Na2CO3 * 2H2O 
B)  Na2CO3 * 4H2O 
C)  Na2CO3 * 6H2O 
D)  Na2CO3 * 8H2O 
E)  Na2CO3 * H2O 
A)  Na2CO3 * 2H2O 
B)  Na2CO3 * 4H2O 
C)  Na2CO3 * 6H2O 
D)  Na2CO3 * 8H2O 
E)  Na2CO3 * H2O

Question 9

Calculate the molecular mass of ethylene glycol, C2H6O2, a compound frequently used as automobile antifreeze.

Accepted Answer

A)  54.4 g 
B)  59.0 g 
C)  62.1 g 
D)  71.9 g 
E)  None of the above 
A)  54.4 g 
B)  59.0 g 
C)  62.1 g 
D)  71.9 g 
E)  None of the above

Question 10

If 0.66 mole of a substance has a mass of 99 g, what is the molecular mass of the substance

Accepted Answer

A)  120 g 
B)  150 g 
C)  170 g 
D)  180 g 
E)  None of the above 
A)  120 g 
B)  150 g 
C)  170 g 
D)  180 g 
E)  None of the above

Question 11

What is the minimum mass of sulfur dioxide necessary to produce 200. g of sulfuric acid in the following reaction?
2SO2 + O2 + 2H2O$\rarr$ 2H2SO4

Accepted Answer

A)  141 g 
B)  131 g 
C)  121 g 
D)  111 g 
E)  None of the above 
A)  141 g 
B)  131 g 
C)  121 g 
D)  111 g 
E)  None of the above

Question 12

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper
Cu + 2 AgNO3 $\rarr$  Cu(NO3 )2 + 2 Ag

Accepted Answer

A)  2349 g 
B)  2359 g 
C)  2369 g 
D)  2379 g 
E)  None of the above 
A)  2349 g 
B)  2359 g 
C)  2369 g 
D)  2379 g 
E)  None of the above

Question 13

Calculate the molar mass of Ba(NO3)2.

Accepted Answer

A)  199.3 g/mol 
B)  323.3 g/mol 
C)  247.3 g/mol 
D)  261.3 g/mol 
E)  398.6 g/mol 
A)  199.3 g/mol 
B)  323.3 g/mol 
C)  247.3 g/mol 
D)  261.3 g/mol 
E)  398.6 g/mol

Question 14

What is the average mass, in grams, of one Zn atom

Accepted Answer

A)  65.39 amu 
B)  65.39 g 
C)  3.94 x 1025g 
D)  1.09 x 10-22 g 
E)  1.661 x 10-24g 
A)  65.39 amu 
B)  65.39 g 
C)  3.94 x 1025g 
D)  1.09 x 10-22 g 
E)  1.661 x 10-24g

Question 15

Ferrocene, Fe(C5H5)2(s), can be prepared by reacting 3.0 g of FeCl2(s) with an equal mass of cyclopentadiene, C5H6(l), and an excess of KOH, as shown in the following reaction FeCl2 + 2C5H6 + 2KOH $\rarr$  FeC10H10 + 2H2O
A student who carried out this reaction obtained 2.7 g of ferrocene. Of the following choices which has three correct answers?

Accepted Answer

A)  C5H6 is limiting; 5.2 g of ferrocene could be theoretically formed; obtained 64 % yield 
B)  FeCl2 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 59 % yield 
C)  C5H6 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 54 % yield 
D)  C5H6 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 64 % yield 
E)  None of the choices have three correct responses 
A)  C5H6 is limiting; 5.2 g of ferrocene could be theoretically formed; obtained 64 % yield 
B)  FeCl2 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 59 % yield 
C)  C5H6 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 54 % yield 
D)  C5H6 is limiting; 4.2 g of ferrocene could be theoretically formed; obtained 64 % yield 
E)  None of the choices have three correct responses

Question 16

Aluminum metal reacts with nitric acid to produce aluminum nitrate and hydrogen gas. Identify the balanced reaction that describes this process.

Accepted Answer

A)  Al + HNO3 $\rarr$ AlNO3 + H2 
B)  Al + HNO3 $\rarr$ AlNO3 + H 
C)  Al + 2HNO3 $\rarr$ Al(NO3)2 + H2 
D)  Al + 3HNO3 $\rarr$ Al(NO3)3 + H2 
E)  2Al + 6HNO3 $\rarr$ 2Al(NO3)3 + 3H2 
A)  Al + HNO3 $\rarr$ AlNO3 + H2 
B)  Al + HNO3 $\rarr$ AlNO3 + H 
C)  Al + 2HNO3 $\rarr$ Al(NO3)2 + H2 
D)  Al + 3HNO3 $\rarr$ Al(NO3)3 + H2 
E)  2Al + 6HNO3 $\rarr$ 2Al(NO3)3 + 3H2

Question 17

In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia. How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed

Accepted Answer

A)  0.22 kg hydrogen required, 2.1 kg ammonia produced 
B)  0.22 kg hydrogen required, 1.2 kg ammonia produced 
C)  0.42 kg hydrogen required, 2.1 kg ammonia produced 
D)  0.32 kg hydrogen required, 1.2 kg ammonia produced 
E)  None of the above have both values correct 
A)  0.22 kg hydrogen required, 2.1 kg ammonia produced 
B)  0.22 kg hydrogen required, 1.2 kg ammonia produced 
C)  0.42 kg hydrogen required, 2.1 kg ammonia produced 
D)  0.32 kg hydrogen required, 1.2 kg ammonia produced 
E)  None of the above have both values correct

Question 18

What is the coefficient of H2O when the following equation is properly balanced
___ Al4C3 + ___ H2O $\rarr$ ___ Al(OH)3 + ___ CH4

Accepted Answer

A)  3 
B)  4 
C)  6 
D)  12 
E)  24 
A)  3 
B)  4 
C)  6 
D)  12 
E)  24

Question 19

A compound with an empirical formula of C2H2Br3 has a molar mass of 531.47 g/mol. What is the molecular formula

Accepted Answer

A)  C2H2Br3 
B)  C4H4Br6 
C)  CHBr 
D)  C4H4Br3 
E)  C6H6Br9 
A)  C2H2Br3 
B)  C4H4Br6 
C)  CHBr 
D)  C4H4Br3 
E)  C6H6Br9

Question 20

What is the theoretical yield of PI3 from the reaction of 27.0 g of P and 68.0 g of I2
2P(s) + 3I2(s) $\rarr$2PI3(s)

Accepted Answer

A)  70.5 g 
B)  71.5 g 
C)  73.5 g 
D)  75.5 g 
E)  None of the above 
A)  70.5 g 
B)  71.5 g 
C)  73.5 g 
D)  75.5 g 
E)  None of the above

Exam 3: Mass Relationships in Chemical Reactions

How many moles of HCl are represented by 1.0 * 1019 HCl molecules

The mineral orpiment, having the empirical formula As2S3, was used in ancient times as a cosmetic. What mass of arsenic is present in 5.0 g of orpiment [Given: naturally occurring arsenic is all arsenic-75; assume that all naturally occurring sulfur is sulfur-32 (only approximately true)]

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 →\rarr→ 4NO + 6H2O When 40.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent

Calculate the number of moles of xenon in 12.0 g of xenon.

The reaction of 44.1 g of Cr2O3 with 35.0 g of Al produced 25.6 g of Cr. What is the percent yield for this reaction 2Al + Cr2O3 →\rarr→ Al2O3 + 2Cr

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 moles of V2O5 with 6.0 moles of calcium based on the chemical reaction below V2O5(s) + 5Ca(l) →\rarr→ 2V(l) + 5CaO(s)

Washing soda is a hydrate of sodium carbonate. Elemental analysis of a sample of washing soda gave 4.20% C and 7.05% H. What is the formula for washing soda

Calculate the molecular mass of ethylene glycol, C2H6O2, a compound frequently used as automobile antifreeze.

If 0.66 mole of a substance has a mass of 99 g, what is the molecular mass of the substance

What is the minimum mass of sulfur dioxide necessary to produce 200. g of sulfuric acid in the following reaction? 2SO2 + O2 + 2H2O →\rarr→ 2H2SO4

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper Cu + 2 AgNO3 →\rarr→ Cu(NO3 )2 + 2 Ag

Calculate the molar mass of Ba(NO3)2.

What is the average mass, in grams, of one Zn atom

Aluminum metal reacts with nitric acid to produce aluminum nitrate and hydrogen gas. Identify the balanced reaction that describes this process.

In the Haber process, hydrogen gas reacts with nitrogen gas to produce ammonia. How many kilograms of hydrogen would be required to react completely with 1.0 kg of nitrogen, and how many kilograms of ammonia would be formed

What is the coefficient of H2O when the following equation is properly balanced ___ Al4C3 + ___ H2O →\rarr→ ___ Al(OH)3 + ___ CH4

A compound with an empirical formula of C2H2Br3 has a molar mass of 531.47 g/mol. What is the molecular formula

What is the theoretical yield of PI3 from the reaction of 27.0 g of P and 68.0 g of I2 2P(s) + 3I2(s) →\rarr→ 2PI3(s)

Chemistry: The Study of Change

Atoms Molecules and Ions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

How many moles of HCl are represented by 1.0 * 10¹⁹ HCl molecules

The mineral orpiment, having the empirical formula As₂S₃, was used in ancient times as a cosmetic. What mass of arsenic is present in 5.0 g of orpiment [Given: naturally occurring arsenic is all arsenic-75; assume that all naturally occurring sulfur is sulfur-32 (only approximately true)]

Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH₃ + 5O₂ $\rarr$ 4NO + 6H₂O When 40.0 g NH₃ and 50.0 g O₂ are allowed to react, which is the limiting reagent

The reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al produced 25.6 g of Cr. What is the percent yield for this reaction 2Al + Cr₂O₃ $\rarr$ Al₂O₃ + 2Cr

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 moles of V₂O₅ with 6.0 moles of calcium based on the chemical reaction below V₂O₅(s) + 5Ca(l) $\rarr$ 2V(l) + 5CaO(s)

Calculate the molecular mass of ethylene glycol, C₂H₆O₂, a compound frequently used as automobile antifreeze.

What is the minimum mass of sulfur dioxide necessary to produce 200. g of sulfuric acid in the following reaction? 2SO₂ + O₂ + 2H₂O $\rarr$ 2H₂SO₄

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper Cu + 2 AgNO₃ $\rarr$ Cu(NO₃ )₂ + 2 Ag

Calculate the molar mass of Ba(NO₃)₂.

What is the coefficient of H₂O when the following equation is properly balanced _ Al₄C₃ + _ H₂O $\rarr$ _ Al(OH)₃ + _ CH₄

A compound with an empirical formula of C₂H₂Br₃ has a molar mass of 531.47 g/mol. What is the molecular formula

What is the theoretical yield of PI₃ from the reaction of 27.0 g of P and 68.0 g of I₂ 2P(s) + 3I₂(s) $\rarr$ 2PI₃(s)