Question 1

Propane, C3H8, is commonly provided as a bottled gas for use as a fuel. In 0.200 mol of propane
a. what is the mass of propane?
b. what mass of carbon is present?
c. how many molecules of C3H8 are present?
d. how many hydrogen atoms are present?

Accepted Answer

a. 8.82 g
b. 7.21 g
...

Question 2

Calculate the molar mass of Ca(BO2) 2·6H2O.

Accepted Answer

A)   273.87 g/mol
B)   233.79 g/mol
C)   183.79 g/mol
D)   174.89 g/mol
E)   143.71 g/molF) B) and E)
G) A) and B)

Question 3

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4r3/3; density of mercury = 13.6 g/cm3)

Accepted Answer

A)   2.1 × 1019
B)   1.7 × 1020
C)   2.1 × 1022
D)   1.7 × 1023
E)   none of the aboveF) B) and D)
G) All of the above

Question 4

Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

Accepted Answer

A)   2.377 mol
B)   2.146 mol
C)   1.105 mol
D)   0.4660 mol
E)   0.4207 molF) D) and E)
G) B) and C)

Question 5

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 1020 molecules of SO3.

Accepted Answer

A)   6.06 × 10-4 g
B)   2.91 × 10-2 g
C)   4.85 × 10-2 g
D)   20.6 g
E)   1650 gF) A) and E)
G) B) and E)

Question 6

The number of hydrogen atoms in 0.050 mol of C3H8O3 is

Accepted Answer

A)   3.0 × 1022 H atoms.
B)   1.2 × 1023 H atoms.
C)   2.4 × 1023 H atoms.
D)   4.8 × 1023 H atoms.
E)   none of the above.F) A) and B)
G) A) and D)

Question 7

Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. If its molar mass is between 158 and 167 g/mol, what is its molecular formula?

Accepted Answer

A)   C4H6O7
B)   C6H8O5
C)   C7H12O4
D)   C4H3O2
E)   C8H6O4F) D) and E)
G) A) and B)

Question 8

Constitutional (structural) isomers have the same molecular formula but different structural formulas.

Accepted Answer

A) True 
 B)False

Question 9

Ammonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in production of aluminum, in uranium processing, and in frosting of light bulbs) . 2NH3(g)  + 5F2(g)   N2F4(g)  + 6HF(g) 
How many moles of NH3 are needed to react completely with 13.6 mol of F2?

Accepted Answer

A)   34.0 mol
B)   27.2 mol
C)   6.80 mol
D)   5.44 mol
E)   2.27 molF) D) and E)
G) A) and C)

Question 10

Balance the following equation: 
Ca3(PO4) 2(s)  + SiO2(s)  + C(s)   CaSiO3(s)  + CO(g)  + P4(s)

Accepted Answer

A)   Ca3(PO4) 2(s)  + 3SiO2(s)  + 8C(s)   3CaSiO3(s)  + 8CO(g)  + P4(s) 
B)   Ca3(PO4) 2(s)  + 3SiO2(s)  + 14C(s)   3CaSiO3(s)  + 14CO(g)  + P4(s) 
C)   Ca3(PO4) 2(s)  + 3SiO2(s)  + 8C(s)   3CaSiO3(s)  + 8CO(g)  + 2P4(s) 
D)   2Ca3(PO4) 2(s)  + 6SiO2(s)  + 10C(s)   6CaSiO3(s)  + 10CO(g)  + P4(s) 
E)   2Ca3(PO4) 2(s)  + 6SiO2(s)  + 10C(s)   6CaSiO3(s)  + 10CO(g)  + 4P4(s) F) A) and E)
G) All of the above

Question 11

Balance the following equation for partial oxidation of ammonia, an important reaction in the production of nitric acid:
NH3(g) + O2(g) F1F1F1S1F1F1F10 NO(g) + H2O(l)

Accepted Answer

4NH₃(g) + 5...

Question 12

Aluminum sulfate, Al2(SO4) 3, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

Accepted Answer

A)   450.06 g/mol
B)   342.15 g/mol
C)   315.15 g/mol
D)   278.02 g/mol
E)   74.98 g/molF) A) and B)
G) C) and D)

Question 13

Balance the equation
B2O3(s) + NaOH(aq) F1F1F1S1F1F1F10 Na3BO3(aq) + H2O(l)

Accepted Answer

B₂O₃(s) + 6NaOH(aq) F1...

Question 14

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula?

Accepted Answer

The answer of Analysis of a white solid produced in...

Question 15

In the combustion analysis of 0.1127 g of glucose (C6H12O6) , what mass, in grams, of CO2 would be produced?

Accepted Answer

A)   0.0451 g
B)   0.0825 g
C)   0.1652 g
D)   0.4132 g
E)   1.466 gF) B) and E)
G) A) and D)

Question 16

An important reaction sequence in the industrial production of nitric acid is the following: N2(g)   + 3H2(g)   2NH3(g) 
4NH3(g)  + 5O2(g)   4NO(g)  + 6H2O(l) 
Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

Accepted Answer

A)   12.5 mol O2
B)   20.0 mol O2
C)   25.0 mol O2
D)   50.0 mol O2
E)  100. mol O2F) A) and E)
G) A) and D)

Question 17

Lead (II)  nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO3) 2.

Accepted Answer

A)   107 g
B)   90.8 g
C)   87.0 g
D)   83.4 g
E)   62.6 gF) B) and C)
G) C) and D)

Question 18

Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

Accepted Answer

A)   NH2O5
B)   N2H4O4
C)   N3H3O3
D)   N4H8O2
E)   N2H2O4F) A) and B)
G) All of the above

Question 19

Magnesium reacts with iron(III)  chloride to form magnesium chloride (which can be used in fireproofing wood and in disinfectants)  and iron. 3Mg(s)  + 2FeCl3(s)   3MgCl2(s)  + 2Fe(s) 
A mixture of 41.0 g of magnesium ( 3(s)   3MgCl2(s)  + 2Fe(s)  A mixture of 41.0 g of magnesium (   = 24.31 g/mol)  and 175 g of iron(III)  chloride (   = 162.2 g/mol)  is allowed to react. What mass of magnesium chloride = 95.21 g/mol)  is formed? A)  68.5 g MgCl2 B)  77.0 g MgCl2 C)  71.4 g MgCl2 D)  107 g MgCl2 E)  154 g MgCl2" class="answers-bank-image d-inline" rel="preload" > = 24.31 g/mol)  and 175 g of iron(III)  chloride ( 3(s)   3MgCl2(s)  + 2Fe(s)  A mixture of 41.0 g of magnesium (   = 24.31 g/mol)  and 175 g of iron(III)  chloride (   = 162.2 g/mol)  is allowed to react. What mass of magnesium chloride = 95.21 g/mol)  is formed? A)  68.5 g MgCl2 B)  77.0 g MgCl2 C)  71.4 g MgCl2 D)  107 g MgCl2 E)  154 g MgCl2" class="answers-bank-image d-inline" rel="preload" > = 162.2 g/mol)  is allowed to react. What mass of magnesium chloride = 95.21 g/mol)  is formed?

Accepted Answer

A)   68.5 g MgCl2
B)   77.0 g MgCl2
C)   71.4 g MgCl2
D)   107 g MgCl2
E)   154 g MgCl2F) A) and B)
G) B) and C)

Question 20

Tetraphosphorus hexaoxide ( 4(s)  + 3O2(g)   P4O6(s)  If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction? A)  57.5% B)  48.8% C)  38.0% D)  32.4% E)  16.3%" class="answers-bank-image d-inline" rel="preload" > = 219.9 g/mol)  is formed by the reaction of phosphorus with oxygen gas. P4(s)  + 3O2(g)   P4O6(s) 
If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?

Accepted Answer

A)   57.5%
B)   48.8%
C)   38.0%
D)   32.4%
E)   16.3%F) All of the above
G) A) and B)

Exam 3: Stoichiometry of Formulas and Equations

In the combustion analysis of 0.1127 g of glucose (C₆H₁₂O₆) , what mass, in grams, of CO₂ would be produced?

Correct Answer
verified

Balance the following equation: Ca₃(PO₄) ₂(s) + SiO₂(s) + C(s)  CaSiO₃(s) + CO(g) + P₄(s)

Correct Answer
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Calculate the molar mass of Ca(BO₂) ₂·6H₂O.

Correct Answer
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Aluminum sulfate, Al₂(SO₄) ₃, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

Correct Answer
verified

Balance the following equation for partial oxidation of ammonia, an important reaction in the production of nitric acid: NH₃(g) + O₂(g)  NO(g) + H₂O(l)

Correct Answer
verified
4NH₃(g) + 5...
View Answer

Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO₃) ₂.

Correct Answer
verified

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula?

Correct Answer
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Correct Answer
verified

Propane, C₃H₈, is commonly provided as a bottled gas for use as a fuel. In 0.200 mol of propane a. what is the mass of propane? b. what mass of carbon is present? c. how many molecules of C₃H₈ are present? d. how many hydrogen atoms are present?

Correct Answer
verified
a. 8.82 g
b. 7.21 g
...
View Answer

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4r³/3; density of mercury = 13.6 g/cm³)

Correct Answer
verified

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g)  P₄O₆(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

Correct Answer
verified

Constitutional (structural) isomers have the same molecular formula but different structural formulas.

Correct Answer
verified

Aluminum oxide, Al₂O₃, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al₂O₃.

Correct Answer
verified

Correct Answer
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Correct Answer
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Balance the equation B₂O₃(s) + NaOH(aq)  Na₃BO₃(aq) + H₂O(l)

Correct Answer
verified
B₂O₃(s) + 6NaOH(aq) F1...
View Answer

The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is

Correct Answer
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Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

Correct Answer
verified

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 10²⁰ molecules of SO₃.

Correct Answer
verified

An important reaction sequence in the industrial production of nitric acid is the following: N₂(g) + 3H₂(g)  2NH₃(g) 4NH₃(g) + 5O₂(g)  4NO(g) + 6H₂O(l) Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

Correct Answer
verified

Exam 3: Stoichiometry of Formulas and Equations

In the combustion analysis of 0.1127 g of glucose (C6H12O6) , what mass, in grams, of CO2 would be produced?

Correct AnswerverifiedShow Answer

Balance the following equation: Ca3(PO4) 2(s) + SiO2(s) + C(s)  CaSiO3(s) + CO(g) + P4(s)

Correct AnswerverifiedShow Answer

Calculate the molar mass of Ca(BO2) 2·6H2O.

Correct AnswerverifiedShow Answer

Aluminum sulfate, Al2(SO4) 3, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

Correct AnswerverifiedShow Answer

Balance the following equation for partial oxidation of ammonia, an important reaction in the production of nitric acid: NH3(g) + O2(g)  NO(g) + H2O(l)

Correct Answerverified4NH3(g) + 5...View AnswerShow Answer

Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO3) 2.

Correct AnswerverifiedShow Answer

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula?

Correct AnswerverifiedShow Answer

Ammonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in production of aluminum, in uranium processing, and in frosting of light bulbs) . 2NH3(g) + 5F2(g)  N2F4(g) + 6HF(g) How many moles of NH3 are needed to react completely with 13.6 mol of F2?

Correct AnswerverifiedShow Answer

Propane, C3H8, is commonly provided as a bottled gas for use as a fuel. In 0.200 mol of propane a. what is the mass of propane? b. what mass of carbon is present? c. how many molecules of C3H8 are present? d. how many hydrogen atoms are present?

Correct Answerverifieda. 8.82 gb. 7.21 g...View AnswerShow Answer

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4r3/3; density of mercury = 13.6 g/cm3)

Correct AnswerverifiedShow Answer

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g)  P4O6(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?

Correct AnswerverifiedShow Answer

Constitutional (structural) isomers have the same molecular formula but different structural formulas.

Correct AnswerverifiedShow Answer

Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Balance the equation B2O3(s) + NaOH(aq)  Na3BO3(aq) + H2O(l)

Correct AnswerverifiedB2O3(s) + 6NaOH(aq) F1...View AnswerShow Answer

The number of hydrogen atoms in 0.050 mol of C3H8O3 is

Correct AnswerverifiedShow Answer

Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

Correct AnswerverifiedShow Answer

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 1020 molecules of SO3.

Correct AnswerverifiedShow Answer

An important reaction sequence in the industrial production of nitric acid is the following: N2(g) + 3H2(g)  2NH3(g) 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(l) Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

Correct AnswerverifiedShow Answer

In the combustion analysis of 0.1127 g of glucose (C₆H₁₂O₆) , what mass, in grams, of CO₂ would be produced?

Correct Answer
verified

Balance the following equation: Ca₃(PO₄) ₂(s) + SiO₂(s) + C(s)  CaSiO₃(s) + CO(g) + P₄(s)

Correct Answer
verified

Calculate the molar mass of Ca(BO₂) ₂·6H₂O.

Correct Answer
verified

Aluminum sulfate, Al₂(SO₄) ₃, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

Correct Answer
verified

Balance the following equation for partial oxidation of ammonia, an important reaction in the production of nitric acid: NH₃(g) + O₂(g)  NO(g) + H₂O(l)

Correct Answer
verified
4NH₃(g) + 5...
View Answer

Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO₃) ₂.

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Propane, C₃H₈, is commonly provided as a bottled gas for use as a fuel. In 0.200 mol of propane a. what is the mass of propane? b. what mass of carbon is present? c. how many molecules of C₃H₈ are present? d. how many hydrogen atoms are present?

Correct Answer
verified
a. 8.82 g
b. 7.21 g
...
View Answer

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4r³/3; density of mercury = 13.6 g/cm³)

Correct Answer
verified

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g)  P₄O₆(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

Correct Answer
verified

Correct Answer
verified

Aluminum oxide, Al₂O₃, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al₂O₃.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Balance the equation B₂O₃(s) + NaOH(aq)  Na₃BO₃(aq) + H₂O(l)

Correct Answer
verified
B₂O₃(s) + 6NaOH(aq) F1...
View Answer

The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is

Correct Answer
verified

Correct Answer
verified

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 10²⁰ molecules of SO₃.

Correct Answer
verified

An important reaction sequence in the industrial production of nitric acid is the following: N₂(g) + 3H₂(g)  2NH₃(g) 4NH₃(g) + 5O₂(g)  4NO(g) + 6H₂O(l) Starting from 20.0 mol of nitrogen gas in the first reaction, how many moles of oxygen gas are required in the second one?

Correct Answer
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