An important reaction sequence in the industrial production of nitric acid is the following: N2(g) + 3H2(g) F1F1F1S1F1F1F10 2NH3(g) 4NH3(g) + 5O2(g) F1F1F1S1F1F1F10 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?

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

The number of hydrogen atoms in 0.050 mol of C3H8O3 is

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. 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.

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g) F1F1F1S1F1F1F10 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% A) 57.5% B) 48.8% C) 38.0% D) 32.4% E) 16.3%

Balance the following equation: Ca3(PO4)2(s) + SiO2(s) + C(s) F1F1F1S1F1F1F10 CaSiO3(s) + CO(g) + P4(s)

A) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 8CO(g) + P4(s) B) Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 14CO(g) + P4(s) C) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 8CO(g) + 2P4(s) D) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) F1F1F1S1F1F1F10 6CaSiO3(s) + 10CO(g) + P4(s) E) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) F1F1F1S1F1F1F10 6CaSiO3(s) + 10CO(g) + 4P4(s) A) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 8CO(g) + P4(s) B) Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 14CO(g) + P4(s) C) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) F1F1F1S1F1F1F10 3CaSiO3(s) + 8CO(g) + 2P4(s) D) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) F1F1F1S1F1F1F10 6CaSiO3(s) + 10CO(g) + P4(s) E) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) F1F1F1S1F1F1F10 6CaSiO3(s) + 10CO(g) + 4P4(s)

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

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

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4F1F1F1S1F1F1F10r3/3; density of mercury = 13.6 g/cm3)

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

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) F1F1F1S1F1F1F10 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 A) 68.5 g MgCl2 B) 77.0 g MgCl2 C) 71.4 g MgCl2 D) 107 g MgCl2 E) 154 g MgCl2

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

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

Exam 3: Stoichiometry of Formulas and Equations

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?

(Multiple Choice)

4.8/5

(34)

Question 21

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

(Multiple Choice)

4.7/5

(42)

Question 22

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?

(Multiple Choice)

4.8/5

(36)

Question 23

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 NH₃are needed to react completely with 13.6 mol of F₂?

(Multiple Choice)

4.9/5

(36)

Question 24

The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is

(Multiple Choice)

4.8/5

(34)

Question 25

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?

(Essay)

4.8/5

(40)

Question 26

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?

(Multiple Choice)

4.8/5

(51)

Question 27

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

(Multiple Choice)

4.8/5

(37)

Question 28

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.

(Multiple Choice)

4.8/5

(33)

Question 29

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

(Multiple Choice)

4.8/5

(47)

Question 30

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)

(Multiple Choice)

4.9/5

(39)

Question 31

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 CO₂and 0.226 g H₂O. If its molar mass is between 158 and 167 g/mol, what is its molecular formula?

(Multiple Choice)

5.0/5

(43)

Question 32

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

(Essay)

4.8/5

(32)

Question 33

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.

(Multiple Choice)

4.8/5

(39)

Question 34

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?

(Short Answer)

5.0/5

(37)

Question 35

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 ( = 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?

(Multiple Choice)

4.9/5

(41)

Question 36

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)

(Essay)

4.9/5

(36)

Question 37

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

(Multiple Choice)

4.9/5

(32)

Question 38

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.

(Multiple Choice)

4.8/5

(39)

Question 39

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

(True/False)

4.7/5

(39)

Question 40

Showing 21 - 40 of 87

Exam 3: Stoichiometry of Formulas and Equations

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?

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

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?

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?

The number of hydrogen atoms in 0.050 mol of C3H8O3 is

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?

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?

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

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.

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

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)

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

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.

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?

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)

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

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.

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

Keys to the Study of Chemistry

The Components of Matter

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

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

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?

The number of hydrogen atoms in 0.050 mol of C₃H₈O₃ is

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?

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?

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

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.

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

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)

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

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.

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)

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

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.