You create a process to be used in conjunction with combustion analysis using chlorine gas to determine the amount of selenium in certain organic compounds.If there is selenium in the molecule, SeCl2 (149.87 g/mol) is produced.Analysis of 28.20 g of an unknown compound produces 36.21 g CO2, 18.53 g H2O, and 30.83 g SeCl2.The molar mass of the compound is about 137 g/mol.What is its molecular formula?

A) C4H10Se B) C8H2Se C) C9H18Se D) C3H12Se E) C2H8Se A) C4H10Se B) C8H2Se C) C9H18Se D) C3H12Se E) C2H8Se

Hydrogen peroxide (H2O2) decomposes catalytically in the presence of metal ions and enzymes called peroxidases.If a 250 mL bottle of hydrogen peroxide solution containing 3.0% H 2O2 (by mass) decomposes completely, how many liters of oxygen gas will it generate? Assume that 1 mol of gas occupies a volume of 22.4 L and that the density of the solution is 1.0 g/mL.The reaction is 2H2 O2 (aq) $\rightarrow$ 2H2 O(l) +O2 (g)

A) 2.5 L B) 4.9 L C) 9.9 L D) 7.4 L E) 0.22 L A) 2.5 L B) 4.9 L C) 9.9 L D) 7.4 L E) 0.22 L

The empirical formula for buckminsterfullerene is C1, and its molar mass is 720.6 g/mol.What is its molecular formula?

A) C60 B) C72 C) C12 D) C1 E) C720 A) C60 B) C72 C) C12 D) C1 E) C720

Acrylonitrile (C3H3N, 53.07 g/mol) can be produced from propylene (C3H6, 42.09 g/mol) according to the reaction shown below.In a particular experiment, 125 g C3H6 reacts with 175 g NO (30.01 g/mol) and 105 g C3H3N is produced.What is the percent yield for the reaction? 4 C3 H6 (g) + 6 NO(g) $\rightarrow$ 4 C3 H3 N(l) +6 H2 O(l) + N2 (g)

The answer of Acrylonitrile (C3H3N, 53.07 g/mol) can be produced...

An important intermediate reaction in the industrial production process of nitric acid is shown.What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? 4 NH3 (g) +5O2 (g) $\rightarrow$ 4 NO(g) +6 H2 O(l)

A) 42.6 kg B) 54.1 kg C) 47.6 kg D) 17.8 kg E) 71.4 kg A) 42.6 kg B) 54.1 kg C) 47.6 kg D) 17.8 kg E) 71.4 kg

In an aqueous solution under basic conditions, ozone (O3) reacts with iodide (I-) and water to form iodine (I2), hydroxide (OH-), and oxygen (O2).What is the sum of the stoichiometric coefficients in the balanced reaction equation? O3(g) + I-(aq) + H2O(l) $\rightarrow$ I2 (aq) + OH-(aq) + O2(g)

A) 6 B) 8 C) 10 D) 12 E) 14 A) 6 B) 8 C) 10 D) 12 E) 14

The average adult exhales about 1.0 kg of carbon dioxide each day.How much glucose (C6H12O6, 180.16 g/mol) is consumed to make that much carbon dioxide?

A) 3.8 kg B) 4.1 kg C) 0.43 kg D) 0.68 kg E) 0.18 kg A) 3.8 kg B) 4.1 kg C) 0.43 kg D) 0.68 kg E) 0.18 kg

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Potassium perchlorate (KClO₃) oxidizes sucrose (C₁₂H₂₂O₁₁) according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? KClO₃ (s) + C₁₂ H₂₂ O₁₁(s) $\rightarrow$ KCl(s) + CO₂ (g) + H₂O (l)

(Multiple Choice)

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Question 101

You create a process to be used in conjunction with combustion analysis using chlorine gas to determine the amount of selenium in certain organic compounds.If there is selenium in the molecule, SeCl₂ (149.87 g/mol) is produced.Analysis of 28.20 g of an unknown compound produces 36.21 g CO₂, 18.53 g H₂O, and 30.83 g SeCl₂.The molar mass of the compound is about 137 g/mol.What is its molecular formula?

(Multiple Choice)

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Question 102

Hydrogen peroxide (H₂O₂) decomposes catalytically in the presence of metal ions and enzymes called peroxidases.If a 250 mL bottle of hydrogen peroxide solution containing 3.0% H ₂O₂ (by mass) decomposes completely, how many liters of oxygen gas will it generate? Assume that 1 mol of gas occupies a volume of 22.4 L and that the density of the solution is 1.0 g/mL.The reaction is 2H₂ O₂ (aq) $\rightarrow$ 2H₂ O(l) +O₂ (g)

(Multiple Choice)

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Question 103

(Na₂B₄O₅OH)₄ . 8 H₂O, commonly known as borax, is used in a variety of applications, including as a fire retardant, an antifungal agent, a flux in metallurgy, a texturing agent in cooking, and a precursor for other boron compounds.How many cubic meters of borax (381.37 g/mol; 1.73 g/cm³) would be required to produce 250 kg elemental boron?

(Short Answer)

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Question 104

A uranium oxide compound is found to be 84.80% U by mass.What is the empirical formula for the compound?

(Multiple Choice)

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Question 105

The empirical formula for buckminsterfullerene is C₁, and its molar mass is 720.6 g/mol.What is its molecular formula?

(Multiple Choice)

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Question 106

Acrylonitrile (C₃H₃N, 53.07 g/mol) can be produced from propylene (C₃H₆, 42.09 g/mol) according to the reaction shown below.In a particular experiment, 125 g C₃H₆ reacts with 175 g NO (30.01 g/mol) and 105 g C₃H₃N is produced.What is the percent yield for the reaction? 4 C₃ H₆ (g) + 6 NO(g) $\rightarrow$ 4 C₃ H₃ N(l) +6 H₂ O(l) + N₂ (g)

(Short Answer)

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Question 107

The combustion of butane (C₄H₁₀) forms carbon dioxide and water.What is the stoichiometric coefficient for oxygen in the balanced equation when 1 mol of butane undergoes combustion?

(Multiple Choice)

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Question 108

An important intermediate reaction in the industrial production process of nitric acid is shown.What is the theoretical yield of H₂O (18.02 g/mol) if 45.0 kg of NH₃ (17.04 g/mol) reacts with excess O₂ (32.00 g/mol)? 4 NH₃ (g) +5O₂ (g) $\rightarrow$ 4 NO(g) +6 H₂ O(l)

(Multiple Choice)

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Question 109

How many moles of ammonia are there in a 346 g sample of pure NH₃ (17.03 g/mol)?

(Multiple Choice)

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Question 110

Sulfuric acid reacts with a vanadium oxide compound according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? H₂SO₄ (aq) + V₂O₃(s) $\rightarrow$ (V₂SO₄ )₃)(s) + H₂O(l)

(Multiple Choice)

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Question 111

You are given a liquid sample that contains methanol, ethanol, or a mixture of both.You use combustion analysis of a 0.336 g sample and obtain 0.462 g of CO₂ and 0.378 of H₂O.What did you learn about your sample?

(Multiple Choice)

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Question 112

A reaction vessel contains equal masses of iron and oxygen.How much FeO could theoretically be produced?

(Multiple Choice)

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Question 113

How much CO₂ is produced by a car driven 20 * 10⁴ mi in one year? Assume the following: • A car gets 20.0 mi/4.0 L of gasoline. • Gasoline has the chemical formula of octane: C₈H₁₈. • One liter of gasoline has a mass of 0.80 kg. • Gasoline is completely burned to carbon dioxide and water.

(Multiple Choice)

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Question 114

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

(Essay)

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Question 115

Ammonium nitrate (NH₄NO₃) can decompose to form gaseous water, nitrogen, and oxygen.What is the sum of the coefficients in the balanced chemical equation?

(Multiple Choice)

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Question 116

In an aqueous solution under basic conditions, ozone (O₃) reacts with iodide (I^-) and water to form iodine (I₂), hydroxide (OH^-), and oxygen (O₂).What is the sum of the stoichiometric coefficients in the balanced reaction equation? O₃(g) + I^-(aq) + H₂O(l) $\rightarrow$ I₂ (aq) + OH^-(aq) + O₂(g)

(Multiple Choice)

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Question 117

One form of elemental sulfur is a ring of eight sulfur atoms.How many moles of molecular oxygen are consumed when one mole of this allotrope burns to make sulfur trioxide?

(Multiple Choice)

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Question 118

The average adult exhales about 1.0 kg of carbon dioxide each day.How much glucose (C₆H₁₂O₆, 180.16 g/mol) is consumed to make that much carbon dioxide?

(Multiple Choice)

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Question 119

Licopene, a red pigment found in tomatoes, has the empirical formula C₅H₇, and its molecular mass is found to be approximately 537 amu.How many empirical units are in the actual molecular formula?

(Multiple Choice)

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Question 120

Showing 101 - 120 of 140

A uranium oxide compound is found to be 84.80% U by mass.What is the empirical formula for the compound?

The empirical formula for buckminsterfullerene is C₁, and its molar mass is 720.6 g/mol.What is its molecular formula?

The combustion of butane (C₄H₁₀) forms carbon dioxide and water.What is the stoichiometric coefficient for oxygen in the balanced equation when 1 mol of butane undergoes combustion?

An important intermediate reaction in the industrial production process of nitric acid is shown.What is the theoretical yield of H₂O (18.02 g/mol) if 45.0 kg of NH₃ (17.04 g/mol) reacts with excess O₂ (32.00 g/mol)? 4 NH₃ (g) +5O₂ (g) $\rightarrow$ 4 NO(g) +6 H₂ O(l)

How many moles of ammonia are there in a 346 g sample of pure NH₃ (17.03 g/mol)?

Sulfuric acid reacts with a vanadium oxide compound according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? H₂SO₄ (aq) + V₂O₃(s) $\rightarrow$ (V₂SO₄ )₃)(s) + H₂O(l)

You are given a liquid sample that contains methanol, ethanol, or a mixture of both.You use combustion analysis of a 0.336 g sample and obtain 0.462 g of CO₂ and 0.378 of H₂O.What did you learn about your sample?

A reaction vessel contains equal masses of iron and oxygen.How much FeO could theoretically be produced?

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

Ammonium nitrate (NH₄NO₃) can decompose to form gaseous water, nitrogen, and oxygen.What is the sum of the coefficients in the balanced chemical equation?

One form of elemental sulfur is a ring of eight sulfur atoms.How many moles of molecular oxygen are consumed when one mole of this allotrope burns to make sulfur trioxide?

The average adult exhales about 1.0 kg of carbon dioxide each day.How much glucose (C₆H₁₂O₆, 180.16 g/mol) is consumed to make that much carbon dioxide?

Licopene, a red pigment found in tomatoes, has the empirical formula C₅H₇, and its molecular mass is found to be approximately 537 amu.How many empirical units are in the actual molecular formula?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Potassium perchlorate (KClO3) oxidizes sucrose (C12H22O11) according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? KClO3 (s) + C12 H22 O11(s) →\rightarrow→ KCl(s) + CO2 (g) + H2O (l)

A uranium oxide compound is found to be 84.80% U by mass.What is the empirical formula for the compound?

The empirical formula for buckminsterfullerene is C1, and its molar mass is 720.6 g/mol.What is its molecular formula?

The combustion of butane (C4H10) forms carbon dioxide and water.What is the stoichiometric coefficient for oxygen in the balanced equation when 1 mol of butane undergoes combustion?

An important intermediate reaction in the industrial production process of nitric acid is shown.What is the theoretical yield of H2O (18.02 g/mol) if 45.0 kg of NH3 (17.04 g/mol) reacts with excess O2 (32.00 g/mol)? 4 NH3 (g) +5O2 (g) →\rightarrow→ 4 NO(g) +6 H2 O(l)

How many moles of ammonia are there in a 346 g sample of pure NH3 (17.03 g/mol)?

Sulfuric acid reacts with a vanadium oxide compound according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? H2SO4 (aq) + V2O3(s) →\rightarrow→ (V2 SO4 )3)(s) + H2O(l)

You are given a liquid sample that contains methanol, ethanol, or a mixture of both.You use combustion analysis of a 0.336 g sample and obtain 0.462 g of CO2 and 0.378 of H2O.What did you learn about your sample?

A reaction vessel contains equal masses of iron and oxygen.How much FeO could theoretically be produced?

How much CO2 is produced by a car driven 20 * 104 mi in one year? Assume the following: • A car gets 20.0 mi/4.0 L of gasoline. • Gasoline has the chemical formula of octane: C8H18. • One liter of gasoline has a mass of 0.80 kg. • Gasoline is completely burned to carbon dioxide and water.

Which of the following oxides of nitrogen have the same empirical formulas? N2O, NO, NO2, N2O2, N2O4

Ammonium nitrate (NH4NO3) can decompose to form gaseous water, nitrogen, and oxygen.What is the sum of the coefficients in the balanced chemical equation?

In an aqueous solution under basic conditions, ozone (O3) reacts with iodide (I-) and water to form iodine (I2), hydroxide (OH-), and oxygen (O2).What is the sum of the stoichiometric coefficients in the balanced reaction equation? O3(g) + I-(aq) + H2O(l) →\rightarrow→ I2 (aq) + OH-(aq) + O2(g)

One form of elemental sulfur is a ring of eight sulfur atoms.How many moles of molecular oxygen are consumed when one mole of this allotrope burns to make sulfur trioxide?

The average adult exhales about 1.0 kg of carbon dioxide each day.How much glucose (C6H12O6, 180.16 g/mol) is consumed to make that much carbon dioxide?

Licopene, a red pigment found in tomatoes, has the empirical formula C5H7, and its molecular mass is found to be approximately 537 amu.How many empirical units are in the actual molecular formula?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

The empirical formula for buckminsterfullerene is C₁, and its molar mass is 720.6 g/mol.What is its molecular formula?

The combustion of butane (C₄H₁₀) forms carbon dioxide and water.What is the stoichiometric coefficient for oxygen in the balanced equation when 1 mol of butane undergoes combustion?

An important intermediate reaction in the industrial production process of nitric acid is shown.What is the theoretical yield of H₂O (18.02 g/mol) if 45.0 kg of NH₃ (17.04 g/mol) reacts with excess O₂ (32.00 g/mol)? 4 NH₃ (g) +5O₂ (g) $\rightarrow$ 4 NO(g) +6 H₂ O(l)

How many moles of ammonia are there in a 346 g sample of pure NH₃ (17.03 g/mol)?

Sulfuric acid reacts with a vanadium oxide compound according to the following unbalanced reaction.What are the coefficients in the balanced chemical equation in the order in which it is written? H₂SO₄ (aq) + V₂O₃(s) $\rightarrow$ (V₂SO₄ )₃)(s) + H₂O(l)

You are given a liquid sample that contains methanol, ethanol, or a mixture of both.You use combustion analysis of a 0.336 g sample and obtain 0.462 g of CO₂ and 0.378 of H₂O.What did you learn about your sample?

Which of the following oxides of nitrogen have the same empirical formulas? N₂O, NO, NO₂, N₂O₂, N₂O₄

Ammonium nitrate (NH₄NO₃) can decompose to form gaseous water, nitrogen, and oxygen.What is the sum of the coefficients in the balanced chemical equation?

The average adult exhales about 1.0 kg of carbon dioxide each day.How much glucose (C₆H₁₂O₆, 180.16 g/mol) is consumed to make that much carbon dioxide?

Licopene, a red pigment found in tomatoes, has the empirical formula C₅H₇, and its molecular mass is found to be approximately 537 amu.How many empirical units are in the actual molecular formula?