Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C16H34.How many mL of C16H34 are needed to react with 1.00 mol O2? The density of C16H34 is 0.773 g/mL and its molar mass is 226.43 g/mol.

A) 9.23 mL B) 12.0 mL C) 0.561 mL D) 4.61 mL E) 0.140 mL A) 9.23 mL B) 12.0 mL C) 0.561 mL D) 4.61 mL E) 0.140 mL

Potassium superoxide (KO2, 71.10 g/mol) can be used to generate oxygen gas.If the theoretical yield of O2 (32.00 g/mol) must be 12.0 g, how many grams of KO2 should be used? Assume the reaction occurs in the presence of excess H2O (18.02 g/mol). 4 KO2(s) + 2 H2O(l) $\rightarrow$ 4 KOH(s) + 3O2 (g)

A) 26.7 g B) 107 g C) 28.1 g D) 35.6 g E) 20.0 g A) 26.7 g B) 107 g C) 28.1 g D) 35.6 g E) 20.0 g

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C 16H34.Write the balanced reaction equation for the combustion of C 16H34 and report the sum of the stoichiometric coefficients.

A) 117 B) 120 C) 76 D) 83 E) 4 A) 117 B) 120 C) 76 D) 83 E) 4

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

A) 3.45 g B) 13.8 g C) 21.8 g D) 16.0 g E) 32.6 g A) 3.45 g B) 13.8 g C) 21.8 g D) 16.0 g E) 32.6 g

The space shuttle uses liquid hydrogen and liquid oxygen to produce thrust for liftoff in the following reaction: 2H2 (l) +O2 (l) $\rightarrow$2H2 O(g) If the liquid oxygen supply is set to provide 420 kg/s during a launch, what does the rate of liquid hydrogen supply need to be in kilograms per second?

A) 840 kg/s B) 210 kg/s C) 106 kg/s D) 53.1kg/s E) 63.4 kg/s A) 840 kg/s B) 210 kg/s C) 106 kg/s D) 53.1kg/s E) 63.4 kg/s

Suppose the combustion of fossil fuels adds about 8.0 * 1012 kg of carbon to the atmosphere per year in the form of CO2.How much oxygen gas is required to produce this amount of carbon dioxide?

A) about 2.1*1013 kg B) about 5.8 * 1012 kg C) about 4.3 *1012 kg D) about 1.1 * 1013 kg E) about 4.8 * 1013 kg A) about 2.1*1013 kg B) about 5.8 * 1012 kg C) about 4.3 *1012 kg D) about 1.1 * 1013 kg E) about 4.8 * 1013 kg

Paris green is a highly toxic emerald green compound with the formula Cu(C2H3O2 )2 . 3Cu(AsO2 )2 .What is its percent by mass arsenic?

A) 31.99% B) 14.78% C) 22.17% D) 7.389% E) 44.34% A) 31.99% B) 14.78% C) 22.17% D) 7.389% E) 44.34%

Ammonia (NH3, 17.04 g/mol) is industrially produced from N2 and H2 using the Haber process.What mass of H2 should be used if 34.0 kg NH3 must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

A) 6.05 kg B) 9.07 kg C) 18.3 kg D) 3.03 kg E) 2.00 kg A) 6.05 kg B) 9.07 kg C) 18.3 kg D) 3.03 kg E) 2.00 kg

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226.43 g/mol.

(Multiple Choice)

4.9/5

(42)

Question 61

Potassium superoxide (KO₂, 71.10 g/mol) can be used to generate oxygen gas.If the theoretical yield of O₂ (32.00 g/mol) must be 12.0 g, how many grams of KO₂ should be used? Assume the reaction occurs in the presence of excess H₂O (18.02 g/mol). 4 KO₂(s) + 2 H₂O(l) $\rightarrow$ 4 KOH(s) + 3O₂ (g)

(Multiple Choice)

4.9/5

(29)

Question 62

The combustion of ethanol (CH₃CH₂OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

(Multiple Choice)

4.7/5

(36)

Question 63

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

(Essay)

4.8/5

(34)

Question 64

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

(Short Answer)

4.8/5

(27)

Question 65

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C₈ H₁₈ (l) +O₂ (g) $\rightarrow$ CO₂ (g) + H₂ O(l)

(Multiple Choice)

4.9/5

(32)

Question 66

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

(Multiple Choice)

4.9/5

(33)

Question 67

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C ₁₆H₃₄.Write the balanced reaction equation for the combustion of C ₁₆H₃₄ and report the sum of the stoichiometric coefficients.

(Multiple Choice)

4.9/5

(38)

Question 68

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

(Multiple Choice)

4.7/5

(37)

Question 69

The space shuttle uses liquid hydrogen and liquid oxygen to produce thrust for liftoff in the following reaction: 2H₂ (l) +O₂ (l) $\rightarrow$ 2H₂ O(g) If the liquid oxygen supply is set to provide 420 kg/s during a launch, what does the rate of liquid hydrogen supply need to be in kilograms per second?

(Multiple Choice)

5.0/5

(35)

Question 70

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

(Multiple Choice)

4.7/5

(41)

Question 71

Suppose the combustion of fossil fuels adds about 8.0 * 10¹² kg of carbon to the atmosphere per year in the form of CO₂.How much oxygen gas is required to produce this amount of carbon dioxide?

(Multiple Choice)

4.8/5

(35)

Question 72

A copper ore consisting of 12.5% copper(II) sulfide 95.61 g/mol), when heated and reacted with oxygen gas 32.00 g/mol), produces copper(II) oxide (79.55 g/mol) and sulfur dioxide (64.06 g/mol).If the reaction has a 90.0% yield, how many grams of copperII) oxide are produced when 1.00 kg of the copper ore is processed? 2 CuS(s) +3 O₂ (g) $\rightarrow$ 2 CuO(s) + 2 SO₂ (g)

(Multiple Choice)

4.7/5

(36)

Question 73

Extracting copper from sulfide ores can be performed by roasting the ore in oxygen, with a subsequent reaction of copper(I) oxide with carbon.Simplified chemical equations for these steps are shown below.Mathematically combine the two reactions to create an overall balanced equation that contains CU(s) as the only form of copper as a product.Eliminate like terms from your final equation and use the lowest whole-number coefficients possible.Select the statement regarding the overall balanced reaction that is FALSE. 2 Cu₂ S(s) +3O₂ (g) $\rightarrow$ 2 Cu₂ O(s) + 2 SO₂ (g) Cu₂ O(s) + C(s) $\rightarrow$ 2 Cu(s) + CO(g)

(Multiple Choice)

4.9/5

(33)

Question 74

Paris green is a highly toxic emerald green compound with the formula Cu(C₂H₃O₂ )2 . 3Cu(AsO₂ )₂ .What is its percent by mass arsenic?

(Multiple Choice)

4.9/5

(28)

Question 75

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

(Multiple Choice)

4.9/5

(44)

Question 76

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

(Multiple Choice)

4.8/5

(36)

Question 77

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

(Multiple Choice)

4.9/5

(36)

Question 78

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical formula.

(Multiple Choice)

4.9/5

(36)

Question 79

TiCl₄ (189.68 g/mol), a source of Ti metal, can be produced from titanium dioxide (79.87 g/mol), carbon (12.01 g/mol), and chlorine gas (70.90 g/mol).Identify the limiting reactant if 195 g TiO₂ and 325 g Cl₂ react in the presence of excess C.Assuming 100% yield, calculate the mass of TiCl ₄ produced. 3 Ti O₂ (s) + 4 C(s) + 6 CL₂ (g) $\rightarrow$ 3 Ti CL₄ (s) + 2 CO₂ (g) + 2 CO(g)

(Short Answer)

4.9/5

(33)

Question 80

Showing 61 - 80 of 140

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH₃CH₂OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C₈ H₁₈ (l) +O₂ (g) $\rightarrow$ CO₂ (g) + H₂ O(l)

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C ₁₆H₃₄.Write the balanced reaction equation for the combustion of C ₁₆H₃₄ and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

Suppose the combustion of fossil fuels adds about 8.0 * 10¹² kg of carbon to the atmosphere per year in the form of CO₂.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C₂H₃O₂ )2 . 3Cu(AsO₂ )₂ .What is its percent by mass arsenic?

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical 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

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C16H34.How many mL of C16H34 are needed to react with 1.00 mol O2? The density of C16H34 is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH3CH2OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH3 and 150 g O2 react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH3 (g) + 5O2 (g) →\rightarrow→ 4 NO(g) +6H2 O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C8 H18 (l) +O2 (g) →\rightarrow→ CO2 (g) + H2 O(l)

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C 16H34.Write the balanced reaction equation for the combustion of C 16H34 and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

Suppose the combustion of fossil fuels adds about 8.0 * 1012 kg of carbon to the atmosphere per year in the form of CO2.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C2H3O2 )2 . 3Cu(AsO2 )2 .What is its percent by mass arsenic?

Ammonia (NH3, 17.04 g/mol) is industrially produced from N2 and H2 using the Haber process.What mass of H2 should be used if 34.0 kg NH3 must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical 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

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH₃CH₂OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C₈ H₁₈ (l) +O₂ (g) $\rightarrow$ CO₂ (g) + H₂ O(l)

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C ₁₆H₃₄.Write the balanced reaction equation for the combustion of C ₁₆H₃₄ and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

Suppose the combustion of fossil fuels adds about 8.0 * 10¹² kg of carbon to the atmosphere per year in the form of CO₂.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C₂H₃O₂ )2 . 3Cu(AsO₂ )₂ .What is its percent by mass arsenic?

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?