Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S8(s) + 24 F2(g) → 8 SF6(g) What is the percent yield if 18.3 g SF6 is isolated from the reaction of 10.0 g S8 and 30.0 g F2?

A) 40.2% B) 45.8% C) 47.6% D) 54.6% E) 61.0% A) 40.2% B) 45.8% C) 47.6% D) 54.6% E) 61.0%

If 15.0 g of nitrogen (N2) and 2.00 g of hydrogen (H2) react to produce 1.38 g of ammonia (NH3), according to the reaction below, what is the percent yield of the reaction? N2(g) + 3 H2(g) → 2 NH3(g)

A) 7.57% B) 12.2% C) 8.12% D) 15.1% E) 8.17% A) 7.57% B) 12.2% C) 8.12% D) 15.1% E) 8.17%

Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH3 must react with excess oxygen to yield 157 g NO? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

A) 89.1 g B) 302 g C) 263 g D) 26.3 g E) 938 g A) 89.1 g B) 302 g C) 263 g D) 26.3 g E) 938 g

The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.3 g of CCl4, carbon tetrachloride: 2CHCl3 + 2Cl2 → 2CCl4 + 2HCl What is the percent yield?

A) 86.6 % B) 100 % C) 67.2 % D) 33.6 % E) 44.8 % A) 86.6 % B) 100 % C) 67.2 % D) 33.6 % E) 44.8 %

A 1.295 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 3.553 g CO2 and water. What mass of hydrogen is contained in the original sample?

A) 0.3255 g B) 2.258 g C) 4.848 g D) 1.288 g E) 0.6475 g A) 0.3255 g B) 2.258 g C) 4.848 g D) 1.288 g E) 0.6475 g

What is the pH of 4.1 × 10−3 M HCl(aq)?

A) -1.01 B) 2.39 C) 3.50 D) 1.01 E) 5.65 A) -1.01 B) 2.39 C) 3.50 D) 1.01 E) 5.65

Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol). C7H6O3(s) + C4H6O3( $\ell$ ) ? C9H8O4(s) + C2H4O2( $\ell$ ) If 2.04 g of C9H8O4 (M = 180.2 g/mol) is produced from the reaction of 3.03 g C7H6O3 and 4.01 g C4H6O3, what is the percent yield?

A) 28.8% B) 29.0% C) 50.9% D) 51.6% E) 67.3% A) 28.8% B) 29.0% C) 50.9% D) 51.6% E) 67.3%

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

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Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S₈(s) + 24 F₂(g) → 8 SF₆(g) What is the percent yield if 18.3 g SF₆ is isolated from the reaction of 10.0 g S₈ and 30.0 g F₂?

(Multiple Choice)

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Question 61

If 15.0 g of nitrogen (N₂) and 2.00 g of hydrogen (H₂) react to produce 1.38 g of ammonia (NH₃), according to the reaction below, what is the percent yield of the reaction? N₂(g) + 3 H₂(g) → 2 NH₃(g)

(Multiple Choice)

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Question 62

Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH₃ must react with excess oxygen to yield 157 g NO? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

(Multiple Choice)

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Question 63

The reaction of 5.07 g N₂ with 0.722 g H₂ produces 1.27 g NH₃. The percent yield of this reaction is ________.

(Short Answer)

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Question 64

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆. (Molar mass P₄O₆ = 219.9 g/mol)

(Multiple Choice)

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Question 65

A 30.00-mL sample of a weak monoprotic acid is titrated with 0.0915 M NaOH. At the endpoint, it is found that 45.98 mL of titrant was used. What was the concentration of the weak acid?

(Multiple Choice)

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Question 66

The reaction of 11.9 g of CHCl₃ with excess chlorine produced 10.3 g of CCl₄, carbon tetrachloride: 2CHCl₃ + 2Cl₂ → 2CCl₄ + 2HCl What is the percent yield?

(Multiple Choice)

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Question 67

Phosphorus trichloride, PCl₃, can be produced from the reaction below: P₄(s) + 6 Cl₂(g) → 4 PCl₃(g) If 1.00 g of phosphorus, P₄, reacts with 1.00 g of chlorine, Cl₂, which reactant is the limiting reactant and what mass of product may be produced?

(Essay)

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Question 68

A 1.295 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 3.553 g CO₂ and water. What mass of hydrogen is contained in the original sample?

(Multiple Choice)

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Question 69

What is the pH of 4.1 × 10−³ M HCl(aq)?

(Multiple Choice)

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Question 70

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂)?

(Multiple Choice)

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Question 71

Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol). C₇H₆O₃(s) + C₄H₆O₃( $\ell$ ) ? C₉H₈O₄(s) + C₂H₄O₂( $\ell$ ) If 2.04 g of C₉H₈O₄ (M = 180.2 g/mol) is produced from the reaction of 3.03 g C₇H₆O₃ and 4.01 g C₄H₆O₃, what is the percent yield?

(Multiple Choice)

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Question 72

The reaction of 0.779 g K with O₂ forms 1.417 g potassium superoxide, a substance used in self-contained breathing devices. Determine the formula for potassium superoxide.

(Multiple Choice)

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Question 73

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI₂, can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

(Multiple Choice)

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Question 74

The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.

(Short Answer)

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Question 75

An impure sample of benzoic acid (C₆H₅COOH, 122.12 g/mol) is titrated with 0.5360 M NaOH. A 1.888-g sample requires 20.50 mL of titrant to reach the endpoint. What is the percent by mass of benzoic acid in the sample? C₆H₅COOH(aq) + NaOH(aq) → NaC₆H₅COO(aq) + H₂O(l)

(Multiple Choice)

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Question 76

The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?

(Multiple Choice)

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Question 77

Showing 61 - 77 of 77

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S8(s) + 24 F2(g) → 8 SF6(g) What is the percent yield if 18.3 g SF6 is isolated from the reaction of 10.0 g S8 and 30.0 g F2?

If 15.0 g of nitrogen (N2) and 2.00 g of hydrogen (H2) react to produce 1.38 g of ammonia (NH3), according to the reaction below, what is the percent yield of the reaction? N2(g) + 3 H2(g) → 2 NH3(g)

Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH3 must react with excess oxygen to yield 157 g NO? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

The reaction of 5.07 g N2 with 0.722 g H2 produces 1.27 g NH3. The percent yield of this reaction is ________.

Calculate the number of moles of O2 required to react with phosphorus to produce 5.20 g of P4O6. (Molar mass P4O6 = 219.9 g/mol)

A 30.00-mL sample of a weak monoprotic acid is titrated with 0.0915 M NaOH. At the endpoint, it is found that 45.98 mL of titrant was used. What was the concentration of the weak acid?

The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.3 g of CCl4, carbon tetrachloride: 2CHCl3 + 2Cl2 → 2CCl4 + 2HCl What is the percent yield?

Phosphorus trichloride, PCl3, can be produced from the reaction below: P4(s) + 6 Cl2(g) → 4 PCl3(g) If 1.00 g of phosphorus, P4, reacts with 1.00 g of chlorine, Cl2, which reactant is the limiting reactant and what mass of product may be produced?

A 1.295 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 3.553 g CO2 and water. What mass of hydrogen is contained in the original sample?

What is the pH of 4.1 × 10−3 M HCl(aq)?

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H2O2)?

The reaction of 0.779 g K with O2 forms 1.417 g potassium superoxide, a substance used in self-contained breathing devices. Determine the formula for potassium superoxide.

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI2, can be produced from the reaction of 5.15 g Mg and 50.0 g I2?

The percent yield of a chemical reaction is calculated by dividing the actual yield by the ________ yield and multiplying by 100%.

An impure sample of benzoic acid (C6H5COOH, 122.12 g/mol) is titrated with 0.5360 M NaOH. A 1.888-g sample requires 20.50 mL of titrant to reach the endpoint. What is the percent by mass of benzoic acid in the sample? C6H5COOH(aq) + NaOH(aq) → NaC6H5COO(aq) + H2O(l)

The compound P4S3 is used in matches. It reacts with oxygen to produce P4O10 and SO2. The unbalanced chemical equation is shown below. P4S3(s) + O2(g) → P4O10(s) + SO2(g) What mass of SO2 is produced from the combustion of 0.401 g P4S3?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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Sulfur hexafluoride is produced by reacting elemental sulfur with fluorine gas. S₈(s) + 24 F₂(g) → 8 SF₆(g) What is the percent yield if 18.3 g SF₆ is isolated from the reaction of 10.0 g S₈ and 30.0 g F₂?

If 15.0 g of nitrogen (N₂) and 2.00 g of hydrogen (H₂) react to produce 1.38 g of ammonia (NH₃), according to the reaction below, what is the percent yield of the reaction? N₂(g) + 3 H₂(g) → 2 NH₃(g)

Under certain conditions the reaction of ammonia with excess oxygen will produce a 29.5% yield of NO. What mass of NH₃ must react with excess oxygen to yield 157 g NO? 4 NH₃(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g)

The reaction of 5.07 g N₂ with 0.722 g H₂ produces 1.27 g NH₃. The percent yield of this reaction is ________.

Calculate the number of moles of O₂ required to react with phosphorus to produce 5.20 g of P₄O₆. (Molar mass P₄O₆ = 219.9 g/mol)

The reaction of 11.9 g of CHCl₃ with excess chlorine produced 10.3 g of CCl₄, carbon tetrachloride: 2CHCl₃ + 2Cl₂ → 2CCl₄ + 2HCl What is the percent yield?

Phosphorus trichloride, PCl₃, can be produced from the reaction below: P₄(s) + 6 Cl₂(g) → 4 PCl₃(g) If 1.00 g of phosphorus, P₄, reacts with 1.00 g of chlorine, Cl₂, which reactant is the limiting reactant and what mass of product may be produced?

A 1.295 g sample of a hydrocarbon is burned in an excess of dioxygen, producing 3.553 g CO₂ and water. What mass of hydrogen is contained in the original sample?

What is the pH of 4.1 × 10−³ M HCl(aq)?

Hydrogen peroxide decomposes into oxygen and water. What mass of oxygen is formed from the decomposition of 125 g of hydrogen peroxide (H₂O₂)?

The reaction of 0.779 g K with O₂ forms 1.417 g potassium superoxide, a substance used in self-contained breathing devices. Determine the formula for potassium superoxide.

Magnesium reacts with iodine gas at high temperatures to form magnesium iodide. What mass of magnesium iodide, MgI₂, can be produced from the reaction of 5.15 g Mg and 50.0 g I₂?

An impure sample of benzoic acid (C₆H₅COOH, 122.12 g/mol) is titrated with 0.5360 M NaOH. A 1.888-g sample requires 20.50 mL of titrant to reach the endpoint. What is the percent by mass of benzoic acid in the sample? C₆H₅COOH(aq) + NaOH(aq) → NaC₆H₅COO(aq) + H₂O(l)

The compound P₄S₃ is used in matches. It reacts with oxygen to produce P₄O₁₀ and SO₂. The unbalanced chemical equation is shown below. P₄S₃(s) + O₂(g) → P₄O₁₀(s) + SO₂(g) What mass of SO₂ is produced from the combustion of 0.401 g P₄S₃?