A solution of sodium oxalate (Na2C2O4)in acidic solution is titrated with a solution of potassium permanganate (KMnO4)according to the following balanced chemical equation: 2KMnO4(aq)+ 8H2SO4(aq)+ 5Na2C2O4(aq)→ 2MnSO4(aq)+ 8H2O(l)+ 10CO2(g)+ 5Na2SO4(aq)+ K2SO4(aq) What volume of 0.0206 M KMnO4 is required to titrate 0.176 g of Na2C2O4 dissolved in 50.0 mL of solution?

A) 3.42 mL B) 8.54 mL C) 25.5 mL D) 63.8 mL E) 50.0 mL A) 3.42 mL B) 8.54 mL C) 25.5 mL D) 63.8 mL E) 50.0 mL C

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( )→ C9H8O4(s)+ C2H4O2( ) 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%

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g)+ H2O(l)→ H2SO3(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H2SO3(l)?

A) 28.96 g B) 47.55 g C) 0.5793 g D) 0.4521 g E) 37.11 g A) 28.96 g B) 47.55 g C) 0.5793 g D) 0.4521 g E) 37.11 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)

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

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

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

An unknown diprotic acid (H₂A)requires 31.81 mL of 0.109 M NaOH to completely neutralize a 0.685 g sample.Calculate the approximate molar mass of the acid.

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(Multiple Choice)

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Question 1

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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?

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

A solution of sodium oxalate (Na₂C₂O₄)in acidic solution is titrated with a solution of potassium permanganate (KMnO₄)according to the following balanced chemical equation: 2KMnO₄(aq)+ 8H₂SO₄(aq)+ 5Na₂C₂O₄(aq)→ 2MnSO₄(aq)+ 8H₂O(l)+ 10CO₂(g)+ 5Na₂SO₄(aq)+ K₂SO₄(aq) What volume of 0.0206 M KMnO₄ is required to titrate 0.176 g of Na₂C₂O₄ dissolved in 50.0 mL of solution?

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Question 3

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Verified

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

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Question 4

Calibration of a spectrophotometer using a series of green dye containing solutions provides a set of data which follows the Beer-Lambert Law,with a trendline of y = 1.398 × 10³x (y-axis = absorbance,x-axis = molar concentration).What is the molar concentration of a solution with an absorbance of 0.8427?

(Multiple Choice)

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Question 5

One step in the isolation of pure rhodium metal (Rh)is the precipitation of rhodium(III)hydroxide from a solution containing rhodium(III)sulfate according to the following balanced chemical equation: Rh₂(SO₄)₃(aq)+ 6NaOH(aq)→ 2Rh(OH)₃(s)+ 3Na₂SO₄(aq) If 3.10 g of rhodium(III)sulfate reacts with excess sodium hydroxide,what mass of rhodium(III)hydroxide may be produced?

(Multiple Choice)

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Question 6

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s)+ Br₂(g)→ 2 NaBr(s)

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Question 7

Which of the following is true about the actual yield of a product?

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Question 8

In combustion analysis,the gases produced by the combustion of a hydrocarbon are passed through a tube containing finely divided sodium hydroxide supported on asbestos.The purpose of the sodium hydroxide is to absorb ________ produced by the combustion reaction.

(Short Answer)

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Question 9

How many moles of Mg₃P₂(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P₄(s)? 6 Mg(s)+ P₄(s)→ 2 Mg₃P₂(s)

(Multiple Choice)

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Question 10

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( )→ C₉H₈O₄(s)+ C₂H₄O₂( ) 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 11

The pH of an aqueous sodium hydroxide solution is 12.83.What is the hydronium ion concentration of this solution?

(Multiple Choice)

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Question 12

What is the molarity of an NaI solution that contains 4.5 g of NaI in 21.0 mL of solution?

(Multiple Choice)

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Question 13

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g)+ H₂O(l)→ H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l)?

(Multiple Choice)

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Question 14

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)

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Question 15

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)

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Question 16

A compound consists of only C and F.It contains 24% C by mass.What is the empirical formula of the compound?

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Question 17

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

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Question 18

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

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Question 19

A 2.197 g sample of a compound containing only carbon,hydrogen,and oxygen is burned in an excess of dioxygen,producing 4.197 g CO₂ and 2.578 g H₂O.What is the empirical formula of the compound?

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Question 20

Showing 1 - 20 of 77

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

An unknown diprotic acid (H2A)requires 31.81 mL of 0.109 M NaOH to completely neutralize a 0.685 g sample.Calculate the approximate molar mass of the acid.

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?

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

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s)+ Br2(g)→ 2 NaBr(s)

Which of the following is true about the actual yield of a product?

In combustion analysis,the gases produced by the combustion of a hydrocarbon are passed through a tube containing finely divided sodium hydroxide supported on asbestos.The purpose of the sodium hydroxide is to absorb ________ produced by the combustion reaction.

How many moles of Mg3P2(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P4(s)? 6 Mg(s)+ P4(s)→ 2 Mg3P2(s)

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( )→ C9H8O4(s)+ C2H4O2( ) 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?

The pH of an aqueous sodium hydroxide solution is 12.83.What is the hydronium ion concentration of this solution?

What is the molarity of an NaI solution that contains 4.5 g of NaI in 21.0 mL of solution?

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g)+ H2O(l)→ H2SO3(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H2SO3(l)?

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)

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 compound consists of only C and F.It contains 24% C by mass.What is the empirical formula of the compound?

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

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

A 2.197 g sample of a compound containing only carbon,hydrogen,and oxygen is burned in an excess of dioxygen,producing 4.197 g CO2 and 2.578 g H2O.What is the empirical formula of the compound?

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

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An unknown diprotic acid (H₂A)requires 31.81 mL of 0.109 M NaOH to completely neutralize a 0.685 g sample.Calculate the approximate molar mass of the acid.

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?

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

How many moles of sodium bromide can be produced from the reaction of 1.03 moles of sodium with 0.650 moles of bromine gas? 2 Na(s)+ Br₂(g)→ 2 NaBr(s)

How many moles of Mg₃P₂(s)can be produced from the reaction of 0.14 mol Mg(s)with 0.020 mol P₄(s)? 6 Mg(s)+ P₄(s)→ 2 Mg₃P₂(s)

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g)+ H₂O(l)→ H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 37.11 g of H₂SO₃(l)?

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)

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)

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

A 2.197 g sample of a compound containing only carbon,hydrogen,and oxygen is burned in an excess of dioxygen,producing 4.197 g CO₂ and 2.578 g H₂O.What is the empirical formula of the compound?