What mass of iron can be produced from the reaction of 175 kg Fe2O3 with 385 kg CO? Fe2O3(s)+ 3 CO(g)$\to$ 2 Fe(s)+ 3 CO2(g)

A) 2.19 kg B) 30.6 kg C) 61.2 kg D) 122 kg E) 512 kg A) 2.19 kg B) 30.6 kg C) 61.2 kg D) 122 kg E) 512 kg D

What volume of 0.464 M Na2CO3 solution contains 74.7 g of Na2CO3?

A) 0.327 L B) 1.71 $\times$ 104 L C) 1.52 L D) 3.67 $\times$ 103 L E) 0.658 L A) 0.327 L B) 1.71 $\times$ 104 L C) 1.52 L D) 3.67 $\times$ 103 L E) 0.658 L C

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)$\to$ 2MnSO4(aq)+ 8H2O(l)+ 10CO2(g)+ 5Na2SO4(aq)+ K2SO4(aq) What volume of 0.0388 M KMnO4 is required to titrate 0.134 g of Na2C2O4 dissolved in 20.0 mL of solution?

A) 1.38 mL B) 3.45 mL C) 10.3 mL D) 25.8 mL E) 20.0 mL A) 1.38 mL B) 3.45 mL C) 10.3 mL D) 25.8 mL E) 20.0 mL C

Nitric oxide,NO,is made from the oxidation of NH3 as follows: 4NH3 + 5O2 $\to$ 4NO + 6H2O If 9.4-g of NH3 gives 12.0 g of NO,what is the percent yield of NO?

A) 91 % B) 44 % C) 17 % D) 72 % E) 22 % A) 91 % B) 44 % C) 17 % D) 72 % E) 22 %

The reaction of 11.9 g of CHCl3 with excess chlorine produced 10.3 g of CCl4,carbon tetrachloride: 2CHCl3 + 2Cl2 $\to$ 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 %

Complete combustion of a 0.30-mol sample of a hydrocarbon,CxHy,gives 1.80 mol of CO2 and 1.20 mol of H2O.The molecular formula of the original hydrocarbon is

A) C3H8. B) C6H8. C) C7H18. D) C5H5. E) C5H6. A) C3H8. B) C6H8. C) C7H18. D) C5H5. E) C5H6.

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)$\to$ 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

Aspirin (C9H8O4)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol).C7H6O3(s)+ C4H6O3( )$\to$C9H8O4(s)+ C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?

A) 0.40 g B) 2.61 g C) 2.82 g D) 1.53 g E) 3.60 g A) 0.40 g B) 2.61 g C) 2.82 g D) 1.53 g E) 3.60 g

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( )$\to$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%

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

A) 29.5 g B) 44.9 g C) 54.8 g D) 55.2 g E) 58.9 g A) 29.5 g B) 44.9 g C) 54.8 g D) 55.2 g E) 58.9 g

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g)+ H2O(l)$\to$H2SO3(l) What mass of sulfur dioxide is needed to prepare 21.06 g of H2SO3(l)?

A) 16.44 g B) 26.98 g C) 0.3287 g D) 0.2566 g E) 21.06 g A) 16.44 g B) 26.98 g C) 0.3287 g D) 0.2566 g E) 21.06 g

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s)+ 3 CO(g) $\to$ 2 Fe(s)+ 3 CO₂(g)

Free

(Multiple Choice)

4.7/5

(39)

Question 1

Correct Answer:

Verified

What volume of 0.464 M Na₂CO₃ solution contains 74.7 g of Na₂CO₃?

Free

(Multiple Choice)

4.8/5

(39)

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) $\to$ 2MnSO₄(aq)+ 8H₂O(l)+ 10CO₂(g)+ 5Na₂SO₄(aq)+ K₂SO₄(aq) What volume of 0.0388 M KMnO₄ is required to titrate 0.134 g of Na₂C₂O₄ dissolved in 20.0 mL of solution?

Free

(Multiple Choice)

4.8/5

(42)

Question 3

Correct Answer:

Verified

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

(Multiple Choice)

4.9/5

(47)

Question 4

Nitric oxide,NO,is made from the oxidation of NH₃ as follows: 4NH₃ + 5O₂ $\to$ 4NO + 6H₂O If 9.4-g of NH₃ gives 12.0 g of NO,what is the percent yield of NO?

(Multiple Choice)

4.7/5

(29)

Question 5

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

(Multiple Choice)

4.9/5

(33)

Question 6

The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.

(Short Answer)

4.8/5

(34)

Question 7

In order to dilute 35.5 mL of 0.533 M HCl to 0.100 M,the volume of water that must be added is

(Multiple Choice)

4.7/5

(35)

Question 8

An unknown diprotic acid (H₂A)requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580 g sample.Calculate the approximate molar mass of the acid.

(Multiple Choice)

4.8/5

(37)

Question 9

Complete combustion of a 0.30-mol sample of a hydrocarbon,C_xH_y,gives 1.80 mol of CO₂ and 1.20 mol of H₂O.The molecular formula of the original hydrocarbon is

(Multiple Choice)

4.8/5

(38)

Question 10

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) $\to$ 4 NO(g)+ 6 H₂O(g)

(Multiple Choice)

4.8/5

(42)

Question 11

Transmittance,T,is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample.The absorbance,A,is defined as

(Multiple Choice)

4.9/5

(32)

Question 12

What volume of 2.52 M HCl is required to prepare 176.5 mL of 0.449 M HCl?

(Multiple Choice)

4.9/5

(39)

Question 13

Aspirin (C₉H₈O₄)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol).C₇H₆O₃(s)+ C₄H₆O₃( $Aspirin (C9H8O4)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol).C7H6O3(s)+ C4H6O3( ) \to C9H8O4(s)+ C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?$ ) $\to$ C₉H₈O₄(s)+ C₂H₄O₂( $Aspirin (C9H8O4)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol).C7H6O3(s)+ C4H6O3( ) \to C9H8O4(s)+ C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?$ ) If you react 2.00 g C₇H₆O₃ with 1.60 g C₄H₆O₃,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?

(Multiple Choice)

4.8/5

(39)

Question 14

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

4.9/5

(35)

Question 15

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

(Multiple Choice)

4.9/5

(49)

Question 16

Of the following,the only empirical formula is

(Multiple Choice)

4.7/5

(34)

Question 17

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g)+ H₂O(l) $\to$ H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 21.06 g of H₂SO₃(l)?

(Multiple Choice)

4.8/5

(36)

Question 18

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

(Short Answer)

4.8/5

(36)

Question 19

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

(Multiple Choice)

4.9/5

(37)

Question 20

Showing 1 - 20 of 76

Exam 5: Stoichiometry: Quantitative Information About Chemical Reactions

What mass of iron can be produced from the reaction of 175 kg Fe2O3 with 385 kg CO? Fe2O3(s)+ 3 CO(g) →\to→ 2 Fe(s)+ 3 CO2(g)

What volume of 0.464 M Na2CO3 solution contains 74.7 g of Na2CO3?

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

Nitric oxide,NO,is made from the oxidation of NH3 as follows: 4NH3 + 5O2 →\to→ 4NO + 6H2O If 9.4-g of NH3 gives 12.0 g of NO,what is the percent yield of NO?

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

The numbers preceding the formulas in chemical equations are referred to as the ________ coefficients.

In order to dilute 35.5 mL of 0.533 M HCl to 0.100 M,the volume of water that must be added is

An unknown diprotic acid (H2A)requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580 g sample.Calculate the approximate molar mass of the acid.

Complete combustion of a 0.30-mol sample of a hydrocarbon,CxHy,gives 1.80 mol of CO2 and 1.20 mol of H2O.The molecular formula of the original hydrocarbon is

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) →\to→ 4 NO(g)+ 6 H2O(g)

Transmittance,T,is defined as the intensity of light transmitted through a sample divided by the intensity of light incident on the sample.The absorbance,A,is defined as

What volume of 2.52 M HCl is required to prepare 176.5 mL of 0.449 M HCl?

Aspirin (C9H8O4)is produced by the reaction of salicylic acid (M = 138.1 g/mol)and acetic anhydride (M = 102.1 g/mol).C7H6O3(s)+ C4H6O3( ) →\to→ C9H8O4(s)+ C2H4O2( ) If you react 2.00 g C7H6O3 with 1.60 g C4H6O3,what mass of aspirin (M = 180.2 g/mol)can theoretically be obtained?

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( ) →\to→ 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?

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

Of the following,the only empirical formula is

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO2(g)+ H2O(l) →\to→ H2SO3(l) What mass of sulfur dioxide is needed to prepare 21.06 g of H2SO3(l)?

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

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

Basic Concepts of Chemistry

Mathlets 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 Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Principles of 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

Filters

What mass of iron can be produced from the reaction of 175 kg Fe₂O₃ with 385 kg CO? Fe₂O₃(s)+ 3 CO(g) $\to$ 2 Fe(s)+ 3 CO₂(g)

What volume of 0.464 M Na₂CO₃ solution contains 74.7 g of Na₂CO₃?

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

Nitric oxide,NO,is made from the oxidation of NH₃ as follows: 4NH₃ + 5O₂ $\to$ 4NO + 6H₂O If 9.4-g of NH₃ gives 12.0 g of NO,what is the percent yield of NO?

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

An unknown diprotic acid (H₂A)requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580 g sample.Calculate the approximate molar mass of the acid.

Complete combustion of a 0.30-mol sample of a hydrocarbon,C_xH_y,gives 1.80 mol of CO₂ and 1.20 mol of H₂O.The molecular formula of the original hydrocarbon is

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) $\to$ 4 NO(g)+ 6 H₂O(g)

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

Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below). SO₂(g)+ H₂O(l) $\to$ H₂SO₃(l) What mass of sulfur dioxide is needed to prepare 21.06 g of H₂SO₃(l)?

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