Given the reaction: 2KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O How many moles of H2SO4 are required to produce 2.0 moles of I2, given the other reactants are in excess?

A) 0.80 mol B) 1.3 mol C) 3.2 mol D) 4.0 mol E) 1.6 mol A) 0.80 mol B) 1.3 mol C) 3.2 mol D) 4.0 mol E) 1.6 mol

What mass of MgCl2 in grams must be added to 250.0 mL of a 0.25 M MgCl2 solution to produce a 0.40 M solution, assuming no change of volume upon addition?

A) 9.5 g B) 6.0 g C) 2.2 g D) 3.6 g E) 19 g A) 9.5 g B) 6.0 g C) 2.2 g D) 3.6 g E) 19 g

Given the reaction: 2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O, How many moles of K2SO4 are produced by allowing five moles each of KMnO4, KI, and H2SO4 to react?

A) 3 mol B) 1 mol C) 2 mol D) 4 mol E) 5 mol A) 3 mol B) 1 mol C) 2 mol D) 4 mol E) 5 mol

For the reaction 2 Al + Fe2O3 → Al2O3 + 2 Fe, 2.5 g of Al (27.0 g/mol) and 7.2 g of Fe2O3 (159.8 g/mol) produce how many g of Fe (55.9 g/mol)?

A) 2.5 (55.9/27.0) g B) 2.5 (55.9)(2)/(27.0)(2) g C) 7.2 (55.9)(2)/159.8 g D) 7.2 (55.9/159.8) g E) 2.5 (55.9/159.8) g A) 2.5 (55.9/27.0) g B) 2.5 (55.9)(2)/(27.0)(2) g C) 7.2 (55.9)(2)/159.8 g D) 7.2 (55.9/159.8) g E) 2.5 (55.9/159.8) g

How many grams of ZnSO4 will be made from 41.0 grams each of Zn, K2Cr2O7, and H2SO4? 4 Zn + K2Cr2O7 + 7 H2SO4 → 4 ZnSO4 + 2 CrSO4 + K2SO4 + 7 H2O

A) 67.6 g B) 38.6 g C) 101 g D) 20.6 g E) 82.5 g A) 67.6 g B) 38.6 g C) 101 g D) 20.6 g E) 82.5 g

What is the molarity of a sucrose solution (C12H22O11) if 110.0 g of a 92.0% pure solid is dissolved per 250.0 mL of water?

A) 0.296 M B) 1.29 M C) 0.321 M D) 1.40 M E) 1.18 M A) 0.296 M B) 1.29 M C) 0.321 M D) 1.40 M E) 1.18 M

Given the following reaction: Na2SO4(s) + 2 C(s) → Na2S(s) + 2 CO2(g) How many grams of carbon are required to produce 18.4 g Na2S(s)?

A) 11.3 g B) 5.66 g C) 2.83 g D) 239 g E) 142 g A) 11.3 g B) 5.66 g C) 2.83 g D) 239 g E) 142 g

If 8.52 g each of zinc, potassium dichromate, and sulfuric acid are reacted by the reaction: 4 Zn + K2Cr2O7 + 7 H2SO4→ 4 ZnSO4 + 2 CrSO4 +K2SO4 + 7 H2O How many grams of potassium dichromate will be left unreacted?

A) 1.05 g B) 2.84 g C) 7.30 g D) 4.87 g E) 3.65 g A) 1.05 g B) 2.84 g C) 7.30 g D) 4.87 g E) 3.65 g

What volume of concentrated acetic acid (CH3CO2H, density 1.05 g mL-1) is needed to prepare 250 mL of a 0.30 M aqueous solution?

A) 4.7 mL B) 4.3 mL C) 3.0 mL D) 2.5 mL E) 2.2 mL A) 4.7 mL B) 4.3 mL C) 3.0 mL D) 2.5 mL E) 2.2 mL

Exam 4: Chemical Reactions

306 mL of a 0.208 M solution of silver nitrate will react with 146 mL of a 0.170 M solution of sodium phosphate to produce how many grams of silver phosphate precipitate? The balanced reaction is: 3 AgNO₃ + Na₃PO₄ → Ag₃PO₄ + 3 NaNO₃

(Multiple Choice)

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Question 21

Given the reaction: 2KMnO₄ + 10 KI + 8 H₂SO₄→ 6 K₂SO₄ + 2 MnSO₄ + 5 I₂+ 8 H₂O How many moles of H₂SO₄ are required to produce 2.0 moles of I₂, given the other reactants are in excess?

(Multiple Choice)

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Question 22

The numbers in front of formulas in balanced equations are called stoichiometric coefficients.

(True/False)

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Question 23

What mass of MgCl₂ in grams must be added to 250.0 mL of a 0.25 M MgCl₂ solution to produce a 0.40 M solution, assuming no change of volume upon addition?

(Multiple Choice)

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Question 24

What volume of 6.0 M sulfuric acid is required for the preparation of 500.0 mL of 0.30 M solution?

(Multiple Choice)

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Question 25

52.5 mL of a solution were diluted to a volume of 6.25 L and then had a concentration of 3.16 M. What was the molarity of the initial solution?

(Multiple Choice)

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Question 26

Given the reaction: 2 KMnO₄ + 10 KI + 8 H₂SO₄ → 6 K₂SO₄ + 2 MnSO₄ + 5 I₂ + 8 H₂O, How many moles of K₂SO₄ are produced by allowing five moles each of KMnO₄, KI, and H₂SO₄ to react?

(Multiple Choice)

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Question 27

What volume of 2.0 M HCl, in mL, is required to dissolve a 10.0 g piece of Zn? Zn(s) + 2 HCl → ZnCl₂ + H₂(g)

(Multiple Choice)

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Question 28

For the reaction 2 Al + Fe₂O₃ → Al₂O₃ + 2 Fe, 2.5 g of Al (27.0 g/mol) and 7.2 g of Fe₂O₃ (159.8 g/mol) produce how many g of Fe (55.9 g/mol)?

(Multiple Choice)

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Question 29

Which metal will produce the most hydrogen per gram of metal?

(Multiple Choice)

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Question 30

How many grams of ZnSO₄ will be made from 41.0 grams each of Zn, K₂Cr₂O₇, and H₂SO₄? 4 Zn + K₂Cr₂O₇ + 7 H₂SO₄ → 4 ZnSO₄ + 2 CrSO₄ + K₂SO₄ + 7 H₂O

(Multiple Choice)

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Question 31

What is the molarity of a sucrose solution (C₁₂H₂₂O₁₁) if 110.0 g of a 92.0% pure solid is dissolved per 250.0 mL of water?

(Multiple Choice)

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Question 32

Which of the following represents a 1.00 M aqueous solution of glucose (C₆H₁₂O₆)?

(Multiple Choice)

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Question 33

(aq) indicates that the compound is dissolved in alcohol.

(True/False)

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Question 34

Molarity is defined as moles of solute per kg of solution.

(True/False)

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Question 35

Given the following reaction: Na₂SO₄(s) + 2 C(s) → Na₂S(s) + 2 CO₂(g) How many grams of carbon are required to produce 18.4 g Na₂S(s)?

(Multiple Choice)

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Question 36

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? H₂(g) + O₂(g) → H₂O(l)

(Multiple Choice)

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Question 37

If 8.52 g each of zinc, potassium dichromate, and sulfuric acid are reacted by the reaction: 4 Zn + K₂Cr₂O₇ + 7 H₂SO₄→ 4 ZnSO₄ + 2 CrSO₄ +K₂SO₄ + 7 H₂O How many grams of potassium dichromate will be left unreacted?

(Multiple Choice)

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Question 38

Consider the gaseous reaction: N₂H₄(g) + 3 O₂(g) → 2 NO₂(g) + 2 H₂O(g) If the above reaction has a percent yield of 98.5%, what mass in grams of oxygen is needed to produce 49.0 g of NO₂(g), assuming an excess of N₂H₄?

(Multiple Choice)

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Question 39

What volume of concentrated acetic acid (CH₃CO₂H, density 1.05 g mL-1) is needed to prepare 250 mL of a 0.30 M aqueous solution?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 100

Exam 4: Chemical Reactions

306 mL of a 0.208 M solution of silver nitrate will react with 146 mL of a 0.170 M solution of sodium phosphate to produce how many grams of silver phosphate precipitate? The balanced reaction is: 3 AgNO3 + Na3PO4 → Ag3PO4 + 3 NaNO3

Given the reaction: 2KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O How many moles of H2SO4 are required to produce 2.0 moles of I2, given the other reactants are in excess?

The numbers in front of formulas in balanced equations are called stoichiometric coefficients.

What mass of MgCl2 in grams must be added to 250.0 mL of a 0.25 M MgCl2 solution to produce a 0.40 M solution, assuming no change of volume upon addition?

What volume of 6.0 M sulfuric acid is required for the preparation of 500.0 mL of 0.30 M solution?

52.5 mL of a solution were diluted to a volume of 6.25 L and then had a concentration of 3.16 M. What was the molarity of the initial solution?

Given the reaction: 2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O, How many moles of K2SO4 are produced by allowing five moles each of KMnO4, KI, and H2SO4 to react?

What volume of 2.0 M HCl, in mL, is required to dissolve a 10.0 g piece of Zn? Zn(s) + 2 HCl → ZnCl2 + H2(g)

For the reaction 2 Al + Fe2O3 → Al2O3 + 2 Fe, 2.5 g of Al (27.0 g/mol) and 7.2 g of Fe2O3 (159.8 g/mol) produce how many g of Fe (55.9 g/mol)?

Which metal will produce the most hydrogen per gram of metal?

How many grams of ZnSO4 will be made from 41.0 grams each of Zn, K2Cr2O7, and H2SO4? 4 Zn + K2Cr2O7 + 7 H2SO4 → 4 ZnSO4 + 2 CrSO4 + K2SO4 + 7 H2O

What is the molarity of a sucrose solution (C12H22O11) if 110.0 g of a 92.0% pure solid is dissolved per 250.0 mL of water?

Which of the following represents a 1.00 M aqueous solution of glucose (C6H12O6)?

(aq) indicates that the compound is dissolved in alcohol.

Molarity is defined as moles of solute per kg of solution.

Given the following reaction: Na2SO4(s) + 2 C(s) → Na2S(s) + 2 CO2(g) How many grams of carbon are required to produce 18.4 g Na2S(s)?

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? H2(g) + O2(g) → H2O(l)

If 8.52 g each of zinc, potassium dichromate, and sulfuric acid are reacted by the reaction: 4 Zn + K2Cr2O7 + 7 H2SO4→ 4 ZnSO4 + 2 CrSO4 +K2SO4 + 7 H2O How many grams of potassium dichromate will be left unreacted?

Consider the gaseous reaction: N2H4(g) + 3 O2(g) → 2 NO2(g) + 2 H2O(g) If the above reaction has a percent yield of 98.5%, what mass in grams of oxygen is needed to produce 49.0 g of NO2(g), assuming an excess of N2H4?

What volume of concentrated acetic acid (CH3CO2H, density 1.05 g mL-1) is needed to prepare 250 mL of a 0.30 M aqueous solution?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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306 mL of a 0.208 M solution of silver nitrate will react with 146 mL of a 0.170 M solution of sodium phosphate to produce how many grams of silver phosphate precipitate? The balanced reaction is: 3 AgNO₃ + Na₃PO₄ → Ag₃PO₄ + 3 NaNO₃

Given the reaction: 2KMnO₄ + 10 KI + 8 H₂SO₄→ 6 K₂SO₄ + 2 MnSO₄ + 5 I₂+ 8 H₂O How many moles of H₂SO₄ are required to produce 2.0 moles of I₂, given the other reactants are in excess?

What mass of MgCl₂ in grams must be added to 250.0 mL of a 0.25 M MgCl₂ solution to produce a 0.40 M solution, assuming no change of volume upon addition?

Given the reaction: 2 KMnO₄ + 10 KI + 8 H₂SO₄ → 6 K₂SO₄ + 2 MnSO₄ + 5 I₂ + 8 H₂O, How many moles of K₂SO₄ are produced by allowing five moles each of KMnO₄, KI, and H₂SO₄ to react?

What volume of 2.0 M HCl, in mL, is required to dissolve a 10.0 g piece of Zn? Zn(s) + 2 HCl → ZnCl₂ + H₂(g)

For the reaction 2 Al + Fe₂O₃ → Al₂O₃ + 2 Fe, 2.5 g of Al (27.0 g/mol) and 7.2 g of Fe₂O₃ (159.8 g/mol) produce how many g of Fe (55.9 g/mol)?

How many grams of ZnSO₄ will be made from 41.0 grams each of Zn, K₂Cr₂O₇, and H₂SO₄? 4 Zn + K₂Cr₂O₇ + 7 H₂SO₄ → 4 ZnSO₄ + 2 CrSO₄ + K₂SO₄ + 7 H₂O

What is the molarity of a sucrose solution (C₁₂H₂₂O₁₁) if 110.0 g of a 92.0% pure solid is dissolved per 250.0 mL of water?

Which of the following represents a 1.00 M aqueous solution of glucose (C₆H₁₂O₆)?

Given the following reaction: Na₂SO₄(s) + 2 C(s) → Na₂S(s) + 2 CO₂(g) How many grams of carbon are required to produce 18.4 g Na₂S(s)?

What is the sum of the coefficients when the following is balanced with the smallest integer coefficients? H₂(g) + O₂(g) → H₂O(l)

If 8.52 g each of zinc, potassium dichromate, and sulfuric acid are reacted by the reaction: 4 Zn + K₂Cr₂O₇ + 7 H₂SO₄→ 4 ZnSO₄ + 2 CrSO₄ +K₂SO₄ + 7 H₂O How many grams of potassium dichromate will be left unreacted?

Consider the gaseous reaction: N₂H₄(g) + 3 O₂(g) → 2 NO₂(g) + 2 H₂O(g) If the above reaction has a percent yield of 98.5%, what mass in grams of oxygen is needed to produce 49.0 g of NO₂(g), assuming an excess of N₂H₄?

What volume of concentrated acetic acid (CH₃CO₂H, density 1.05 g mL-1) is needed to prepare 250 mL of a 0.30 M aqueous solution?