Tetraphosphorus hexaoxide (? = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g) $\rightarrow$ P4O6(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?

A) 57.5% B) 48.8% C) 38.0% D) 32.4% E) 16.3% A) 57.5% B) 48.8% C) 38.0% D) 32.4% E) 16.3% B

Calculate the mass in grams of 8.35 * 1022 molecules of CBr4.

A) 0.0217 g B) 0.139 g C) 7.21 g D) 12.7 g E) 46.0 g A) 0.0217 g B) 0.139 g C) 7.21 g D) 12.7 g E) 46.0 g

In the combustion analysis of 0.1127 g of glucose (C6H12O6), what mass, in grams, of CO2 would be produced?

A) 0.0451 g B) 0.0825 g C) 0.1652 g D) 0.4132 g E) 1.466 g A) 0.0451 g B) 0.0825 g C) 0.1652 g D) 0.4132 g E) 1.466 g

Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass?

A) 26.7% B) 33.3% C) 41.4% D) 42.1% E) 52.8% A) 26.7% B) 33.3% C) 41.4% D) 42.1% E) 52.8%

Aqueous potassium iodate (KIO3) and potassium iodide (KI) react in the presence of dilute hydrochloric acid, as shown below. KIO3(aq) + 5KI(aq) + 6HCl(aq) $\rightarrow$ 3I2(aq) + 6KCl(aq) + 3H2O(l) What mass of iodine (I2) is formed when 50.0 mL of 0.020 M KIO3 solution reacts with an excess of KI and HCl?

A) 0.13 g I2 B) 0.25 g I2 C) 0.38 g I2 D) 0.76 g I2 E) None of these answers is correct. A) 0.13 g I2 B) 0.25 g I2 C) 0.38 g I2 D) 0.76 g I2 E) None of these answers is correct.

Exam 3: Stoichiometry of Formulas and Equations

Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO₃)₂.

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(Multiple Choice)

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Question 1

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Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

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Question 2

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Tetraphosphorus hexaoxide (? = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g) $\rightarrow$ P₄O₆(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

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Question 3

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Phosphorus pentachloride, PCl₅, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl₅.

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Question 4

One mole of O₂ has a mass of 16.0 g.

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Question 5

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 * 10²⁰ molecules of SO₃.

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Question 6

Calculate the mass in grams of 8.35 * 10²² molecules of CBr₄.

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Question 7

Calcium fluoride, CaF₂, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass.

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Question 8

Analysis of a carbohydrate showed that it consisted of 40.0 % C, 6.71 % H and 53.3 % O by mass. Its molecular mass was found to be between 140 and 160 amu. What is the molecular formula of this compound?

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Question 9

Determine the percent composition of potassium dichromate, K₂Cr₂O₇.

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Question 10

Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron. 3Mg(s) + 2FeCl₃(s) $\rightarrow$ 3MgCl₂(s) + 2Fe(s) A mixture of 41.0 g of magnesium (? = 24.31 g/mol) and 175 g of iron(III) chloride (? = 162.2 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

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Question 11

In the combustion analysis of 0.1127 g of glucose (C₆H₁₂O₆), what mass, in grams, of CO₂ would be produced?

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Question 12

Household sugar, sucrose, has the molecular formula C₁₂H₂₂O₁₁. What is the % of carbon in sucrose, by mass?

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Question 13

Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.

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Question 14

Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

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Question 15

When a solution is diluted with water, the ratio of the initial to final volumes of solution is equal to the ratio of final to initial molarities.

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Question 16

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

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Question 17

Which of the following samples has the most moles of the compound?

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Question 18

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4 $\pi$ r³/3; density of mercury = 13.6 g/cm³)

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Question 19

Aqueous potassium iodate (KIO₃) and potassium iodide (KI) react in the presence of dilute hydrochloric acid, as shown below. KIO₃(aq) + 5KI(aq) + 6HCl(aq) $\rightarrow$ 3I₂(aq) + 6KCl(aq) + 3H₂O(l) What mass of iodine (I₂) is formed when 50.0 mL of 0.020 M KIO₃ solution reacts with an excess of KI and HCl?

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Question 20

Showing 1 - 20 of 96

Exam 3: Stoichiometry of Formulas and Equations

Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO3)2.

Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

Tetraphosphorus hexaoxide (? = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g) →\rightarrow→ P4O6(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?

Phosphorus pentachloride, PCl5, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl5.

One mole of O2 has a mass of 16.0 g.

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 * 1020 molecules of SO3.

Calculate the mass in grams of 8.35 * 1022 molecules of CBr4.

Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass.

Analysis of a carbohydrate showed that it consisted of 40.0 % C, 6.71 % H and 53.3 % O by mass. Its molecular mass was found to be between 140 and 160 amu. What is the molecular formula of this compound?

Determine the percent composition of potassium dichromate, K2Cr2O7.

In the combustion analysis of 0.1127 g of glucose (C6H12O6), what mass, in grams, of CO2 would be produced?

Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass?

Calcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165 mL of 0.688 M calcium chloride to 925.0 mL.

Hydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

When a solution is diluted with water, the ratio of the initial to final volumes of solution is equal to the ratio of final to initial molarities.

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

Which of the following samples has the most moles of the compound?

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4 π\piπ r3/3; density of mercury = 13.6 g/cm3)

Keys to the Study of Chemistry

The Components of Matter

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Lead (II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO₃)₂.

Tetraphosphorus hexaoxide (? = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g) $\rightarrow$ P₄O₆(s) If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

Phosphorus pentachloride, PCl₅, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl₅.

One mole of O₂ has a mass of 16.0 g.

Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 * 10²⁰ molecules of SO₃.

Calculate the mass in grams of 8.35 * 10²² molecules of CBr₄.

Calcium fluoride, CaF₂, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass.

Determine the percent composition of potassium dichromate, K₂Cr₂O₇.

In the combustion analysis of 0.1127 g of glucose (C₆H₁₂O₆), what mass, in grams, of CO₂ would be produced?

Household sugar, sucrose, has the molecular formula C₁₂H₂₂O₁₁. What is the % of carbon in sucrose, by mass?

How many atoms are in a drop of mercury that has a diameter of 1.0 mm? (Volume of a sphere is 4 $\pi$ r³/3; density of mercury = 13.6 g/cm³)