Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen. 4Al(s) + 3O2(g) → 2Al2O3(s) A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

A) 155.8 g B) 200.2 g C) 249.9 g D) 311.7 g E) 374.9 g A) 155.8 g B) 200.2 g C) 249.9 g D) 311.7 g E) 374.9 g

Balance the following equation: C8H18O3(l) + O2(g) → H2O(g) + CO2(g)

A) C8H18O3(l) + 8O2(g) → 9H2O(g) + 8CO2(g) B) C8H18O3(l) + 11O2(g) → 9H2O(g) + 8CO2(g) C) 2C8H18O3(l) + 22O2(g) → 9H2O(g) + 16CO2(g) D) C8H18O3(l) + 13O2(g) → 18H2O(g) + 8CO2(g) E) 2C8H18O3(l) + 17O2(g) → 18H2O(g) + 16CO2(g) A) C8H18O3(l) + 8O2(g) → 9H2O(g) + 8CO2(g) B) C8H18O3(l) + 11O2(g) → 9H2O(g) + 8CO2(g) C) 2C8H18O3(l) + 22O2(g) → 9H2O(g) + 16CO2(g) D) C8H18O3(l) + 13O2(g) → 18H2O(g) + 8CO2(g) E) 2C8H18O3(l) + 17O2(g) → 18H2O(g) + 16CO2(g)

Balance the following equation: UO2(s) + HF(l) → UF4(s) + H2O(l)

A) UO2(s) + 2HF(l) → UF4(s) + H2O(l) B) UO2(s) + 4HF(l) → UF4(s) + 2H2O(l) C) UO2(s) + H4F4(l) → UF4 (s) + H4O2(l) D) UO2(s) + 4HF(l) → UF4(s) + 4H2O(l) E) UO2(s) + 8HF(l) → 2UF4(s) + 4H2O(l) A) UO2(s) + 2HF(l) → UF4(s) + H2O(l) B) UO2(s) + 4HF(l) → UF4(s) + 2H2O(l) C) UO2(s) + H4F4(l) → UF4 (s) + H4O2(l) D) UO2(s) + 4HF(l) → UF4(s) + 4H2O(l) E) UO2(s) + 8HF(l) → 2UF4(s) + 4H2O(l)

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl3. What mass of chlorine gas is needed to react completely with 163 g of aluminum?

A) 214 g B) 245 g C) 321 g D) 489 g E) 643 g A) 214 g B) 245 g C) 321 g D) 489 g E) 643 g

Balance the following equation: B2O3(s) + HF(l) → BF3(g) + H2O(l)

A) B2O3(s) + 6HF(l) → 2BF3(g) + 3H2O(l) B) B2O3 (s) + H6F6(l) → B2F6(g) + H6O3(l) C) B2O3 (s) + 2HF(l) → 2BF3(g) + H2O(l) D) B2O3 (s) + 3HF(l) → 2BF3(g) + 3H2O(l) E) B2O3 (s) + 6HF(l) → 2BF3(g) + 6H2O(l) A) B2O3(s) + 6HF(l) → 2BF3(g) + 3H2O(l) B) B2O3 (s) + H6F6(l) → B2F6(g) + H6O3(l) C) B2O3 (s) + 2HF(l) → 2BF3(g) + H2O(l) D) B2O3 (s) + 3HF(l) → 2BF3(g) + 3H2O(l) E) B2O3 (s) + 6HF(l) → 2BF3(g) + 6H2O(l)

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g) → 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%

Household sugar, sucrose, has the molecular formula C12H22O11. What is the percent 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%

What is the percent yield for the reaction PCl3(g) + Cl2(g) → PCl5(g) If 119.3 g of PCl5 (M = 208.2 g/mol) are formed when 61.3 g of Cl2 ( = 70.91 g/mol) react with excess PCl3?

A) 195% B) 85.0% C) 66.3% D) 51.4% E) 43.7% A) 195% B) 85.0% C) 66.3% D) 51.4% E) 43.7%

Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced] Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

A) 1880 g B) 940. g C) 900. g D) 470 g E) 56.3 g A) 1880 g B) 940. g C) 900. g D) 470 g E) 56.3 g

Exam 3: Stoichiometry of Formulas and Equations

Aluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when aluminum reacts with oxygen. 4Al(s) + 3O₂(g) → 2Al₂O₃(s) A mixture of 82.49 g of aluminum ( = 26.98 g/mol) and 117.65 g of oxygen ( = 32.00g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

(Multiple Choice)

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Question 21

Sodium bromate is used in a mixture which dissolves gold from its ores. Calculate the mass in grams of 4.68 mol of sodium bromate.

(Multiple Choice)

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Question 22

One mole of methane (CH₄) contains a total of 3 × 10²⁴ atoms.

(True/False)

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Question 23

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

(Multiple Choice)

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Question 24

Balance the following equation: C₈H₁₈O₃(l) + O₂(g) → H₂O(g) + CO₂(g)

(Multiple Choice)

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Question 25

A compound of bromine and fluorine is used to make UF₆, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.

(Multiple Choice)

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Question 26

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?

(Multiple Choice)

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Question 27

Aluminum oxide, Al₂O₃, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al₂O₃.

(Multiple Choice)

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Question 28

Balance the following equation: UO₂(s) + HF(l) → UF₄(s) + H₂O(l)

(Multiple Choice)

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Question 29

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl₃. What mass of chlorine gas is needed to react completely with 163 g of aluminum?

(Multiple Choice)

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Question 30

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N₂(g) + 3H₂(g) → 2NH₃(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

(Multiple Choice)

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Question 31

Balance the following equation: B₂O₃(s) + HF(l) → BF₃(g) + H₂O(l)

(Multiple Choice)

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Question 32

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g) → 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?

(Multiple Choice)

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Question 33

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

(Multiple Choice)

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Question 34

What is the percent yield for the reaction PCl₃(g) + Cl₂(g) → PCl₅(g) If 119.3 g of PCl₅ (M = 208.2 g/mol) are formed when 61.3 g of Cl₂ ( = 70.91 g/mol) react with excess PCl3?

(Multiple Choice)

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Question 35

Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

(Multiple Choice)

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Question 36

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp, and textiles). SO₂(g) + 2Cl₂(g) → SOCl₂(g) + Cl₂O(g) If 0.400 mol of Cl₂ reacts with excess SO₂, how many moles of Cl₂O are formed?

(Multiple Choice)

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Question 37

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.

(Multiple Choice)

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Question 38

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

(Multiple Choice)

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Question 39

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

(Multiple Choice)

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Question 40

Showing 21 - 40 of 70

Exam 3: Stoichiometry of Formulas and Equations

Sodium bromate is used in a mixture which dissolves gold from its ores. Calculate the mass in grams of 4.68 mol of sodium bromate.

One mole of methane (CH4) contains a total of 3 × 1024 atoms.

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Balance the following equation: C8H18O3(l) + O2(g) → H2O(g) + CO2(g)

A compound of bromine and fluorine is used to make UF6, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.

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?

Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

Balance the following equation: UO2(s) + HF(l) → UF4(s) + H2O(l)

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl3. What mass of chlorine gas is needed to react completely with 163 g of aluminum?

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N2(g) + 3H2(g) → 2NH3(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Balance the following equation: B2O3(s) + HF(l) → BF3(g) + H2O(l)

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P4(s) + 3O2(g) → 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?

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

What is the percent yield for the reaction PCl3(g) + Cl2(g) → PCl5(g) If 119.3 g of PCl5 (M = 208.2 g/mol) are formed when 61.3 g of Cl2 ( = 70.91 g/mol) react with excess PCl3?

Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced] Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp, and textiles). SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g) If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?

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.

A normal breath takes in about 1.0 L of air. Assuming that air has an average molar mass of 28.8g, and that its density is 0.97 g/L, how many molecules of air do you take in with each breath?

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

Keys to Studying Chemistry Definitions, Units, and Problem Solving

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

One mole of methane (CH₄) contains a total of 3 × 10²⁴ atoms.

Balance the following equation: C₈H₁₈O₃(l) + O₂(g) → H₂O(g) + CO₂(g)

A compound of bromine and fluorine is used to make UF₆, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.

Aluminum oxide, Al₂O₃, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al₂O₃.

Balance the following equation: UO₂(s) + HF(l) → UF₄(s) + H₂O(l)

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl₃. What mass of chlorine gas is needed to react completely with 163 g of aluminum?

Ammonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine. N₂(g) + 3H₂(g) → 2NH₃(g) How many grams of nitrogen are needed to produce 325 grams of ammonia?

Balance the following equation: B₂O₃(s) + HF(l) → BF₃(g) + H₂O(l)

Tetraphosphorus hexaoxide ( = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas. P₄(s) + 3O₂(g) → 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?

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

What is the percent yield for the reaction PCl₃(g) + Cl₂(g) → PCl₅(g) If 119.3 g of PCl₅ (M = 208.2 g/mol) are formed when 61.3 g of Cl₂ ( = 70.91 g/mol) react with excess PCl3?

Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

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.