Calculate the molar mass of tetraphosphorus decaoxide,P4O10,a corrosive substance which can be used as a drying agent.

A) 469.73 g/mol B) 283.89 g/mol C) 190.97 g/mol D) 139.88 g/mol E) 94.97 g/mol A) 469.73 g/mol B) 283.89 g/mol C) 190.97 g/mol D) 139.88 g/mol E) 94.97 g/mol

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s)+ Br2(l) $\to$Al2Br6(s)[unbalanced] How many moles of Al are needed to form 2.43 mol of Al2Br6?

A) 7.29 mol B) 4.86 mol C) 2.43 mol D) 1.62 mol E) 1.22 mol A) 7.29 mol B) 4.86 mol C) 2.43 mol D) 1.62 mol E) 1.22 mol

Calculate the molar mass of Ca(BO2)2·6H2O.

A) 273.87 g/mol B) 233.79 g/mol C) 183.79 g/mol D) 174.89 g/mol E) 143.71 g/mol A) 273.87 g/mol B) 233.79 g/mol C) 183.79 g/mol D) 174.89 g/mol E) 143.71 g/mol

Aluminum oxide (used as an adsorbent or a catalyst for organic reactions)forms when aluminum reacts with oxygen. 4Al(s)+ 3O2(g) $\to$ 2Al2O3(s) A mixture of 82.49 g of aluminum ( = 26.98 g/mol)and 117.65 g of oxygen ( = 32.00 g/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

Calculate the molar mass of (NH4)3AsO4.

A) 417.80 g/mol B) 193.03 g/mol C) 165.02 g/mol D) 156.96 g/mol E) 108.96 g/mol A) 417.80 g/mol B) 193.03 g/mol C) 165.02 g/mol D) 156.96 g/mol E) 108.96 g/mol

Balance the following equation: C8H18O3(l)+ O2(g) $\to$ H2O(g)+ CO2(g)

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

Exam 3: Stoichiometry of Formulas and Equations

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.If its molar mass is between 158 and 167 g/mol,what is its molecular formula?

(Multiple Choice)

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Question 41

The formula CH₃O_0.5 is an example of an empirical formula.

(True/False)

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Question 42

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) $\to$ 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 43

In a correctly balanced equation,the number of reactant molecules must equal the number of product molecules.

(True/False)

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Question 44

Calculate the molar mass of tetraphosphorus decaoxide,P₄O₁₀,a corrosive substance which can be used as a drying agent.

(Multiple Choice)

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Question 45

Hydroxylamine nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.Determine its empirical formula.

(Multiple Choice)

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Question 46

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s)+ Br₂(l) $\to$ Al₂Br₆(s)[unbalanced] How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

(Multiple Choice)

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Question 47

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?

(Multiple Choice)

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Question 48

You are provided with a 250 mL volumetric flask,deionized water and solid NaOH.How much NaOH should be weighed out in order to make 250.mL of 0.100 M solution?

(Short Answer)

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Question 49

One mole of methane (CH₄)contains a total of 3 $\times$ 10²⁴ atoms.

(True/False)

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Question 50

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.What is its empirical formula?

(Multiple Choice)

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Question 51

Calculate the molar mass of Ca(BO₂)₂·6H₂O.

(Multiple Choice)

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Question 52

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.

(Multiple Choice)

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Question 53

One mole of O₂ has a mass of 16.0 g.

(True/False)

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Question 54

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

(Multiple Choice)

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Question 55

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

(Multiple Choice)

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Question 56

Calculate the molar mass of (NH₄)₃AsO₄.

(Multiple Choice)

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Question 57

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus.What is its empirical formula?

(Short Answer)

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Question 58

For a sample consisting of 2.50 g of methane,CH₄,calculate a.the number of moles of methane present. b.the total number of atoms present.

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Question 59

Balance the following equation: C₈H₁₈O₃(l)+ O₂(g) $\to$ H₂O(g)+ CO₂(g)

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Question 60

Showing 41 - 60 of 90

The formula CH₃O_0.5 is an example of an empirical formula.

In a correctly balanced equation,the number of reactant molecules must equal the number of product molecules.

Calculate the molar mass of tetraphosphorus decaoxide,P₄O₁₀,a corrosive substance which can be used as a drying agent.

Hydroxylamine nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.Determine its empirical formula.

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s)+ Br₂(l) $\to$ Al₂Br₆(s)[unbalanced] How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

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?

You are provided with a 250 mL volumetric flask,deionized water and solid NaOH.How much NaOH should be weighed out in order to make 250.mL of 0.100 M solution?

One mole of methane (CH₄)contains a total of 3 $\times$ 10²⁴ atoms.

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.What is its empirical formula?

Calculate the molar mass of Ca(BO₂)₂·6H₂O.

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.

One mole of O₂ has a mass of 16.0 g.

Calculate the molar mass of (NH₄)₃AsO₄.

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus.What is its empirical formula?

For a sample consisting of 2.50 g of methane,CH₄,calculate a.the number of moles of methane present. b.the total number of atoms present.

Balance the following equation: C₈H₁₈O₃(l)+ O₂(g) $\to$ H₂O(g)+ CO₂(g)

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 Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

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 Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Exam 3: Stoichiometry of Formulas and Equations

The formula CH3O0.5 is an example of an empirical formula.

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) →\to→ SOCl2(g)+ Cl2O(g) If 0.400 mol of Cl2 reacts with excess SO2,how many moles of Cl2O are formed?

In a correctly balanced equation,the number of reactant molecules must equal the number of product molecules.

Calculate the molar mass of tetraphosphorus decaoxide,P4O10,a corrosive substance which can be used as a drying agent.

Hydroxylamine nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.Determine its empirical formula.

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s)+ Br2(l) →\to→ Al2Br6(s)[unbalanced] How many moles of Al are needed to form 2.43 mol of Al2Br6?

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?

You are provided with a 250 mL volumetric flask,deionized water and solid NaOH.How much NaOH should be weighed out in order to make 250.mL of 0.100 M solution?

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

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O.What is its empirical formula?

Calculate the molar mass of Ca(BO2)2·6H2O.

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.

One mole of O2 has a mass of 16.0 g.

Calculate the molar mass of (NH4)3AsO4.

Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus.What is its empirical formula?

For a sample consisting of 2.50 g of methane,CH4,calculate a.the number of moles of methane present. b.the total number of atoms present.

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

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 Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

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 Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

The formula CH₃O_0.5 is an example of an empirical formula.

Calculate the molar mass of tetraphosphorus decaoxide,P₄O₁₀,a corrosive substance which can be used as a drying agent.

Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s)+ Br₂(l) $\to$ Al₂Br₆(s)[unbalanced] How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

One mole of methane (CH₄)contains a total of 3 $\times$ 10²⁴ atoms.

Terephthalic acid,used in the production of polyester fibers and films,is composed of carbon,hydrogen,and oxygen.When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO₂ and 0.226 g H₂O.What is its empirical formula?

Calculate the molar mass of Ca(BO₂)₂·6H₂O.

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.

One mole of O₂ has a mass of 16.0 g.

Calculate the molar mass of (NH₄)₃AsO₄.

For a sample consisting of 2.50 g of methane,CH₄,calculate a.the number of moles of methane present. b.the total number of atoms present.

Balance the following equation: C₈H₁₈O₃(l)+ O₂(g) $\to$ H₂O(g)+ CO₂(g)