How many mL of hexadecane (C16H34) are needed to react with 0.050 mol O2, assuming complete combustion occurs? The density of C16H34 is 0.80 g/mL.

A) 0.99 mL B) 0.37 mL C) 0.58 mL D) 0.46 mL E) 0.89 mL A) 0.99 mL B) 0.37 mL C) 0.58 mL D) 0.46 mL E) 0.89 mL C

If the combustion of fossil fuels adds about 5 $\times$ 1012 kg of carbon to the atmosphere as CO2 each year, how much oxygen is required to produce this amount of carbon dioxide?

A) about 1.3 1012 kg B) about 1.3 1013 kg C) about 2.6 1012 kg D) about 2.6 1013 kg E) about 6.7 1012 kg A) about 1.3 1012 kg B) about 1.3 1013 kg C) about 2.6 1012 kg D) about 2.6 1013 kg E) about 6.7 1012 kg

Burning coal that contains sulfur releases sulfur dioxide gas into the atmosphere, where it combines with water to form sulfurous and sulfuric acid, thereby producing acid rain. Assume sulfur in coal is in the form of pyrite (FeS2(s)), which reacts with molecular oxygen to produce Fe2O3(s) and SO2(g). Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.

A) 16 B) 14 C) 23 D) 25 E) 18 A) 16 B) 14 C) 23 D) 25 E) 18

Like many metals, manganese reacts with halogens to give metal halides. How many grams of MnF3 can be produced using excess fluorine and 5.49 g of Mn? (molar masses: Mn = 54.9 g/mol, F 19.0 g/mol) 2Mn(s) 3F2(g) 2MnF3(s)

The answer of Like many metals, manganese reacts with halogens...

Exam 3: Stoichiometry: Mass, Formulas, and Reactions

In a demonstration of the complete combustion of propane (C₃H₈) with oxygen (O₂), several balloons were prepared with various proportions by volume of propane and oxygen. The loudest explosion occurred for the balloon with the correct stoichiometric proportions of the gases. Which balloon had the loudest explosion? Note that the number of molecules of a gas is proportional to the volume of the gas at a given pressure and temperature.

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Question 1

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How many mL of hexadecane (C₁₆H₃₄) are needed to react with 0.050 mol O₂, assuming complete combustion occurs? The density of C₁₆H₃₄ is 0.80 g/mL.

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What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 12.00 g water?

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One reaction that occurs during the deployment of an air bag is shown below, where sodium metal reacts with potassium nitrate. If 5.10 g of sodium and 305 g of potassium nitrate react in an airbag, how many grams of KNO₃ remain because of the limited amount of sodium present? 10Na(s) 2KNO₃(s) K₂O(s) 5Na₂O(s) N₂(g)

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Question 4

If the combustion of fossil fuels adds about 5 $\times$ 10¹² kg of carbon to the atmosphere as CO₂ each year, how much oxygen is required to produce this amount of carbon dioxide?

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Question 5

A range of organic molecules can undergo combustion. Pyridine (C₅H₅N) undergoes combustion in the unbalanced reaction shown below. Write the balanced equation, and find the percent yield for the reaction if 10.0 g of pyridine yields 18.1 g of carbon dioxide. C₅H₅N O₂ H₂O CO₂ NO

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Question 6

Arizona was the site of a 400,000-acre wildfire in June 2002. How much carbon dioxide was produced by this fire? Assume that the density of carbon on the acreage was 10 kg/m² and that 50% of the biomass burned. (10,000 m² = 2.47 acre)

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Question 7

Burning coal that contains sulfur releases sulfur dioxide gas into the atmosphere, where it combines with water to form sulfurous and sulfuric acid, thereby producing acid rain. Assume sulfur in coal is in the form of pyrite (FeS₂(s)), which reacts with molecular oxygen to produce Fe₂O₃(s) and SO₂(g). Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.

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Question 8

In a self-contained breathing apparatus, potassium superoxide, KO₂, reacts with carbon dioxide to form potassium carbonate and oxygen. Identify the limiting reactant and determine the amount of oxygen gas, in moles, that can be produced from 250 g of KO₂ and 450 g of CO₂. 4KO₂(s) 2CO₂(g) 2K₂CO₃(s) 3O₂(g)

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Question 9

Methylheptenone (MHP) is used in producing lemon fragrances and flavors. It contains the elements carbon, hydrogen, and oxygen. The complete combustion of 192 mg of MHP produces 536 mg of carbon dioxide and 192 mg water. Mass spectrometry experiments showed that its molar mass is less than 200 g/mol. What is the molecular formula of MHP?

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Question 10

An iron ore, magnetite, contains only iron and oxygen. In refining 100.0 g of the ore, 72.35 g of iron are obtained. What is the empirical formula of the ore?

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Question 11

In one analysis, 3.01 10¹³ molecules of ozone were found in 1.00 mL of an air sample. How many moles of ozone is this?

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Question 12

Acetaminophen is a common medication used to treat pain and relieve fever. Mass analysis shows that the composition of acetaminophen is 63.56% C, 6.00% H, 9.27% N, and the remainder of the mass is oxygen. Determine the empirical formula of acetaminophen.

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Question 13

Azobenzene is a highly colored organic compound. Many diazo dyes used in coloring of clothing are based on an azobenzene core. The elemental analysis of azobenzene provides 79.10% carbon, 5.53% hydrogen, and the rest is nitrogen. It has a molar mass of 182.23 g/mol. What is the molecular formula of azobenzene?

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Question 14

For movie night, Annabelle popped two bags of popcorn. In Bag 1, 654 of a possible 1,213 kernels popped. In Bag 2, 343 of 690 kernels popped. Identify the bag with the highest popcorn yield and report this percent yield.

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Question 15

Balance the following combustion reaction and report the sum of the stoichiometric coefficients. C₄H₈S₂ O₂ CO₂ H₂O __SO₃

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Question 16

Like many metals, manganese reacts with halogens to give metal halides. How many grams of MnF₃ can be produced using excess fluorine and 5.49 g of Mn? (molar masses: Mn = 54.9 g/mol, F 19.0 g/mol) 2Mn(s) 3F₂(g) 2MnF₃(s)

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Question 17

Ammonia undergoes combustion to produce nitrogen monoxide and water, both as gases. Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.

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Question 18

Which statements regarding combustion analysis to determine percent composition are not correct? I. The mass of oxygen in the sample compound can be determined from the mass of carbon dioxide that is produced. II. If a compound contains an element other than carbon and hydrogen, combustion analysis cannot be used to determine its empirical formula. III. Combustion analysis data alone is not sufficient to determine the molecular formula with certainty. IV. If some CO is produced rather than all CO₂, then the empirical formula that is calculated will be too high in carbon.

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Question 19

How many total atoms are there in one mole of water?

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Question 20

Showing 1 - 20 of 141

How many mL of hexadecane (C₁₆H₃₄) are needed to react with 0.050 mol O₂, assuming complete combustion occurs? The density of C₁₆H₃₄ is 0.80 g/mL.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 12.00 g water?

If the combustion of fossil fuels adds about 5 $\times$ 10¹² kg of carbon to the atmosphere as CO₂ each year, how much oxygen is required to produce this amount of carbon dioxide?

A range of organic molecules can undergo combustion. Pyridine (C₅H₅N) undergoes combustion in the unbalanced reaction shown below. Write the balanced equation, and find the percent yield for the reaction if 10.0 g of pyridine yields 18.1 g of carbon dioxide. C₅H₅N O₂ H₂O CO₂ NO

Arizona was the site of a 400,000-acre wildfire in June 2002. How much carbon dioxide was produced by this fire? Assume that the density of carbon on the acreage was 10 kg/m² and that 50% of the biomass burned. (10,000 m² = 2.47 acre)

An iron ore, magnetite, contains only iron and oxygen. In refining 100.0 g of the ore, 72.35 g of iron are obtained. What is the empirical formula of the ore?

In one analysis, 3.01 10¹³ molecules of ozone were found in 1.00 mL of an air sample. How many moles of ozone is this?

Acetaminophen is a common medication used to treat pain and relieve fever. Mass analysis shows that the composition of acetaminophen is 63.56% C, 6.00% H, 9.27% N, and the remainder of the mass is oxygen. Determine the empirical formula of acetaminophen.

For movie night, Annabelle popped two bags of popcorn. In Bag 1, 654 of a possible 1,213 kernels popped. In Bag 2, 343 of 690 kernels popped. Identify the bag with the highest popcorn yield and report this percent yield.

Balance the following combustion reaction and report the sum of the stoichiometric coefficients. C₄H₈S₂ O₂ CO₂ H₂O __SO₃

Like many metals, manganese reacts with halogens to give metal halides. How many grams of MnF₃ can be produced using excess fluorine and 5.49 g of Mn? (molar masses: Mn = 54.9 g/mol, F 19.0 g/mol) 2Mn(s) 3F₂(g) 2MnF₃(s)

Ammonia undergoes combustion to produce nitrogen monoxide and water, both as gases. Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.

How many total atoms are there in one mole of water?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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Exam 3: Stoichiometry: Mass, Formulas, and Reactions

How many mL of hexadecane (C16H34) are needed to react with 0.050 mol O2, assuming complete combustion occurs? The density of C16H34 is 0.80 g/mL.

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 12.00 g water?

If the combustion of fossil fuels adds about 5 ×\times× 1012 kg of carbon to the atmosphere as CO2 each year, how much oxygen is required to produce this amount of carbon dioxide?

A range of organic molecules can undergo combustion. Pyridine (C5H5N) undergoes combustion in the unbalanced reaction shown below. Write the balanced equation, and find the percent yield for the reaction if 10.0 g of pyridine yields 18.1 g of carbon dioxide. C5H5N O2 H2O CO2 NO

Arizona was the site of a 400,000-acre wildfire in June 2002. How much carbon dioxide was produced by this fire? Assume that the density of carbon on the acreage was 10 kg/m2 and that 50% of the biomass burned. (10,000 m2 = 2.47 acre)

An iron ore, magnetite, contains only iron and oxygen. In refining 100.0 g of the ore, 72.35 g of iron are obtained. What is the empirical formula of the ore?

In one analysis, 3.01 1013 molecules of ozone were found in 1.00 mL of an air sample. How many moles of ozone is this?

Acetaminophen is a common medication used to treat pain and relieve fever. Mass analysis shows that the composition of acetaminophen is 63.56% C, 6.00% H, 9.27% N, and the remainder of the mass is oxygen. Determine the empirical formula of acetaminophen.

For movie night, Annabelle popped two bags of popcorn. In Bag 1, 654 of a possible 1,213 kernels popped. In Bag 2, 343 of 690 kernels popped. Identify the bag with the highest popcorn yield and report this percent yield.

Balance the following combustion reaction and report the sum of the stoichiometric coefficients.__ C4H8S2 __O2 __CO2 __H2O __SO3

Like many metals, manganese reacts with halogens to give metal halides. How many grams of MnF3 can be produced using excess fluorine and 5.49 g of Mn? (molar masses: Mn = 54.9 g/mol, F 19.0 g/mol) 2Mn(s) 3F2(g) 2MnF3(s)

Ammonia undergoes combustion to produce nitrogen monoxide and water, both as gases. Write the balanced equation for this reaction and report the sum of the stoichiometric coefficients, written as integers.

How many total atoms are there in one mole of water?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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How many mL of hexadecane (C₁₆H₃₄) are needed to react with 0.050 mol O₂, assuming complete combustion occurs? The density of C₁₆H₃₄ is 0.80 g/mL.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 12.00 g water?

If the combustion of fossil fuels adds about 5 $\times$ 10¹² kg of carbon to the atmosphere as CO₂ each year, how much oxygen is required to produce this amount of carbon dioxide?

A range of organic molecules can undergo combustion. Pyridine (C₅H₅N) undergoes combustion in the unbalanced reaction shown below. Write the balanced equation, and find the percent yield for the reaction if 10.0 g of pyridine yields 18.1 g of carbon dioxide. C₅H₅N O₂ H₂O CO₂ NO

Arizona was the site of a 400,000-acre wildfire in June 2002. How much carbon dioxide was produced by this fire? Assume that the density of carbon on the acreage was 10 kg/m² and that 50% of the biomass burned. (10,000 m² = 2.47 acre)

In one analysis, 3.01 10¹³ molecules of ozone were found in 1.00 mL of an air sample. How many moles of ozone is this?

Balance the following combustion reaction and report the sum of the stoichiometric coefficients. C₄H₈S₂ O₂ CO₂ H₂O __SO₃

Like many metals, manganese reacts with halogens to give metal halides. How many grams of MnF₃ can be produced using excess fluorine and 5.49 g of Mn? (molar masses: Mn = 54.9 g/mol, F 19.0 g/mol) 2Mn(s) 3F₂(g) 2MnF₃(s)