Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound?

A) C3H8O B) C3H5O C) C6H16O2 D) C3H9O3 E) C3H6O3 A) C3H8O B) C3H5O C) C6H16O2 D) C3H9O3 E) C3H6O3

The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.

A) 34 B) 162 C) 86 D) 61 E) 19 A) 34 B) 162 C) 86 D) 61 E) 19

What is the mass % of oxygen in lead (II)nitrate (Pb(NO3)2)rounded to three significant figures?

A) 4.83 B) 19.3 C) 29.0 D) 14.5 E) 0.331 A) 4.83 B) 19.3 C) 29.0 D) 14.5 E) 0.331

When the following equation is balanced, the coefficient of H2 is ________. K (s) + H2O (l) → KOH (aq) + H2 (g)

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

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s)+ 3O2 (g)→ 2SO3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is ________.

A) 30 B) 29 C) 21 D) 88 E) 47 A) 30 B) 29 C) 21 D) 88 E) 47

Calcium carbide (CaC2)reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 13 g of C2H2 requires consumption of ________ g of H2O.

A) 4.5 B) 9.0 C) 18 D) 4.8 × 102 E) 4.8 × 10-2 A) 4.5 B) 9.0 C) 18 D) 4.8 × 102 E) 4.8 × 10-2

What is the mass % of carbon in dimethylsulfoxide (C2H6SO)rounded to three significant figures?

A) 25.4 B) 28.6 C) 30.7 D) 7.74 E) 78.1 A) 25.4 B) 28.6 C) 30.7 D) 7.74 E) 78.1

When the following equation is balanced, the coefficient of HNO3 is ________. HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l)

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

The molecular weight of maltose (C12H22O11), rounded to one decimal place, is ________ amu.

A) 507.2 B) 182.0 C) 15.0 D) 342.3 E) 29.0 A) 507.2 B) 182.0 C) 15.0 D) 342.3 E) 29.0

The mass % of C in methane (CH4)is ________.

A) 25.13 B) 133.6 C) 74.87 D) 92.26 E) 7.743 A) 25.13 B) 133.6 C) 74.87 D) 92.26 E) 7.743

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A ________ g sample of N2 requires 3.0 g of H2 for complete reaction.

A) 0.51 B) 0.76 C) 1.2 D) 14.0 E) 17.2 A) 0.51 B) 0.76 C) 1.2 D) 14.0 E) 17.2

Which of the following are decomposition reactions? 1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g)

A) 1, 2, and 3 B) 4 only C) 1, 2, 3, and 4 D) 2 and 3 E) 2, 3, and 4 A) 1, 2, and 3 B) 4 only C) 1, 2, 3, and 4 D) 2 and 3 E) 2, 3, and 4

How many atoms of nitrogen are in 10 g of NH4NO3?

A) 3.5 B) 1.5 × 1023 C) 3.0 × 1023 D) 1.8 E) 2 A) 3.5 B) 1.5 × 1023 C) 3.0 × 1023 D) 1.8 E) 2

Exam 3: Stoichiometry: Calculations With Chemical Formulas and Equations

Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO₂ and 1.236 g of H₂O. What is the empirical formula of the compound?

(Multiple Choice)

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Question 21

One million argon atoms is ________ mol (rounded to two significant figures)of argon atoms.

(Multiple Choice)

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Question 22

The compound responsible for the characteristic smell of garlic is allicin, C₆H₁₀OS₂. The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.

(Multiple Choice)

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Question 23

What is the mass % of oxygen in lead (II)nitrate (Pb(NO₃)₂)rounded to three significant figures?

(Multiple Choice)

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Question 24

When the following equation is balanced, the coefficient of H₂ is ________. K (s) + H₂O (l) → KOH (aq) + H₂ (g)

(Multiple Choice)

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Question 25

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s)+ 3O₂ (g)→ 2SO₃ (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O₂ produced 0.80 g of SO₃. The % yield in this experiment is ________.

(Multiple Choice)

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Question 26

A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be ________.

(Multiple Choice)

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Question 27

A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by mass. What is the empirical formula of the compound?

(Multiple Choice)

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Question 28

When the following equation is balanced, the coefficients are ________. Al(NO₃)₃ + Na₂S → Al₂S₃ + NaNO₃

(Multiple Choice)

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Question 29

How many moles of carbon monoxide are there in 36.55 g of carbon monoxide?

(Multiple Choice)

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Question 30

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)₂ (s) + C₂H₂ (g) Production of 13 g of C₂H₂ requires consumption of ________ g of H₂O.

(Multiple Choice)

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Question 31

What is the mass % of carbon in dimethylsulfoxide (C₂H₆SO)rounded to three significant figures?

(Multiple Choice)

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Question 32

When the following equation is balanced, the coefficient of HNO₃ is ________. HNO₃ (aq) + CaCO₃ (s) → Ca(NO₃)₂ (aq) + CO₂ (g) + H₂O (l)

(Multiple Choice)

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Question 33

How many carbon atoms are there in 52.06 g of carbon dioxide?

(Multiple Choice)

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Question 34

The balanced equation for the decomposition of sodium azide is ________.

(Multiple Choice)

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Question 35

The molecular weight of maltose (C₁₂H₂₂O₁₁), rounded to one decimal place, is ________ amu.

(Multiple Choice)

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Question 36

The mass % of C in methane (CH₄)is ________.

(Multiple Choice)

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Question 37

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃(g) A ________ g sample of N₂ requires 3.0 g of H₂ for complete reaction.

(Multiple Choice)

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Question 38

Which of the following are decomposition reactions? 1) CH₄ (g) + O₂ (g) → CO₂ (g) + H₂O (l) 2) CaO (s) + CO₂ (g) → CaCO₃ (s) 3) Mg (s) + O₂ (g) → MgO (s) 4) PbCO₃ (s) → PbO (s) + CO₂ (g)

(Multiple Choice)

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Question 39

How many atoms of nitrogen are in 10 g of NH₄NO₃?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 178

Exam 3: Stoichiometry: Calculations With Chemical Formulas and Equations

Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound?

One million argon atoms is ________ mol (rounded to two significant figures)of argon atoms.

The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.

What is the mass % of oxygen in lead (II)nitrate (Pb(NO3)2)rounded to three significant figures?

When the following equation is balanced, the coefficient of H2 is ________. K (s) + H2O (l) → KOH (aq) + H2 (g)

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s)+ 3O2 (g)→ 2SO3 (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The % yield in this experiment is ________.

A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be ________.

A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by mass. What is the empirical formula of the compound?

When the following equation is balanced, the coefficients are ________. Al(NO3)3 + Na2S → Al2S3 + NaNO3

How many moles of carbon monoxide are there in 36.55 g of carbon monoxide?

Calcium carbide (CaC2)reacts with water to produce acetylene (C2H2): CaC2 (s) + 2H2O (g) → Ca(OH)2 (s) + C2H2 (g) Production of 13 g of C2H2 requires consumption of ________ g of H2O.

What is the mass % of carbon in dimethylsulfoxide (C2H6SO)rounded to three significant figures?

When the following equation is balanced, the coefficient of HNO3 is ________. HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l)

How many carbon atoms are there in 52.06 g of carbon dioxide?

The balanced equation for the decomposition of sodium azide is ________.

The molecular weight of maltose (C12H22O11), rounded to one decimal place, is ________ amu.

The mass % of C in methane (CH4)is ________.

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N2 (g) + 3H2 (g) → 2NH3 (g) A ________ g sample of N2 requires 3.0 g of H2 for complete reaction.

Which of the following are decomposition reactions? 1) CH4 (g) + O2 (g) → CO2 (g) + H2O (l) 2) CaO (s) + CO2 (g) → CaCO3 (s) 3) Mg (s) + O2 (g) → MgO (s) 4) PbCO3 (s) → PbO (s) + CO2 (g)

How many atoms of nitrogen are in 10 g of NH4NO3?

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Aqueous Reactions and Solution Stoichiometry

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Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

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Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO₂ and 1.236 g of H₂O. What is the empirical formula of the compound?

The compound responsible for the characteristic smell of garlic is allicin, C₆H₁₀OS₂. The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.

What is the mass % of oxygen in lead (II)nitrate (Pb(NO₃)₂)rounded to three significant figures?

When the following equation is balanced, the coefficient of H₂ is ________. K (s) + H₂O (l) → KOH (aq) + H₂ (g)

Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental pollutant: 2S (s)+ 3O₂ (g)→ 2SO₃ (g) In a particular experiment, the reaction of 1.0 g S with 1.0 g O₂ produced 0.80 g of SO₃. The % yield in this experiment is ________.

When the following equation is balanced, the coefficients are ________. Al(NO₃)₃ + Na₂S → Al₂S₃ + NaNO₃

Calcium carbide (CaC₂)reacts with water to produce acetylene (C₂H₂): CaC₂ (s) + 2H₂O (g) → Ca(OH)₂ (s) + C₂H₂ (g) Production of 13 g of C₂H₂ requires consumption of ________ g of H₂O.

What is the mass % of carbon in dimethylsulfoxide (C₂H₆SO)rounded to three significant figures?

When the following equation is balanced, the coefficient of HNO₃ is ________. HNO₃ (aq) + CaCO₃ (s) → Ca(NO₃)₂ (aq) + CO₂ (g) + H₂O (l)

The molecular weight of maltose (C₁₂H₂₂O₁₁), rounded to one decimal place, is ________ amu.

The mass % of C in methane (CH₄)is ________.

Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃(g) A ________ g sample of N₂ requires 3.0 g of H₂ for complete reaction.

Which of the following are decomposition reactions? 1) CH₄ (g) + O₂ (g) → CO₂ (g) + H₂O (l) 2) CaO (s) + CO₂ (g) → CaCO₃ (s) 3) Mg (s) + O₂ (g) → MgO (s) 4) PbCO₃ (s) → PbO (s) + CO₂ (g)

How many atoms of nitrogen are in 10 g of NH₄NO₃?