A sample of water (H2O) contains 1.81 *1024 molecules.How many moles of atoms are there in this sample?

A) 1.00 B) 2.00 C) 3.01 D) 6.01 E) 9.02 A) 1.00 B) 2.00 C) 3.01 D) 6.01 E) 9.02

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P4O10 (283.9 g/mol) with 12.00 g water (18.02 g/mol).What was the percent yield for this reaction?

A) 78.62% B) 101.1% C) 92.70% D) 84.00% E) 52.70% A) 78.62% B) 101.1% C) 92.70% D) 84.00% E) 52.70%

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Baking soda (NaHCO₃, 84.0 g/mol) can react with acids such as lactic acid (HC ₃H₅O₃, 90.1 g/mol) to generate the carbon dioxide gas needed to make baked goods rise.If sufficient lactic acid is present to completely react with 20.4 g NaHCO₃, how many moles of CO₂ (44.01 g/mol) are generated? HC₃ H₅O₃ (aq) + NaHCO₃ (s) $\rightarrow$ H₂O(l) + CO₂ (g) + NaC₃H₅O₃ (aq)

(Multiple Choice)

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Question 21

Caffeine has an elemental analysis of 49.48% C, 5.190% H, 16.47% O, and 28.85% N.It has a molar mass of 194.19 g/mol.What is the molecular formula of caffeine?

(Multiple Choice)

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Question 22

A sample of water (H₂O) contains 1.81 *10²⁴ molecules.How many moles of atoms are there in this sample?

(Multiple Choice)

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Question 23

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 10² g CO and 8.00 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

(Short Answer)

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Question 24

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

(Essay)

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Question 25

The average adult exhales about 1.0 kg of carbon dioxide each day.How much oxygen is needed in metabolizing glucose (C₆H₁₂O₆, 180.16 g/mol) to make that much carbon dioxide?

(Multiple Choice)

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Question 26

A gas that is produced when fruit ripens contains 85.62% C and 14.38% H by mass.The molecular mass was found to be twice the empirical formula unit molecular mass.What is the molecular formula of this gas?

(Multiple Choice)

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Question 27

Combustion analysis of an organic compound to determine the percentages of carbon, hydrogen, and oxygen in the compound depends on which of the following assumptions?

(Multiple Choice)

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Question 28

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

(Short Answer)

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Question 29

Cyanidin, a pigment found in many red berries, such as grapes, raspberries, and cranberries, contains carbon, hydrogen, and oxygen.The complete combustion of a 2.0000 g sample in excess O₂ produces 4.5964 g CO₂ and 0.6901 g H₂O.Mass spectrometry experiments showed that cyanidin's molecular mass is approximately 290 amu.What is the molecular formula of cyanidin?

(Short Answer)

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Question 30

If 98.0 g B₂O₃ (69.62 g/mol) and 125 g HF (20.01 g/mol) are combined and allowed to react according to the given equation, what mass of the excess reactant will be left over? B₂ O₃ (s) +6 HF(aq) $\rightarrow$ 2 BF3 (g) +3 H₂ O(l)

(Multiple Choice)

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Question 31

A compound known to contain platinum, nitrogen, and hydrogen was analyzed and found to contain 74.1% Pt and 21.3% N; the remainder was hydrogen.What is the empirical formula for the compound?

(Multiple Choice)

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Question 32

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

(Essay)

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Question 33

A burner in a gas grill mixes 20 volumes of air for every one volume of propane (C₃H₈).Is the mixture produced by this burner rich (excess propane), lean (excess oxygen), or just right (a stoichiometric mixture of propane and oxygen)? Assume that the volume of gas is directly proportional to the number of moles of gas and that air is 21% oxygen by volume.

(Essay)

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Question 34

How many moles of chlorine are in 25.0 g of calcium chloride (CaCl₂)?

(Multiple Choice)

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Question 35

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

(Short Answer)

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Question 36

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol) with 12.00 g water (18.02 g/mol).What was the percent yield for this reaction?

(Multiple Choice)

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Question 37

Hydrogen peroxide decomposes to produce water and oxygen.Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? 2H₂O₂ (l) $\rightarrow$ 2 H₂O(l) +O₂(g)

(Multiple Choice)

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Question 38

How many grams of iron(II, III) oxide (Fe₃O₄, 231.53 g/mol) must react in the presence of excess carbon monoxide (28.01 g/mol) if the theoretical yield of iron metal in the following reaction is 1.50 kg? Fe3O₄ (s) + 4 CO(g) $\rightarrow$ 3 Fe(s) +4 CO₂ (g)

(Multiple Choice)

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Question 39

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.

(Essay)

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Question 40

Showing 21 - 40 of 140

Caffeine has an elemental analysis of 49.48% C, 5.190% H, 16.47% O, and 28.85% N.It has a molar mass of 194.19 g/mol.What is the molecular formula of caffeine?

A sample of water (H₂O) contains 1.81 *10²⁴ molecules.How many moles of atoms are there in this sample?

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 10² g CO and 8.00 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

The average adult exhales about 1.0 kg of carbon dioxide each day.How much oxygen is needed in metabolizing glucose (C₆H₁₂O₆, 180.16 g/mol) to make that much carbon dioxide?

A gas that is produced when fruit ripens contains 85.62% C and 14.38% H by mass.The molecular mass was found to be twice the empirical formula unit molecular mass.What is the molecular formula of this gas?

Combustion analysis of an organic compound to determine the percentages of carbon, hydrogen, and oxygen in the compound depends on which of the following assumptions?

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

If 98.0 g B₂O₃ (69.62 g/mol) and 125 g HF (20.01 g/mol) are combined and allowed to react according to the given equation, what mass of the excess reactant will be left over? B₂ O₃ (s) +6 HF(aq) $\rightarrow$ 2 BF3 (g) +3 H₂ O(l)

A compound known to contain platinum, nitrogen, and hydrogen was analyzed and found to contain 74.1% Pt and 21.3% N; the remainder was hydrogen.What is the empirical formula for the compound?

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

How many moles of chlorine are in 25.0 g of calcium chloride (CaCl₂)?

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol) with 12.00 g water (18.02 g/mol).What was the percent yield for this reaction?

Hydrogen peroxide decomposes to produce water and oxygen.Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? 2H₂O₂ (l) $\rightarrow$ 2 H₂O(l) +O₂(g)

How many grams of iron(II, III) oxide (Fe₃O₄, 231.53 g/mol) must react in the presence of excess carbon monoxide (28.01 g/mol) if the theoretical yield of iron metal in the following reaction is 1.50 kg? Fe3O₄ (s) + 4 CO(g) $\rightarrow$ 3 Fe(s) +4 CO₂ (g)

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

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Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Caffeine has an elemental analysis of 49.48% C, 5.190% H, 16.47% O, and 28.85% N.It has a molar mass of 194.19 g/mol.What is the molecular formula of caffeine?

A sample of water (H2O) contains 1.81 *1024 molecules.How many moles of atoms are there in this sample?

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 *102 g CO and 8.00 * 102 g Fe2O3 were allowed to react? Fe 2 O3 (s) + 3 CO(g) →\rightarrow→ 2 Fe(s) + 3 CO2 (g)

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

The average adult exhales about 1.0 kg of carbon dioxide each day.How much oxygen is needed in metabolizing glucose (C6H12O6, 180.16 g/mol) to make that much carbon dioxide?

A gas that is produced when fruit ripens contains 85.62% C and 14.38% H by mass.The molecular mass was found to be twice the empirical formula unit molecular mass.What is the molecular formula of this gas?

Combustion analysis of an organic compound to determine the percentages of carbon, hydrogen, and oxygen in the compound depends on which of the following assumptions?

Calcium carbide (CaC2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C2H2, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)2, 74.10 g/mol).How many kilograms of C2H2 can be produced from 75.0 kg CaC2?

If 98.0 g B2O3 (69.62 g/mol) and 125 g HF (20.01 g/mol) are combined and allowed to react according to the given equation, what mass of the excess reactant will be left over? B2 O3 (s) +6 HF(aq) →\rightarrow→ 2 BF3 (g) +3 H2 O(l)

A compound known to contain platinum, nitrogen, and hydrogen was analyzed and found to contain 74.1% Pt and 21.3% N; the remainder was hydrogen.What is the empirical formula for the compound?

Give the empirical formula for each of the following compounds: H2O, H2O2, NH3, N2H4, C12H22O11, Al2Cl6.

How many moles of chlorine are in 25.0 g of calcium chloride (CaCl2)?

Traumatic acid, an organic acid with a molar mass of 228 g/mol, is composed of carbon, hydrogen, and oxygen.Analysis of a 10.000 g sample yielded 6.314 g C and 0.883 g H.What is its molecular formula?

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P4O10 (283.9 g/mol) with 12.00 g water (18.02 g/mol).What was the percent yield for this reaction?

Hydrogen peroxide decomposes to produce water and oxygen.Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? 2H2O2 (l) →\rightarrow→ 2 H2O(l) +O2(g)

How many grams of iron(II, III) oxide (Fe3O4, 231.53 g/mol) must react in the presence of excess carbon monoxide (28.01 g/mol) if the theoretical yield of iron metal in the following reaction is 1.50 kg? Fe3O4 (s) + 4 CO(g) →\rightarrow→ 3 Fe(s) +4 CO2 (g)

Write the balanced reaction equation for the combustion of dodecane (C12H26), which is found in kerosene.

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

A sample of water (H₂O) contains 1.81 *10²⁴ molecules.How many moles of atoms are there in this sample?

Carbon monoxide (28.01 g/mol) is used in refining iron(III) oxide 159.7 g/mol) to produce the metal.Assuming 100% yield, how many grams of Fe would be produced if 1.40 10² g CO and 8.00 10² g Fe₂O₃ were allowed to react? Fe₂O₃ (s) + 3 CO(g) $\rightarrow$ 2 Fe(s) + 3 CO₂ (g)

The average adult exhales about 1.0 kg of carbon dioxide each day.How much oxygen is needed in metabolizing glucose (C₆H₁₂O₆, 180.16 g/mol) to make that much carbon dioxide?

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

If 98.0 g B₂O₃ (69.62 g/mol) and 125 g HF (20.01 g/mol) are combined and allowed to react according to the given equation, what mass of the excess reactant will be left over? B₂ O₃ (s) +6 HF(aq) $\rightarrow$ 2 BF3 (g) +3 H₂ O(l)

Give the empirical formula for each of the following compounds: H₂O, H₂O₂, NH₃, N₂H₄, C₁₂H₂₂O₁₁, Al₂Cl₆.

How many moles of chlorine are in 25.0 g of calcium chloride (CaCl₂)?

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol) with 12.00 g water (18.02 g/mol).What was the percent yield for this reaction?

Hydrogen peroxide decomposes to produce water and oxygen.Which relationship regarding the quantities of reactants and products associated with this reaction is NOT correct? 2H₂O₂ (l) $\rightarrow$ 2 H₂O(l) +O₂(g)

How many grams of iron(II, III) oxide (Fe₃O₄, 231.53 g/mol) must react in the presence of excess carbon monoxide (28.01 g/mol) if the theoretical yield of iron metal in the following reaction is 1.50 kg? Fe3O₄ (s) + 4 CO(g) $\rightarrow$ 3 Fe(s) +4 CO₂ (g)

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.