Question 1

How many moles of iron are present in an iron cylinder that weighs 25 g?

Accepted Answer

The answer of How many moles of iron are present...

Question 2

The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound?

Accepted Answer

A) C10H6O 
B) C9H18O 
C) C16H28O4 
D) C20H12O2 
E) C18H36O2 
A) C10H6O 
B) C9H18O 
C) C16H28O4 
D) C20H12O2 
E) C18H36O2

Question 3

How many grams of sulfur are there in 6.0 g of Fe2(SO4)3?

Accepted Answer

A) 2.40 g 
B) 0.48 g 
C) 6.00 g 
D) 0.92 g 
E) 1.44 g 
A) 2.40 g 
B) 0.48 g 
C) 6.00 g 
D) 0.92 g 
E) 1.44 g

Question 4

How many atoms are in 5.54 g of F2?

Accepted Answer

A) 6.02 * 1023 atoms 
B) 0.146 atoms 
C) 0.292 atoms 
D) 8.78 * 1022 atoms 
E) 1.76 * 1023 atoms 
A) 6.02 * 1023 atoms 
B) 0.146 atoms 
C) 0.292 atoms 
D) 8.78 * 1022 atoms 
E) 1.76 * 1023 atoms

Question 5

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Accepted Answer

A) 90. g 
B) 36 g 
C) 42 g 
D) 45 g 
E) 108 g 
A) 90. g 
B) 36 g 
C) 42 g 
D) 45 g 
E) 108 g

Question 6

What is the theoretical yield of PI3 if 48.0 g of I2 are reacted with an excess of phosphorus according to the following chemical equation?
2P(s)+ 3I2(s) $\rarr$2PI3(s)

Accepted Answer

Question 7

Formaldehyde has the formula CH2O. How many molecules are there in 0.11 g of formaldehyde?

Accepted Answer

A) 6.1 * 10 -27 
B) 3.7 * 10 -3 
C) 4 
D) 2.2 * 1021 
E) 6.6 * 1022 
A) 6.1 * 10 -27 
B) 3.7 * 10 -3 
C) 4 
D) 2.2 * 1021 
E) 6.6 * 1022

Question 8

A chemistry student determined the empirical formula for tungsten oxide (WxOy). To do so, he heated tungsten with oxygen in a crucible. The data that he recorded are shown below:
Weight of crucible 11.120 g
Weight of tungsten 8.820 g
Weight of crucible and product 22.998 g
What is the empirical formula of tungsten oxide?

Accepted Answer

Question 9

Solid sodium hydrogen carbonate (also known as sodium bicarbonate)can be decomposed to form solid sodium carbonate, gaseous carbon dioxide, and water vapor. When the balanced chemical reaction for this process is written such that the coefficient of water is 1, what is the coefficient of carbon dioxide?

Accepted Answer

A) 0 
B) 1 
C) 2 
D)    
E) cannot be determined 
A) 0 
B) 1 
C) 2 
D)    
E) cannot be determined

Question 10

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Do not forget to count coefficients of one. The sum of the coefficients is __ SF4 + __ H2O $\rarr$ __ H2SO3 + __ HF

Accepted Answer

A) 4. 
B) 6. 
C) 7. 
D) 9. 
E) none of these. 
A) 4. 
B) 6. 
C) 7. 
D) 9. 
E) none of these.

Question 11

How many sodium atoms are there in 6.0 g of Na3N?

Accepted Answer

A) 3.6 * 1024 atoms 
B) 4.6 * 1022 atoms 
C) 1.3 * 1023 atoms 
D) 0.217 atoms 
E) 0.072 atoms 
A) 3.6 * 1024 atoms 
B) 4.6 * 1022 atoms 
C) 1.3 * 1023 atoms 
D) 0.217 atoms 
E) 0.072 atoms

Question 12

Calculate the mass of 3.7 moles of Br2.

Accepted Answer

Question 13

What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers?
 ___ Na + ___ H2O $\rarr$ ___ NaOH + ___ H2

Accepted Answer

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

Question 14

What is the coefficient of H2O when the following equation is properly balanced with smallest set of whole numbers? 
___ Al4C3 + ___ H2O $\rarr$ ___ Al(OH)3 + ___ CH4

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 12 
E) 24 
A) 3 
B) 4 
C) 6 
D) 12 
E) 24

Question 15

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr2O3 $\rarr$Al2O3 + 2Cr

Accepted Answer

A) 7.7 g 
B) 15.4 g 
C) 27.3 g 
D) 30.8 g 
E) 49.9 g 
A) 7.7 g 
B) 15.4 g 
C) 27.3 g 
D) 30.8 g 
E) 49.9 g

Question 16

Calculate the molecular mass, in g/mol, of P4O10.

Accepted Answer

Question 17

What percent by mass of oxygen is present in carbon monoxide, CO?

Accepted Answer

The answer of What percent by mass of oxygen is...

Question 18

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper?
Cu + 2 AgNO3 $\rarr$ Cu(NO3 )2 + 2 Ag

Accepted Answer

Question 19

What mass of sodium nitrate would be produced from the complete reaction of 1.00 mol of lead nitrate?
2 NaCl + Pb(NO3 )2 $\rarr$ 2 NaNO3 + PbCl2

Accepted Answer

Question 20

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm3)

Accepted Answer

A) 0.178 m 
B) 0.567 m 
C) 180 m 
D) 45.1 m 
E) 2.27 m 
A) 0.178 m 
B) 0.567 m 
C) 180 m 
D) 45.1 m 
E) 2.27 m

How many moles of iron are present in an iron cylinder that weighs 25 g?

The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound?

How many grams of sulfur are there in 6.0 g of Fe₂(SO₄)₃?

How many atoms are in 5.54 g of F₂?

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

What is the theoretical yield of PI₃ if 48.0 g of I₂ are reacted with an excess of phosphorus according to the following chemical equation? 2P(s)+ 3I₂(s) $\rarr$ 2PI₃(s)

Formaldehyde has the formula CH₂O. How many molecules are there in 0.11 g of formaldehyde?

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Do not forget to count coefficients of one. The sum of the coefficients is SF₄ + H₂O $\rarr$ H₂SO₃ + HF

How many sodium atoms are there in 6.0 g of Na₃N?

Calculate the mass of 3.7 moles of Br₂.

What is the coefficient of H₂O when the following equation is properly balanced with the smallest set of whole numbers? _ Na + _ H₂O $\rarr$ _ NaOH + _ H₂

What is the coefficient of H₂O when the following equation is properly balanced with smallest set of whole numbers? _ Al₄C₃ + _ H₂O $\rarr$ _ Al(OH)₃ + _ CH₄

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr₂O₃ with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr₂O₃ $\rarr$ Al₂O₃ + 2Cr

Calculate the molecular mass, in g/mol, of P₄O₁₀.

What percent by mass of oxygen is present in carbon monoxide, CO?

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper? Cu + 2 AgNO₃ $\rarr$ Cu(NO₃)₂ + 2 Ag

What mass of sodium nitrate would be produced from the complete reaction of 1.00 mol of lead nitrate? 2 NaCl + Pb(NO₃)₂ $\rarr$ 2 NaNO₃ + PbCl₂

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm³)

Introduction

Atoms, Molecules, and Ions

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 3: Stoichiometry

How many moles of iron are present in an iron cylinder that weighs 25 g?

The percent composition by mass of a compound is 76.0% C, 12.8% H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula of the compound?

How many grams of sulfur are there in 6.0 g of Fe2(SO4)3?

How many atoms are in 5.54 g of F2?

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

What is the theoretical yield of PI3 if 48.0 g of I2 are reacted with an excess of phosphorus according to the following chemical equation? 2P(s)+ 3I2(s) →\rarr→ 2PI3(s)

Formaldehyde has the formula CH2O. How many molecules are there in 0.11 g of formaldehyde?

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Do not forget to count coefficients of one. The sum of the coefficients is __ SF4 + __ H2O →\rarr→ __ H2SO3 + __ HF

How many sodium atoms are there in 6.0 g of Na3N?

Calculate the mass of 3.7 moles of Br2.

What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers? ___ Na + ___ H2O →\rarr→ ___ NaOH + ___ H2

What is the coefficient of H2O when the following equation is properly balanced with smallest set of whole numbers? ___ Al4C3 + ___ H2O →\rarr→ ___ Al(OH)3 + ___ CH4

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr2O3 →\rarr→ Al2O3 + 2Cr

Calculate the molecular mass, in g/mol, of P4O10.

What percent by mass of oxygen is present in carbon monoxide, CO?

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper? Cu + 2 AgNO3 →\rarr→ Cu(NO3 )2 + 2 Ag

What mass of sodium nitrate would be produced from the complete reaction of 1.00 mol of lead nitrate? 2 NaCl + Pb(NO3 )2 →\rarr→ 2 NaNO3 + PbCl2

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm3)

Introduction

Atoms, Molecules, and Ions

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

How many grams of sulfur are there in 6.0 g of Fe₂(SO₄)₃?

How many atoms are in 5.54 g of F₂?

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

What is the theoretical yield of PI₃ if 48.0 g of I₂ are reacted with an excess of phosphorus according to the following chemical equation? 2P(s)+ 3I₂(s) $\rarr$ 2PI₃(s)

Formaldehyde has the formula CH₂O. How many molecules are there in 0.11 g of formaldehyde?

Balance the following equation using the smallest set of whole numbers, then add together the coefficients. Do not forget to count coefficients of one. The sum of the coefficients is SF₄ + H₂O $\rarr$ H₂SO₃ + HF

How many sodium atoms are there in 6.0 g of Na₃N?

Calculate the mass of 3.7 moles of Br₂.

What is the coefficient of H₂O when the following equation is properly balanced with the smallest set of whole numbers? _ Na + _ H₂O $\rarr$ _ NaOH + _ H₂

What is the coefficient of H₂O when the following equation is properly balanced with smallest set of whole numbers? _ Al₄C₃ + _ H₂O $\rarr$ _ Al(OH)₃ + _ CH₄

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr₂O₃ with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr₂O₃ $\rarr$ Al₂O₃ + 2Cr

Calculate the molecular mass, in g/mol, of P₄O₁₀.

How many grams of silver nitrate are necessary to react completely with 7.000 moles of copper? Cu + 2 AgNO₃ $\rarr$ Cu(NO₃)₂ + 2 Ag

What mass of sodium nitrate would be produced from the complete reaction of 1.00 mol of lead nitrate? 2 NaCl + Pb(NO₃)₂ $\rarr$ 2 NaNO₃ + PbCl₂

A copper wire has a diameter of 2.00 mm. What length of this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm³)