Question 1

The formula weight of ammonium carbonate, (NH4)2CO3,is ________ amu.

Accepted Answer

A) 64.11 
B) 82.10 
C) 96.09 
D) 120.13 
E) 180.17 
A) 64.11 
B) 82.10 
C) 96.09 
D) 120.13 
E) 180.17

Question 2

Calculate the number of moles of aspirin,C9H8O4,in a 4.0 gram tablet.

Accepted Answer

A) 2.2 × 10-4 
B) 2.2 
C) 4.6 × 10-3 
D) 0.022 
A) 2.2 × 10-4 
B) 2.2 
C) 4.6 × 10-3 
D) 0.022

Question 3

The formula weight of Al2(SO4)3 is ________ grams.

Accepted Answer

A) 214.14 
B) 278.02 
C) 315.14 
D) 342.14 
E) 450.14 
A) 214.14 
B) 278.02 
C) 315.14 
D) 342.14 
E) 450.14

Question 4

How many molecules are there in 3.00 moles of NH3?

Accepted Answer

A) 1.00 
B) 3.00 
C) 17.00 
D) 1.20 × 1024 
E) 1.81 × 1024 
A) 1.00 
B) 3.00 
C) 17.00 
D) 1.20 × 1024 
E) 1.81 × 1024

Question 5

The reaction N2 + 3 H2 → 2 NH3 is used to produce ammonia.When 450.g of hydrogen was reacted with nitrogen,1575 g of ammonia were produced.What is the percent yield of this reaction?

Accepted Answer

A) 62.1% 
B) 41.5% 
C) 30.8% 
D) 20.7% 
E) More information is needed to solve this problem. 
A) 62.1% 
B) 41.5% 
C) 30.8% 
D) 20.7% 
E) More information is needed to solve this problem.

Question 6

Match the following.
-The molar mass of BaCI2

Accepted Answer

A) 208.2 g 
B) 212.4 g 
C) 219 g 
D) 225 g 
A) 208.2 g 
B) 212.4 g 
C) 219 g 
D) 225 g

Question 7

A thimble of water contains 4.0 × 1021 molecules.The number of moles of H2O is:

Accepted Answer

A) 2.4 × 1045 
B) 6.6 × 10-3 
C) 6.6 × 10-23 
D) 2.4 × 1023 
E) 2.4 × 10-23 
A) 2.4 × 1045 
B) 6.6 × 10-3 
C) 6.6 × 10-23 
D) 2.4 × 1023 
E) 2.4 × 10-23

Question 8

How much Ca(NO3)2 should be weighed out to have 0.650 mol?

Accepted Answer

A) 66.4 g 
B) 97.6 g 
C) 107 g 
D) 133 g 
E) 165 g 
A) 66.4 g 
B) 97.6 g 
C) 107 g 
D) 133 g 
E) 165 g

Question 9

Match the following.
-The mass of 2.25 moles of CaCO3

Accepted Answer

A) 208.2 g 
B) 212.4 g 
C) 219 g 
D) 225 g 
A) 208.2 g 
B) 212.4 g 
C) 219 g 
D) 225 g

Question 10

Which statement concerning the mole concept is not true?

Accepted Answer

A) The molar mass of a metal is its atomic weight expressed in grams. 
B) The mole concept makes a connection between the mass of a substance and the number of particles or units of that substance. 
C) One mole of any compound contains one mole of atoms. 
D) One mole of sodium contains the same number of atoms as one mole of carbon. 
E) One mole of water contains the same number of molecules as one mole of ammonia. 
A) The molar mass of a metal is its atomic weight expressed in grams. 
B) The mole concept makes a connection between the mass of a substance and the number of particles or units of that substance. 
C) One mole of any compound contains one mole of atoms. 
D) One mole of sodium contains the same number of atoms as one mole of carbon. 
E) One mole of water contains the same number of molecules as one mole of ammonia.

Question 11

Given the following balanced equation,answer the following:
C2H5OH + 3 O2 → 2 CO2 + 3 H2O
a)What is the theoretical yield of carbon dioxide in this reaction if 39.6 g of ethanol is burned in the presence of 54.8 g of oxygen?
b)What is the percent yield for this reaction if the actual amount of carbon dioxide formed is 45.5 grams?

Accepted Answer

a)This is a limiting reagent problem.Fir

Question 12

The balanced equation given below means:
CH4 + 2 O2 → CO2 + 2H2O

Accepted Answer

A) One mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and 2 moles of water. 
B) One gram of methane reacts with two grams of oxygen to produce one gram of carbon dioxide and two grams of water. 
C) One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water. 
D) A,B and C are correct. 
E) A and C are correct. 
A) One mole of methane reacts with two moles of oxygen to produce one mole of carbon dioxide and 2 moles of water. 
B) One gram of methane reacts with two grams of oxygen to produce one gram of carbon dioxide and two grams of water. 
C) One molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water. 
D) A,B and C are correct. 
E) A and C are correct.

Question 13

The number of grams in 7.00 moles of N2 is ________.

Accepted Answer

A) 7 × (6.02 × 1023) 
B) 14.0 
C) 28.0 
D) 98.0 
E) 196 
A) 7 × (6.02 × 1023) 
B) 14.0 
C) 28.0 
D) 98.0 
E) 196

Question 14

In the reaction shown,what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C4H10?
2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

Accepted Answer

A) 
  
B) 
  
C) 
  
D) 
  
E) 
  
A) 
  
B) 
  
C) 
  
D) 
  
E)

Question 15

Which quantity contains Avogadro's number of molecules?

Accepted Answer

A) 8.8 g CO2 
B) 34 g of NH3 
C) 9 g of H2O 
D) 98 g of H2SO4 
A) 8.8 g CO2 
B) 34 g of NH3 
C) 9 g of H2O 
D) 98 g of H2SO4

Question 16

How many molecules are present in 1.36 g of AgNO3?

Accepted Answer

A) 3.84 × 10-22 
B) 4.82 × 1021 
C) 1.36 × 1023 
D) 7.52 × 1025 
A) 3.84 × 10-22 
B) 4.82 × 1021 
C) 1.36 × 1023 
D) 7.52 × 1025

Question 17

Interpret in words the equation:
P4O10 (s)+ 6 H2O (l)→ 4 H3PO4 (aq)

Accepted Answer

A) One mole of solid tetraphosphorus decaoxide reacts with six moles of liquid water to produce four moles of phosphoric acid solution. 
B) Zero moles of solid phosphoric oxide dissolve in six moles of water to produce four moles of phosphorous acid. 
C) One mole of phosphorus(X)oxide combines with six moles of water to produce four moles of solution of hydrogen phosphate. 
D) Four moles of solid phosphorus,five moles of diatomic oxygen gas,and six moles of liquid water react together to produce four moles of phosphoric acid in solution. 
E) Four atoms of phosphorus,16 atoms of oxygen,and 12 atoms of hydrogen rearrange to produce four molecules of phosphoric acid. 
A) One mole of solid tetraphosphorus decaoxide reacts with six moles of liquid water to produce four moles of phosphoric acid solution. 
B) Zero moles of solid phosphoric oxide dissolve in six moles of water to produce four moles of phosphorous acid. 
C) One mole of phosphorus(X)oxide combines with six moles of water to produce four moles of solution of hydrogen phosphate. 
D) Four moles of solid phosphorus,five moles of diatomic oxygen gas,and six moles of liquid water react together to produce four moles of phosphoric acid in solution. 
E) Four atoms of phosphorus,16 atoms of oxygen,and 12 atoms of hydrogen rearrange to produce four molecules of phosphoric acid.

Question 18

The number of grams in 2.65 mol of SO2 is

Accepted Answer

A) 2.65. 
B) 64.1. 
C) 24.2. 
D) 170. 
E) 1.60 × 1024. 
A) 2.65. 
B) 64.1. 
C) 24.2. 
D) 170. 
E) 1.60 × 1024.

Question 19

In the reaction shown,how many moles of HCl are needed to react with 2.4 moles of Al?
2 Al + 6 HCl → 2 AlCl3  + 3 H2

Accepted Answer

A) 0.8 
B) 1.3 
C) 4.8 
D) 6.4 
E) 7.2 
A) 0.8 
B) 1.3 
C) 4.8 
D) 6.4 
E) 7.2

Question 20

How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown?
2 Fe + 3F2 → 2 FeF3

Accepted Answer

A) 4.49 g 
B) 5.05 g 
C) 6.74 g 
D) 10.1 g 
E) 20.2 g 
A) 4.49 g 
B) 5.05 g 
C) 6.74 g 
D) 10.1 g 
E) 20.2 g

Exam 6: Chemical Reactions: Mole and Mass Relationships

The formula weight of ammonium carbonate, (NH4)2CO3,is ________ amu.

Calculate the number of moles of aspirin,C9H8O4,in a 4.0 gram tablet.

The formula weight of Al2(SO4)3 is ________ grams.

How many molecules are there in 3.00 moles of NH3?

The reaction N2 + 3 H2 → 2 NH3 is used to produce ammonia.When 450.g of hydrogen was reacted with nitrogen,1575 g of ammonia were produced.What is the percent yield of this reaction?

Match the following. -The molar mass of BaCI2

A thimble of water contains 4.0 × 1021 molecules.The number of moles of H2O is:

How much Ca(NO3)2 should be weighed out to have 0.650 mol?

Match the following. -The mass of 2.25 moles of CaCO3

Which statement concerning the mole concept is not true?

The balanced equation given below means: CH4 + 2 O2 → CO2 + 2H2O

The number of grams in 7.00 moles of N2 is ________.

In the reaction shown,what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C4H10? 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O

Which quantity contains Avogadro's number of molecules?

How many molecules are present in 1.36 g of AgNO3?

Interpret in words the equation: P4O10 (s)+ 6 H2O (l)→ 4 H3PO4 (aq)

The number of grams in 2.65 mol of SO2 is

In the reaction shown,how many moles of HCl are needed to react with 2.4 moles of Al? 2 Al + 6 HCl → 2 AlCl3 + 3 H2

How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown? 2 Fe + 3F2 → 2 FeF3

Matter and Measurements

Atoms and the Periodic Table

Ionic Compounds

Molecular Compounds

Classification and Balancing of Chemical Reactions

Chemical Reactions: Energy, rates, and Equilibrium

Gases, liquids, and Solids

Solutions

Acids and Bases

Nuclear Chemistry

Introduction to Organic Chemistry: Alkanes

Alkenes, alkynes, and Aromatic Compounds

Some Compounds With Oxygen, sulfur, or a Halogen

Amines

Aldehydes and Ketones

Carboxylic Acids and Their Derivatives

Amino Acids and Proteins

Enzymes and Vitamins

The Generation of Biochemical Energy

Carbohydrates

Carbohydrate Metabolism

Lipids

Lipid Metabolism

Nucleic Acids and Protein Synthesis

Genomics

Protein and Amino Acid Metabolism

Chemical Messengers: Hormones, neurotransmitters, and Drugs

Body Fluids

Filters

The formula weight of ammonium carbonate, (NH₄)₂CO₃,is ________ amu.

Calculate the number of moles of aspirin,C₉H₈O₄,in a 4.0 gram tablet.

The formula weight of Al₂(SO₄)₃ is ________ grams.

How many molecules are there in 3.00 moles of NH₃?

The reaction N₂ + 3 H₂ → 2 NH₃ is used to produce ammonia.When 450.g of hydrogen was reacted with nitrogen,1575 g of ammonia were produced.What is the percent yield of this reaction?

Match the following. -The molar mass of BaCI₂

A thimble of water contains 4.0 × 10²¹ molecules.The number of moles of H₂O is:

How much Ca(NO₃)₂ should be weighed out to have 0.650 mol?

Match the following. -The mass of 2.25 moles of CaCO₃

The balanced equation given below means: CH₄ + 2 O₂ → CO₂ + 2H₂O

The number of grams in 7.00 moles of N₂ is ________.

In the reaction shown,what is the mole ratio that would be used to determine the number of moles of oxygen needed to react with 3.2 moles of C₄H₁₀? 2 C₄H₁₀ + 13 O₂ → 8 CO₂ + 10 H₂O

How many molecules are present in 1.36 g of AgNO₃?

Interpret in words the equation: P₄O₁₀ (s)+ 6 H₂O (l)→ 4 H₃PO₄ (aq)

The number of grams in 2.65 mol of SO₂ is

In the reaction shown,how many moles of HCl are needed to react with 2.4 moles of Al? 2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

How many grams of fluorine are required to produce 20.0 grams of FeF₃ from the reaction shown? 2 Fe + 3F₂ → 2 FeF₃