Question 1

What is the molar mass of NH4)3PO4?

Accepted Answer

A)  113 g 
B)  121 g 
C)  149 g 
A)  113 g 
B)  121 g 
C)  149 g

Question 2

What is the mass in grams of 6.022 x 1023 molecules of CO2?

Accepted Answer

A)  22 g 
B)  44 g 
C)  66 g 
A)  22 g 
B)  44 g 
C)  66 g

Question 3

Commercial grade fuming nitric acid contains about 90% HNO3 by mass with a density of 1.50 g/mL, calculate the molarity of the HNO3 solution.

Accepted Answer

A)  0.214 M 
B)  21.4 M 
C)  2.14 M 
A)  0.214 M 
B)  21.4 M 
C)  2.14 M

Question 4

What is the total number of atoms contained in 1.00 mole of sodium?

Accepted Answer

A)  118 
B)  6.02 x 1023 
C)  1.2 x 1024 
A)  118 
B)  6.02 x 1023 
C)  1.2 x 1024

Question 5

What are the proper units for molar mass in chemistry?

Accepted Answer

A)  amu 
B)  g/mol 
C)  g/mmol 
A)  amu 
B)  g/mol 
C)  g/mmol

Question 6

A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO2 and 5.40 g of H2O are produced. What is the empirical formula of the unknown?

Accepted Answer

A)  CH3 
B)  CH 
C)  CH2 
A)  CH3 
B)  CH 
C)  CH2

Question 7

What is the mass in grams of 0.852 moles of ferric oxide?  Paired item 1)

Accepted Answer

A)  5.34 x 10-3 g 
B)  187 g 
C)  136 g 
A)  5.34 x 10-3 g 
B)  187 g 
C)  136 g

What is the molar mass of NH₄)₃PO₄?

What is the mass in grams of 6.022 x 10²³ molecules of CO₂?

Commercial grade fuming nitric acid contains about 90% HNO₃ by mass with a density of 1.50 g/mL, calculate the molarity of the HNO₃ solution.

What is the total number of atoms contained in 1.00 mole of sodium?

What are the proper units for molar mass in chemistry?

A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO₂ and 5.40 g of H₂O are produced. What is the empirical formula of the unknown?

What is the mass in grams of 0.852 moles of ferric oxide? Paired item 1)

Essential Ideas

Atoms, Molecules, and Ions

Stoichiometry of Chemical Reactions

Thermochemistry

Electronic Structure and Periodic Properties of Elements

Chemical Bonding and Molecular Geometry

Advanced Theories of Covalent Bonding

Gases

Liquids and Solids

Solutions and Colloids

Kinetics

Fundamental Equilibrium Concepts

Acid-Base Equilibria

Thermodynamics

Electrochemistry

Representative Metals, Metalloids, and Nonmetals

Organic Chemistry

Nuclear Chemistry

Filters

Exam 3: Composition of Substances and Solutions

What is the molar mass of NH4)3PO4?

What is the mass in grams of 6.022 x 1023 molecules of CO2?

Commercial grade fuming nitric acid contains about 90% HNO3 by mass with a density of 1.50 g/mL, calculate the molarity of the HNO3 solution.

What is the total number of atoms contained in 1.00 mole of sodium?

What are the proper units for molar mass in chemistry?

A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO2 and 5.40 g of H2O are produced. What is the empirical formula of the unknown?

What is the mass in grams of 0.852 moles of ferric oxide? Paired item 1)

Essential Ideas

Atoms, Molecules, and Ions

Stoichiometry of Chemical Reactions

Thermochemistry

Electronic Structure and Periodic Properties of Elements

Chemical Bonding and Molecular Geometry

Advanced Theories of Covalent Bonding

Gases

Liquids and Solids

Solutions and Colloids

Kinetics

Fundamental Equilibrium Concepts

Acid-Base Equilibria

Thermodynamics

Electrochemistry

Representative Metals, Metalloids, and Nonmetals

Organic Chemistry

Nuclear Chemistry

Filters

What is the molar mass of NH₄)₃PO₄?

What is the mass in grams of 6.022 x 10²³ molecules of CO₂?

Commercial grade fuming nitric acid contains about 90% HNO₃ by mass with a density of 1.50 g/mL, calculate the molarity of the HNO₃ solution.

A 3.00 g sample of unknown hydrocarbon is prepared for combustion analysis. After the hydrocarbon undergoes complete combustion, 8.80 g of CO₂ and 5.40 g of H₂O are produced. What is the empirical formula of the unknown?