Question 1

Calculate the molar mass of molecular iodine.

Accepted Answer

A) 126.9 g/mol 
B) 253.8 g/mol 
C) 79.9 g/mol 
D) 159.8 g/mol 
E) Only atomic masses, and not molar masses, can be calculated for elements 
A) 126.9 g/mol 
B) 253.8 g/mol 
C) 79.9 g/mol 
D) 159.8 g/mol 
E) Only atomic masses, and not molar masses, can be calculated for elements

Question 2

From the following,pick those that are empirical formulas.
i.KCl
ii.K2S2O8
iii.K2SO4
iv.K4S2
v.KIO3

Accepted Answer

A) i and v 
B) ii and iv 
C) iii and iv 
D) iv and v 
E) i, iii, and v 
A) i and v 
B) ii and iv 
C) iii and iv 
D) iv and v 
E) i, iii, and v

Question 3

Calculate the percent mercury and nitrogen in mercury(II)cyanide.The formula of the cyanide ion is CN-.

Accepted Answer

A) 20.0% Hg, 40.0% N 
B) 79.4% Hg, 6.2% N 
C) 79.4% Hg, 11.1% N 
D) 83.4% Hg, 11.6% N 
E) 88.5% Hg, 6.2% N 
A) 20.0% Hg, 40.0% N 
B) 79.4% Hg, 6.2% N 
C) 79.4% Hg, 11.1% N 
D) 83.4% Hg, 11.6% N 
E) 88.5% Hg, 6.2% N

Question 4

What is the mass of 7.24 × 1023 formula units of barium oxide?

Accepted Answer

A) 7.85 × 10-3 g 
B) 1.84 × 102 g 
C) 1.11 × 1026 g 
D) 2.84 × 1045 g 
E) 6.68 × 1049 g 
A) 7.85 × 10-3 g 
B) 1.84 × 102 g 
C) 1.11 × 1026 g 
D) 2.84 × 1045 g 
E) 6.68 × 1049 g

Question 5

Calculate the percent composition of aluminum oxide.

Accepted Answer

A) 47.1% Al, 52.9% O 
B) 52.9% Al, 47.1% O 
C) 28.3% Al, 71.7% O 
D) 71.1% Al, 28.3% O 
E) 62.8% Al, 37.2% O 
A) 47.1% Al, 52.9% O 
B) 52.9% Al, 47.1% O 
C) 28.3% Al, 71.7% O 
D) 71.1% Al, 28.3% O 
E) 62.8% Al, 37.2% O

Question 6

What is the mass of 0.0490 mole of potassium sulfate?

Accepted Answer

A) 0.0490 g 
B) 3.55 kg 
C) 6.62 g 
D) 8.54 g 
E) 174.3 g 
A) 0.0490 g 
B) 3.55 kg 
C) 6.62 g 
D) 8.54 g 
E) 174.3 g

Question 7

A compound analyzes as 18.0% carbon,2.26% hydrogen,and 79.7% chlorine.Calculate the empirical formula of the compound.

Accepted Answer

A) C4H3Cl4 
B) C3H2Cl2 
C) C3H3Cl2 
D) C2H2Cl3 
E) C2H3Cl3 
A) C4H3Cl4 
B) C3H2Cl2 
C) C3H3Cl2 
D) C2H2Cl3 
E) C2H3Cl3

Question 8

How many grams of calcium are in 5.00 g of calcium hydroxide?

Accepted Answer

A) 0.541 g 
B) 2.50 g 
C) 2.70 g 
D) 3.51 g 
E) 40.1 g 
A) 0.541 g 
B) 2.50 g 
C) 2.70 g 
D) 3.51 g 
E) 40.1 g

Question 9

How much silver nitrate must be measured to yield 1.00 g silver?

Accepted Answer

A) 1.00 g 
B) 1.57 g 
C) 1.70 g 
D) 2.00 g 
E) 0.635 g 
A) 1.00 g 
B) 1.57 g 
C) 1.70 g 
D) 2.00 g 
E) 0.635 g

Question 10

Calculate the number of atoms in 0.377 grams of Ar.

Accepted Answer

A) 1.57 × 10-26 
B) 2.50 × 10-23 
C) 5.67 × 1021 
D) 9.08 × 1024 
E) 9.42 × 10-3 
A) 1.57 × 10-26 
B) 2.50 × 10-23 
C) 5.67 × 1021 
D) 9.08 × 1024 
E) 9.42 × 10-3

Question 11

Calculate the percentage composition of calcium chlorate.

Accepted Answer

A) 19.4% Ca, 34. 3% Cl, 46.4% O 
B) 32.4% Ca, 28.7% Cl, 38.8% O 
C) 49.0% Ca, 21.8% Cl, 29.3% O 
D) 32.4% Ca, 67.6% ClO3 
E) 49.0% Ca, 51.0% ClO3 
A) 19.4% Ca, 34. 3% Cl, 46.4% O 
B) 32.4% Ca, 28.7% Cl, 38.8% O 
C) 49.0% Ca, 21.8% Cl, 29.3% O 
D) 32.4% Ca, 67.6% ClO3 
E) 49.0% Ca, 51.0% ClO3

Question 12

Which of the following statements is/are incorrect?

Accepted Answer

A) One mole is that amount of any substance that contains the same number of units as the number of atoms in exactly 12 grams of carbon-12 
B) To three significant figures, there are 6.02 × 1023 units per mole 
C) The number of particles in a mole is called Avogadro's number 
D) The mass of 1/12 mole of carbon-12 is 1 gram 
E) The mole is a fundamental constant derived from the laws of nature 
A) One mole is that amount of any substance that contains the same number of units as the number of atoms in exactly 12 grams of carbon-12 
B) To three significant figures, there are 6.02 × 1023 units per mole 
C) The number of particles in a mole is called Avogadro's number 
D) The mass of 1/12 mole of carbon-12 is 1 gram 
E) The mole is a fundamental constant derived from the laws of nature

Question 13

Calculate the mass of silver in a sample of silver sulfide that contains 0.890 g of sulfur.

Accepted Answer

A) 1.08 g 
B) 1.78 g 
C) 3.00 g 
D) 5.99 g 
E) 6.89 g 
A) 1.08 g 
B) 1.78 g 
C) 3.00 g 
D) 5.99 g 
E) 6.89 g

Question 14

Calculate the formula mass of aluminum carbonate.

Accepted Answer

A) 87.0 u 
B) 114.0 u 
C) 147.0 u 
D) 201.0 u 
E) 234.0 u 
A) 87.0 u 
B) 114.0 u 
C) 147.0 u 
D) 201.0 u 
E) 234.0 u

Question 15

Determine the molecular formula of a compound that has a molar mass of 264 g/mol and the empirical formula C3H4O3.

Accepted Answer

A) CHO 
B) CH1.33O 
C) C9H12O9 
D) C6H8O6 
E) C3H4O3 
A) CHO 
B) CH1.33O 
C) C9H12O9 
D) C6H8O6 
E) C3H4O3

Question 16

Which of the following statements is/are correct?
i.One mole of a substance contains as many particles as exactly 12 u of carbon-12
ii.A mole of iodine atoms contains fewer atoms than a mole of bromine atoms
iii.There are 6.02 × 1023 carbon atoms in 12.0 grams of carbon-12
iv.Because both use carbon-12 as a reference,one mole of a low molecular mass substance contains more particles than one mole of a high molecular mass substance
v.One mole of a substance contains 6.02 × 1023 particles of that substance

Accepted Answer

A) i and iii 
B) i and v 
C) iii and v 
D) ii and iv 
E) ii and v 
A) i and iii 
B) i and v 
C) iii and v 
D) ii and iv 
E) ii and v

Question 17

A compound is composed of 74.0% C,8.70% H,and 17.3% N.Its molar mass is 162 g/mol.What is its molecular formula?

Accepted Answer

A) C9H12N3 
B) C74H9N17 
C) C6H8N 
D) C5H7N 
E) C10H14N2 
A) C9H12N3 
B) C74H9N17 
C) C6H8N 
D) C5H7N 
E) C10H14N2

Question 18

What is the empirical formula of a compound that contains 80.0% carbon and 20.0% hydrogen by mass?

Accepted Answer

A) CH3 
B) CH2 
C) CH 
D) C3H 
E) C2H3 
A) CH3 
B) CH2 
C) CH 
D) C3H 
E) C2H3

Question 19

Which of the following are empirical formulas?
i.C10H8
ii.CH2
iii.Al2Cl6
iv.NO2
v.Hg2Cl2

Accepted Answer

A) i only 
B) i and ii 
C) ii and iv 
D) i, ii, and v 
E) iii, iv, and v 
A) i only 
B) i and ii 
C) ii and iv 
D) i, ii, and v 
E) iii, iv, and v

Question 20

Which of the following statements is incorrect?

Accepted Answer

A) Molecular mass is expressed in atomic mass units 
B) Formula mass compares the mass of one formula unit of a substance to the mass of one atom of carbon-12 
C) Atomic mass has units of grams per atom 
D) Both molecular mass and formula mass use carbon-12 as a reference standard 
E) Sodium chloride, an ionic compound, is said to have a formula weight, but not a molecular weight 
A) Molecular mass is expressed in atomic mass units 
B) Formula mass compares the mass of one formula unit of a substance to the mass of one atom of carbon-12 
C) Atomic mass has units of grams per atom 
D) Both molecular mass and formula mass use carbon-12 as a reference standard 
E) Sodium chloride, an ionic compound, is said to have a formula weight, but not a molecular weight

Calculate the molar mass of molecular iodine.

From the following,pick those that are empirical formulas. i.KCl ii.K₂S₂O₈ iii.K₂SO₄ iv.K₄S₂ v.KIO₃

Calculate the percent mercury and nitrogen in mercury(II)cyanide.The formula of the cyanide ion is CN^-.

What is the mass of 7.24 × 10²³ formula units of barium oxide?

Calculate the percent composition of aluminum oxide.

What is the mass of 0.0490 mole of potassium sulfate?

A compound analyzes as 18.0% carbon,2.26% hydrogen,and 79.7% chlorine.Calculate the empirical formula of the compound.

How many grams of calcium are in 5.00 g of calcium hydroxide?

How much silver nitrate must be measured to yield 1.00 g silver?

Calculate the number of atoms in 0.377 grams of Ar.

Calculate the percentage composition of calcium chlorate.

Which of the following statements is/are incorrect?

Calculate the mass of silver in a sample of silver sulfide that contains 0.890 g of sulfur.

Calculate the formula mass of aluminum carbonate.

Determine the molecular formula of a compound that has a molar mass of 264 g/mol and the empirical formula C₃H₄O₃.

A compound is composed of 74.0% C,8.70% H,and 17.3% N.Its molar mass is 162 g/mol.What is its molecular formula?

What is the empirical formula of a compound that contains 80.0% carbon and 20.0% hydrogen by mass?

Which of the following are empirical formulas? i.C₁₀H₈ ii.CH₂ iii.Al₂Cl₆ iv.NO₂ v.Hg₂Cl₂

Which of the following statements is incorrect?

Matter and Energy

Measurement and Chemical Calculations

Introduction to Gases

Atomic Theory: The Nuclear Model of the Atom

Chemical Nomenclature

Chemical Reactions

Chemical Change

Quantity Relationships in Chemical Reactions

Atomic Theory: The Quantum Model of the Atom

Chemical Bonding

Structure and Shape

The Ideal Gas Law and Its Applications

Gases, Liquids, and Solids

Solutions

Acidbase Proton Transferreactions

Chemical Equilibrium

Oxidationreduction Electron Transferreactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

Exam 7: Chemical Formula Relationships

Calculate the molar mass of molecular iodine.

From the following,pick those that are empirical formulas. i.KCl ii.K2S2O8 iii.K2SO4 iv.K4S2 v.KIO3

Calculate the percent mercury and nitrogen in mercury(II)cyanide.The formula of the cyanide ion is CN-.

What is the mass of 7.24 × 1023 formula units of barium oxide?

Calculate the percent composition of aluminum oxide.

What is the mass of 0.0490 mole of potassium sulfate?

A compound analyzes as 18.0% carbon,2.26% hydrogen,and 79.7% chlorine.Calculate the empirical formula of the compound.

How many grams of calcium are in 5.00 g of calcium hydroxide?

How much silver nitrate must be measured to yield 1.00 g silver?

Calculate the number of atoms in 0.377 grams of Ar.

Calculate the percentage composition of calcium chlorate.

Which of the following statements is/are incorrect?

Calculate the mass of silver in a sample of silver sulfide that contains 0.890 g of sulfur.

Calculate the formula mass of aluminum carbonate.

Determine the molecular formula of a compound that has a molar mass of 264 g/mol and the empirical formula C3H4O3.

A compound is composed of 74.0% C,8.70% H,and 17.3% N.Its molar mass is 162 g/mol.What is its molecular formula?

What is the empirical formula of a compound that contains 80.0% carbon and 20.0% hydrogen by mass?

Which of the following are empirical formulas? i.C10H8 ii.CH2 iii.Al2Cl6 iv.NO2 v.Hg2Cl2

Which of the following statements is incorrect?

Matter and Energy

Measurement and Chemical Calculations

Introduction to Gases

Atomic Theory: The Nuclear Model of the Atom

Chemical Nomenclature

Chemical Reactions

Chemical Change

Quantity Relationships in Chemical Reactions

Atomic Theory: The Quantum Model of the Atom

Chemical Bonding

Structure and Shape

The Ideal Gas Law and Its Applications

Gases, Liquids, and Solids

Solutions

Acidbase Proton Transferreactions

Chemical Equilibrium

Oxidationreduction Electron Transferreactions

Nuclear Chemistry

Organic Chemistry

Biochemistry

Filters

From the following,pick those that are empirical formulas. i.KCl ii.K₂S₂O₈ iii.K₂SO₄ iv.K₄S₂ v.KIO₃

Calculate the percent mercury and nitrogen in mercury(II)cyanide.The formula of the cyanide ion is CN^-.

What is the mass of 7.24 × 10²³ formula units of barium oxide?

Determine the molecular formula of a compound that has a molar mass of 264 g/mol and the empirical formula C₃H₄O₃.

Which of the following are empirical formulas? i.C₁₀H₈ ii.CH₂ iii.Al₂Cl₆ iv.NO₂ v.Hg₂Cl₂