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CHM 101 EXAM 2 — DONOVAN 2026/2027 COMPLETE
(100) CURRENT TESTING QUESTIONS AND CORRECT
ANSWERS WITH DETAILED RATIONALES.
CHM
Prepare for CHM 101 Exam 2 – Donovan with a focused study resource covering
foundational chemistry concepts and essential principles introduced early in the
course. It is designed to support review of key topics, reinforce understanding, and
help you recognize areas that may require additional study. Use the practice material
to structure your preparation and build confidence before the exam. This resource is
best suited for CHM 101 students preparing for Exam 1 and reviewing introductory
chemistry concepts.
MULTIPLE CHOICE.
TOPIC 1: The Mole & Molar Mass (Questions 1–10)
Question 1:
What is the molar mass of calcium carbonate (CaCO₃)?
A) 68.08 g/mol
B) 84.08 g/mol
C) 100.09 g/mol
D) 116.09 g/mol
Answer: C) 100.09 g/mol
Rationale: The molar mass is calculated by summing the atomic masses:
Ca (40.08) + C (12.01) + O₃ (3 × 16.00) = 100.09 g/mol. Option A omits
oxygen, B uses incorrect values, and D adds an extra oxygen.
Question 2:
How many moles are present in 22.0 g of CO₂?
A) 0.25 mol
B) 0.50 mol
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C) 1.00 mol
D) 2.00 mol
Answer: B) 0.50 mol
Rationale: Molar mass of CO₂ = 12.01 + 2(16.00) = 44.01 g/mol. Moles =
22.0 g / 44.01 g/mol = 0.50 mol. Option A would be 11 g, C would be 44 g,
and D would be 88 g.
Question 3:
Avogadro's number is equal to:
A) 6.022 × 10²²
B) 6.022 × 10²³
C) 6.022 × 10²⁴
D) 6.022 × 10²⁵
Answer: B) 6.022 × 10²³
Rationale: Avogadro's number is defined as the number of particles in one
mole of a substance, which is 6.022 × 10²³. Options A, C, and D represent
incorrect powers of ten.
Question 4:
What is the mass in grams of 3.00 moles of water (H₂O)?
A) 18.02 g
B) 36.04 g
C) 54.06 g
D) 72.08 g
Answer: C) 54.06 g
Rationale: Molar mass of H₂O = 2(1.008) + 16.00 = 18.016 g/mol. Mass =
3.00 mol × 18.016 g/mol = 54.06 g. Option A is 1 mole, B is 2 moles, and D is
4 moles.
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Question 5:
How many molecules are present in 2.50 moles of NaCl?
A) 1.51 × 10²⁴ molecules
B) 3.01 × 10²³ molecules
C) 6.02 × 10²³ molecules
D) 1.20 × 10²⁴ molecules
Answer: A) 1.51 × 10²⁴ molecules
Rationale: Molecules = moles × Avogadro's number = 2.50 × 6.022 × 10²³ =
1.5055 × 10²⁴ molecules. Option B is 0.5 mol, C is 1 mol, and D is 2 mol.
Question 6:
Calculate the molar mass of glucose (C₆H₁₂O₆).
A) 120.16 g/mol
B) 150.16 g/mol
C) 180.16 g/mol
D) 210.16 g/mol
Answer: C) 180.16 g/mol
Rationale: Molar mass = 6(12.01) + 12(1.008) + 6(16.00) = 72.06 + 12.096 +
96.00 = 180.156 g/mol. Option A is missing carbons, B is missing oxygens,
and D adds extra atoms.
Question 7:
How many moles of oxygen atoms are in 1.00 mole of CO₂?
A) 0.50 mol
B) 1.00 mol
C) 1.50 mol
D) 2.00 mol
Answer: D) 2.00 mol
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Rationale: Each molecule of CO₂ contains 2 oxygen atoms. Therefore, 1.00
mole of CO₂ contains 2.00 moles of oxygen atoms. Option A would be for
0.5 mol CO₂, B is incorrect, and C is not stoichiometrically valid.
Question 8:
What is the mass of 4.50 × 10²³ atoms of iron (Fe)?
A) 20.9 g
B) 41.8 g
C) 55.8 g
D) 83.7 g
Answer: B) 41.8 g
Rationale: Moles = 4.50 × 10²³ / 6.022 × 10²³ = 0.747 mol. Mass = 0.747 mol
× 55.85 g/mol = 41.8 g. Option A uses incorrect molar mass, C is 1 mole,
and D is 1.5 moles.
Question 9:
The molar mass of sulfuric acid (H₂SO₄) is approximately:
A) 82.08 g/mol
B) 98.09 g/mol
C) 114.09 g/mol
D) 130.09 g/mol
Answer: B) 98.09 g/mol
Rationale: Molar mass = 2(1.008) + 32.07 + 4(16.00) = 2.016 + 32.07 + 64.00 =
98.086 g/mol. Option A misses sulfur, C adds oxygen, and D adds extra
atoms.
Question 10:
How many grams are in 0.750 moles of methane (CH₄)?
A) 4.00 g
B) 8.00 g
CHM 101 EXAM 2 — DONOVAN 2026/2027 COMPLETE
(100) CURRENT TESTING QUESTIONS AND CORRECT
ANSWERS WITH DETAILED RATIONALES.
CHM
Prepare for CHM 101 Exam 2 – Donovan with a focused study resource covering
foundational chemistry concepts and essential principles introduced early in the
course. It is designed to support review of key topics, reinforce understanding, and
help you recognize areas that may require additional study. Use the practice material
to structure your preparation and build confidence before the exam. This resource is
best suited for CHM 101 students preparing for Exam 1 and reviewing introductory
chemistry concepts.
MULTIPLE CHOICE.
TOPIC 1: The Mole & Molar Mass (Questions 1–10)
Question 1:
What is the molar mass of calcium carbonate (CaCO₃)?
A) 68.08 g/mol
B) 84.08 g/mol
C) 100.09 g/mol
D) 116.09 g/mol
Answer: C) 100.09 g/mol
Rationale: The molar mass is calculated by summing the atomic masses:
Ca (40.08) + C (12.01) + O₃ (3 × 16.00) = 100.09 g/mol. Option A omits
oxygen, B uses incorrect values, and D adds an extra oxygen.
Question 2:
How many moles are present in 22.0 g of CO₂?
A) 0.25 mol
B) 0.50 mol
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C) 1.00 mol
D) 2.00 mol
Answer: B) 0.50 mol
Rationale: Molar mass of CO₂ = 12.01 + 2(16.00) = 44.01 g/mol. Moles =
22.0 g / 44.01 g/mol = 0.50 mol. Option A would be 11 g, C would be 44 g,
and D would be 88 g.
Question 3:
Avogadro's number is equal to:
A) 6.022 × 10²²
B) 6.022 × 10²³
C) 6.022 × 10²⁴
D) 6.022 × 10²⁵
Answer: B) 6.022 × 10²³
Rationale: Avogadro's number is defined as the number of particles in one
mole of a substance, which is 6.022 × 10²³. Options A, C, and D represent
incorrect powers of ten.
Question 4:
What is the mass in grams of 3.00 moles of water (H₂O)?
A) 18.02 g
B) 36.04 g
C) 54.06 g
D) 72.08 g
Answer: C) 54.06 g
Rationale: Molar mass of H₂O = 2(1.008) + 16.00 = 18.016 g/mol. Mass =
3.00 mol × 18.016 g/mol = 54.06 g. Option A is 1 mole, B is 2 moles, and D is
4 moles.
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Question 5:
How many molecules are present in 2.50 moles of NaCl?
A) 1.51 × 10²⁴ molecules
B) 3.01 × 10²³ molecules
C) 6.02 × 10²³ molecules
D) 1.20 × 10²⁴ molecules
Answer: A) 1.51 × 10²⁴ molecules
Rationale: Molecules = moles × Avogadro's number = 2.50 × 6.022 × 10²³ =
1.5055 × 10²⁴ molecules. Option B is 0.5 mol, C is 1 mol, and D is 2 mol.
Question 6:
Calculate the molar mass of glucose (C₆H₁₂O₆).
A) 120.16 g/mol
B) 150.16 g/mol
C) 180.16 g/mol
D) 210.16 g/mol
Answer: C) 180.16 g/mol
Rationale: Molar mass = 6(12.01) + 12(1.008) + 6(16.00) = 72.06 + 12.096 +
96.00 = 180.156 g/mol. Option A is missing carbons, B is missing oxygens,
and D adds extra atoms.
Question 7:
How many moles of oxygen atoms are in 1.00 mole of CO₂?
A) 0.50 mol
B) 1.00 mol
C) 1.50 mol
D) 2.00 mol
Answer: D) 2.00 mol
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Rationale: Each molecule of CO₂ contains 2 oxygen atoms. Therefore, 1.00
mole of CO₂ contains 2.00 moles of oxygen atoms. Option A would be for
0.5 mol CO₂, B is incorrect, and C is not stoichiometrically valid.
Question 8:
What is the mass of 4.50 × 10²³ atoms of iron (Fe)?
A) 20.9 g
B) 41.8 g
C) 55.8 g
D) 83.7 g
Answer: B) 41.8 g
Rationale: Moles = 4.50 × 10²³ / 6.022 × 10²³ = 0.747 mol. Mass = 0.747 mol
× 55.85 g/mol = 41.8 g. Option A uses incorrect molar mass, C is 1 mole,
and D is 1.5 moles.
Question 9:
The molar mass of sulfuric acid (H₂SO₄) is approximately:
A) 82.08 g/mol
B) 98.09 g/mol
C) 114.09 g/mol
D) 130.09 g/mol
Answer: B) 98.09 g/mol
Rationale: Molar mass = 2(1.008) + 32.07 + 4(16.00) = 2.016 + 32.07 + 64.00 =
98.086 g/mol. Option A misses sulfur, C adds oxygen, and D adds extra
atoms.
Question 10:
How many grams are in 0.750 moles of methane (CH₄)?
A) 4.00 g
B) 8.00 g
