Question 1

The molecular formula is a whole number multiple of the empirical formula.

Accepted Answer

A) True 
 B)False

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)   C18H36O2F) B) and D)
G) A) and C)

Question 3

Aluminum metal reacts with chlorine gas to form solid aluminum chloride. What mass of chlorine gas is required to react completely with 163 g of aluminum?

Accepted Answer

A)   214 g
B)   286 g
C)   321 g
D)   428 g
E)   643 gF) None of the above
G) B) and C)

Question 4

What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?

Accepted Answer

A)   25.8 g
B)   12.9 g
C)   78.2 g
D)   38.7 g
E)   77.4 gF) A) and C)
G) B) and D)

Question 5

What is the name given to the quantitative relationship between the substances that are consumed and produced in a chemical reaction?

Accepted Answer

A)   Law of definite proportions
B)   Law of molecular balance
C)   Percent composition
D)   Stoichiometry
E)   Percent equivalencyF) B) and E)
G) None of the above

Question 6

What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia?

Accepted Answer

A)   11.2 g
B)   0.06 g
C)   22.4 g
D)   16.5 g
E)   44.8 gF) A) and E)
G) A) and B)

Question 7

What is the molecular mass of acetaminophen, C8H9NO2?

Accepted Answer

A)   43 amu
B)   76 amu
C)   151 amu
D)   162 amu
E)   125 amuF) C) and E)
G) D) and E)

Question 8

Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol-1)

Accepted Answer

A)   2.92 × 1023 molecules
B)   4.73 × 10-25 molecules
C)   1.24 × 1023 molecules
D)   5.83 × 10-24 molecules
E)   1.71 × 1023 moleculesF) A) and B)
G) C) and D)

Question 9

Balance the following equation: UO2(s)  + HF(l)  → UF4(s)  + H2O(l)

Accepted Answer

A)   UO2(s)  + 2HF(l)  → UF4(s)  + H2O(l) 
B)   UO2(s)  + 4HF(l)  → UF4(s)  + 2H2O(l) 
C)   UO2(s)  + H4F4(l)  → UF4(s)  + H4O2(l) 
D)   UO2(s)  + 4HF(l)  → UF4(s)  + 4H2O(l) 
E)   UO2(s)  + 8HF(l)  → 2UF4(s)  + 4H2O(l) F) A) and D)
G) A) and B)

Question 10

What is the coefficient preceding O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C18H36O2 + ________ O2 → ________ CO2 + ________ H2O

Accepted Answer

A)   1
B)   8
C)   9
D)   26
E)   27F) All of the above
G) A) and B)

Question 11

Lead(II)  sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II)  sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II)  sulfide?

Accepted Answer

A)   151 g
B)   123 g
C)   50.3 g
D)   37.7 g
E)   9.41 gF) A) and D)
G) A) and E)

Question 12

Calculate the formula mass of rubidium carbonate, Rb2CO3.

Accepted Answer

A)   340.43 amu
B)   255.00 amu
C)   230.95 amu
D)   145.47 amu
E)   113.48 amuF) All of the above
G) A) and C)

Question 13

There is only one distinct empirical formula for each compound that exists.

Accepted Answer

A) True 
 B)False

Question 14

What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr2O3 → Al2O3 + 2Cr

Accepted Answer

A)   15.1 g
B)   30.2 g
C)   67.4 g
D)   99.9g
E)   104 gF) A) and E)
G) A) and D)

Question 15

What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0 moles of calcium based on the following chemical equation? V2O5(s)  + 5Ca(l)  → 2V(l)  + 5CaO(s)

Accepted Answer

A)   1.0 mol
B)   1.6 mol
C)   2.0 mol
D)   0.80 mol
E)   3.2 molF) A) and B)
G) C) and D)

Question 16

Balance the following equation for the combustion of benzene: C6H6(l)  + O2(g)  → H2O(g)  + CO2(g)

Accepted Answer

A)   C6H6(l)  + 9O2(g)  → 3H2O(g)  + 6CO2(g) 
B)   C6H6(l)  + 9O2(g)  → 6H2O(g)  + 6CO2(g) 
C)   2C6H6(l)  + 15O2(g)  → 6H2O(g)  + 12CO2(g) 
D)   C6H6(l)  + 15O2(g)  → 3H2O(g)  + 6CO2(g) 
E)   2C6H6(l)  + 9O2(g)  → 6H2O(g)  + 12CO2(g) F) B) and C)
G) B) and E)

Question 17

What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3 + 3C → 2Al + 3CO

Accepted Answer

A)   15.9 g
B)   31.8 g
C)   44.9 g
D)   63.6 g
E)   67.4 gF) A) and D)
G) B) and E)

Question 18

What is the coefficient of H2SO4 when the following equation is properly balanced with the smallest set of whole numbers? ________ Ca3(PO4) 2 + ________ H2SO4 → ________ CaSO4 + ________ H3PO4

Accepted Answer

A)   3
B)   8
C)   10
D)   11
E)   None of these answers is correct.F) A) and E)
G) A) and C)

Question 19

What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

Accepted Answer

A)   4.00 × 102 g
B)   25.0 g
C)   17.0 g
D)   4.00 × 10-2 g
E)   2.50 × 10-3 gF) A) and E)
G) A) and D)

Question 20

What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?

Accepted Answer

A)   3.26 g
B)   0.629 g
C)   13.04 g
D)   17.63 g
E)   6.52 gF) B) and D)
G) C) and D)

Exam 3: Stoichiometry: Ratios of Combination

What is the coefficient preceding O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C18H36O2 + ________ O2 → ________ CO2 + ________ H2O

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What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V2O5 with 4.0 moles of calcium based on the following chemical equation? V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Correct AnswerverifiedShow Answer

What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3 + 3C → 2Al + 3CO

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What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia?

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Balance the following equation: UO2(s) + HF(l) → UF4(s) + H2O(l)

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What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

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Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?

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What is the coefficient of H2SO4 when the following equation is properly balanced with the smallest set of whole numbers? ________ Ca3(PO4) 2 + ________ H2SO4 → ________ CaSO4 + ________ H3PO4

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What mass of nitrogen gas is required to react completely with 2.79 g of hydrogen gas to produce ammonia?

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There is only one distinct empirical formula for each compound that exists.

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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?

Correct AnswerverifiedShow Answer

Aluminum metal reacts with chlorine gas to form solid aluminum chloride. What mass of chlorine gas is required to react completely with 163 g of aluminum?

Correct AnswerverifiedShow Answer

Balance the following equation for the combustion of benzene: C6H6(l) + O2(g) → H2O(g) + CO2(g)

Correct AnswerverifiedShow Answer

What is the name given to the quantitative relationship between the substances that are consumed and produced in a chemical reaction?

Correct AnswerverifiedShow Answer

Calculate the formula mass of rubidium carbonate, Rb2CO3.

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Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol-1)

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What mass of ammonia is formed when 5.36 g of nitrogen gas reacts with excess hydrogen gas?

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What is the molecular mass of acetaminophen, C8H9NO2?

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What mass of Cr can be produced by the reaction of 44.1 g of Cr2O3 with 35.0 g of Al according to the following chemical equation? 2Al + Cr2O3 → Al2O3 + 2Cr

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The molecular formula is a whole number multiple of the empirical formula.

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What is the coefficient preceding O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? C₁₈H₃₆O₂ + O₂ → CO₂ + H₂O

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What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1.0 mole of V₂O₅ with 4.0 moles of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Correct Answer
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What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al₂O₃ + 3C → 2Al + 3CO

Correct Answer
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Balance the following equation: UO₂(s) + HF(l) → UF₄(s) + H₂O(l)

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What is the coefficient of H₂SO₄ when the following equation is properly balanced with the smallest set of whole numbers? Ca₃(PO₄) ₂ + H₂SO₄→ CaSO₄ + H₃PO₄

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Correct Answer
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Balance the following equation for the combustion of benzene: C₆H₆(l) + O₂(g) → H₂O(g) + CO₂(g)

Correct Answer
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Correct Answer
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Calculate the formula mass of rubidium carbonate, Rb₂CO₃.

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Determine the number of ammonia molecules in 4.85 g of ammonia. (N_A = 6.022 × 10²³ mol^-1)

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Correct Answer
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What is the molecular mass of acetaminophen, C₈H₉NO₂?

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What mass of Cr can be produced by the reaction of 44.1 g of Cr₂O₃ with 35.0 g of Al according to the following chemical equation? 2Al + Cr₂O₃→ Al₂O₃ + 2Cr

Correct Answer
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Correct Answer
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