Question 1

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 B)
G) C) and D)

Question 2

What is the average mass,in grams,of one atom of iron? (NA = 6.022 × 1023 mol-1)

Accepted Answer

A)  6.02 × 1023 g
B)  1.66 × 10-24 g
C)  9.27 × 10-23 g
D)  55.85 g
E)  55.85 × 10-23 gF) A) and D)
G) B) and E)

Question 3

Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form nitrogen trichloride?

Accepted Answer

A)   
B)   
C)   
D)   
E)   F) A) and D)
G) A) and B)

Question 4

Many compounds can be represented with the same empirical formula.

Accepted Answer

A) True 
 B)False

Question 5

What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol-1)

Accepted Answer

A)  3.88 × 1021 g
B)  2.00 mg
C)  32.06 g
D)  6.44 mg
E)  2.00 × 10-4 gF) C) and E)
G) B) and C)

Question 6

The ____ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

Accepted Answer

The answer of The ____ is the amount of product...

Question 7

Calculate the molar mass of sulfuric acid.

Accepted Answer

A)  98.086 g/mol
B)  81.078 g/mol
C)  49 g/mol
D)  41 g/mol
E)  None of the answers are correct.F) A) and C)
G) A) and B)

Question 8

What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole 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)  2.4 mol
E)  4.0 molF) C) and E)
G) B) and E)

Question 9

What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine by mass?

Accepted Answer

A)  U2F
B)  U3F4
C)  UF4
D)  UF6
E)  UF8F) C) and D)
G) B) and C)

Question 10

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Accepted Answer

A)  90.g
B)  36 g
C)  42 g
D)  45 g
E)  108 gF) B) and E)
G) B) and C)

Question 11

Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.)  __ SF4 + __ H2O → __ H2SO3 + __ HF

Accepted Answer

A)  4
B)  6
C)  7
D)  9
E)  None of these answers is correct.F) C) and E)
G) A) and C)

Question 12

A compound was discovered whose composition by mass is 85.6% C and 14.4% H.Which of these formulas could be the molecular formula of this compound?

Accepted Answer

A)  CH4
B)  C2H4
C)  C3H4
D)  C2H6
E)  C3H8F) A) and B)
G) B) and D)

Question 13

How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

Accepted Answer

A)  6.52 g
B)  7.29 g
C)  13.0 g
D)  14.6 g
E)  58.4 gF) A) and E)
G) A) and B)

Question 14

How many moles are present in 17.4 g of lead?

Accepted Answer

A)  0.0994 moles
B)  1.05 × 1025 moles
C)  0.0840 moles
D)  10.06 moles
E)  11.9 molesF) All of the above
G) A) and C)

Question 15

What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

Accepted Answer

A)  12.8 g
B)  25.6 g
C)  6.39 g
D)  0.399 g
E)  51.1 gF) A) and D)
G) C) and D)

Question 16

What is the percent carbon in CH3CH2OH?

Accepted Answer

A)  13%
B)  26%
C)  35%
D)  46%
E)  52%F) A) and E)
G) B) and E)

Question 17

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.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) All of the above
G) A) and B)

Question 18

Hydroxylammonium nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.What is its empirical formula?

Accepted Answer

A)  HNO
B)  H2NO2
C)  HN6O16
D)  HN16O7
E)  H2NO3F) B) and D)
G) B) and C)

Question 19

Calculate the molecular mass of menthol,C10H20O.

Accepted Answer

A)  156 amu
B)  140 amu
C)  29 amu
D)  146 amu
E)  136 amuF) A) and C)
G) B) and D)

Question 20

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) B) and D)
G) C) and D)

Exam 3: Stoichiometry Ratios of Combination

Many compounds can be represented with the same empirical formula.

Correct AnswerverifiedShow Answer

Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form nitrogen trichloride?

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What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine by mass?

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What is the molecular mass of acetaminophen,C8H9NO2?

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The ____ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

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What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

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A compound was discovered whose composition by mass is 85.6% C and 14.4% H.Which of these formulas could be the molecular formula of this compound?

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What is the percent carbon in CH3CH2OH?

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

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Calculate the molecular mass of menthol,C10H20O.

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Calculate the molar mass of sulfuric acid.

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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?

Correct AnswerverifiedShow Answer

How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

Correct AnswerverifiedShow Answer

Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.) __ SF4 + __ H2O → __ H2SO3 + __ HF

Correct AnswerverifiedShow Answer

What is the average mass,in grams,of one atom of iron? (NA = 6.022 × 1023 mol-1)

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What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

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What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol-1)

Correct AnswerverifiedShow Answer

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Correct AnswerverifiedShow Answer

Hydroxylammonium nitrate contains 29.17 mass % N,4.20 mass % H,and 66.63 mass % O.What is its empirical formula?

Correct AnswerverifiedShow Answer

How many moles are present in 17.4 g of lead?

Correct AnswerverifiedShow Answer

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What is the molecular mass of acetaminophen,C₈H₉NO₂?

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What is the percent carbon in CH₃CH₂OH?

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Calculate the molecular mass of menthol,C₁₀H₂₀O.

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How many grams of Cl₂ can be prepared from the reaction of 16.0 g of MnO₂ and 30.0 g of HCl according to the following balanced chemical equation? MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

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Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.) SF₄ + H₂O → H₂SO₃ + HF

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What is the average mass,in grams,of one atom of iron? (N_A = 6.022 × 10²³ mol^-1)

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What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

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What is the mass of 1.21 × 10²⁰atoms of sulfur? (N_A = 6.022 × 10²³ mol^-1)

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How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

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