Question 1

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) A) and E)

Question 2

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

Question 3

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) D) and E)
G) C) and E)

Question 4

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 B)
G) A) and C)

Question 5

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) B) and D)

Question 6

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 C)
G) All of the above

Question 7

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) None of the above
G) B) and C)

Question 8

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) C) and E)
G) A) and B)

Question 9

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) All of the above
G) B) and E)

Question 10

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) A) and B)
G) A) and C)

Question 11

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 B)
G) A) and E)

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) B) and E)
G) A) and B)

Question 13

Many compounds can be represented with the same empirical formula.

Accepted Answer

A) True 
 B)False

Question 14

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) All of the above
G) A) and E)

Question 15

What is the percent carbon in CH3CH2OH?

Accepted Answer

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

Question 16

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) C) and D)
G) D) and E)

Question 17

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) C) and D)
G) All of the above

Question 18

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 19

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) A) and E)
G) B) and E)

Question 20

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

Exam 3: Stoichiometry Ratios of Combination

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

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How many moles are present in 17.4 g of lead?

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

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What is the percent carbon in CH3CH2OH?

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What is the molecular mass of acetaminophen,C8H9NO2?

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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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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 molar mass of sulfuric acid.

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Many compounds can be represented with the same empirical formula.

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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

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

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

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

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Calculate the molecular mass of menthol,C10H20O.

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

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

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What is the percent carbon in CH₃CH₂OH?

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What is the molecular mass of acetaminophen,C₈H₉NO₂?

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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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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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Calculate the molecular mass of menthol,C₁₀H₂₀O.

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

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