Question 1

The empirical formula of C6H6 is CH.

Accepted Answer

A) True 
 B)False

Question 2

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 C)
G) A) and B)

Question 3

If 31.3 g of manganese(II) chloride,48.3 g of chlorine gas,and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid,what is the limiting reactant and what mass of hydrochloric acid is produced?

Accepted Answer

A)  manganese(II) chloride is the limiting reactant and 9.07 g of hydrochloric acid is produced
B)  chlorine is the limiting reactant and 99.3 g of hydrochloric acid is produced
C)  chlorine is the limiting reactant and 24.8 g of hydrochloric acid is produced
D)  manganese(II) chloride is the limiting reactant and 36.3 g of hydrochloric acid is produced
E)  water is the limiting reactant and 52.0 g of hydrochloric acid is producedF) B) and E)
G) A) and D)

Question 4

Phosphorus pentachloride,a white solid that has a pungent,unpleasant odor,is used as a catalyst for certain organic reactions.Calculate the number of moles in 38.7 g of phosphorus pentachloride.

Accepted Answer

A)  5.38 mol
B)  3.55 mol
C)  0.583 mol
D)  0.282 mol
E)  0.186 molF) A) and B)
G) B) and E)

Question 5

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.)  ___ Al + ___ H2SO4 → ___ Al2(SO4) 3 + ___ H2

Accepted Answer

A)  3
B)  5
C)  6
D)  9
E)  12F) A) and C)
G) None of the above

Question 6

Which could represent the reaction mixture after the complete combustion of acetaldehyde,CH3CHO?

Accepted Answer

A)   3CHO? 
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C)   3CHO? 
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D)   3CHO? 
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G) D) and E)

Question 7

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

Question 8

Balance the following equation: Ca3(PO4) 2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)

Accepted Answer

A)  Ca3(PO4) 2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + P4(s) 
B)  Ca3(PO4) 2(s) + 3SiO2(s) + 14C(s) → 3CaSiO3(s) + 14CO(g) + P4(s) 
C)  Ca3(PO4) 2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + 2P4(s) 
D)  2Ca3(PO4) 2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + P4(s) 
E)  2Ca3(PO4) 2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + 4P4(s) F) A) and B)
G) All of the above

Question 9

The ______________ is the one component that is completely consumed during a chemical reaction.

Accepted Answer

The answer of The ______________ is the one component that...

Question 10

Calculate the formula mass of (NH4) 3AsO4.

Accepted Answer

A)  417.80 amu
B)  193.05 amu
C)  165.02 amu
D)  156.96 amu
E)  108.96 amuF) A) and C)
G) A) and E)

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.)  ___ Cr + ___ H2SO4 → ___ Cr2(SO4) 3 + ___H2

Accepted Answer

A)  4
B)  9
C)  11
D)  13
E)  15F) C) and E)
G) None of the above

Question 12

Calculate the molar mass of Ca(BO2) 2·6H2O.

Accepted Answer

A)  273.87 g/mol
B)  233.80 g/mol
C)  183.79 g/mol
D)  174.89 g/mol
E)  143.71 g/molF) A) and E)
G) None of the above

Question 13

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

Accepted Answer

A)  5.48 × 10-23 g
B)  33.0 g
C)  74.9 g
D)  1.24 × 10-22 g
E)  8.04 × 1021 gF) A) and B)
G) A) and C)

Question 14

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH3 + 5O2 → __________4NO + 6H2O
What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react?

Accepted Answer

A)  1.56mol
B)  1.88 mol
C)  3.52 mol
D)  3.91 mol
E)  2.35 molF) None of the above
G) A) and D)

Question 15

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

Question 16

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO2 + O2 → 2SO3

Accepted Answer

A)  10.0 g
B)  12.5 g
C)  22.5 g
D)  55.0 g
E)  77.5 gF) C) and D)
G) All of the above

Question 17

Suppose white atoms (W) and black atoms (B) react according to the following balanced chemical equation. 2W + B → BW2
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Accepted Answer

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Question 18

Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced]
Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

Accepted Answer

A)  1880 g
B)  940.g
C)  900.g
D)  470.g
E)  56.3 gF) A) and B)
G) B) and E)

Question 19

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) B) and E)
G) B) and D)

Question 20

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

Exam 3: Stoichiometry Ratios of Combination

What mass of excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO2 + O2 → 2SO3

Correct AnswerverifiedShow Answer

Which could represent the reaction mixture after the complete combustion of acetaldehyde,CH3CHO?

Correct AnswerverifiedShow Answer

If 31.3 g of manganese(II) chloride,48.3 g of chlorine gas,and 25.7 g of water react to produce manganese(IV) oxide and hydrochloric acid,what is the limiting reactant and what mass of hydrochloric acid is produced?

Correct AnswerverifiedShow Answer

Calculate the formula mass of (NH4) 3AsO4.

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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?

Correct AnswerverifiedShow Answer

Suppose white atoms (W) and black atoms (B) react according to the following balanced chemical equation. 2W + B → BW2 If the initial reaction mixture is prepared as follows,what will the final reaction mixture be once the reaction is complete?

Correct AnswerverifiedShow Answer

Calculate the molar mass of Ca(BO2) 2·6H2O.

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The ______________ is the one component that is completely consumed during a chemical reaction.

Correct AnswerverifiedShow Answer

Phosphorus pentachloride,a white solid that has a pungent,unpleasant odor,is used as a catalyst for certain organic reactions.Calculate the number of moles in 38.7 g of phosphorus pentachloride.

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Balance the following equation: Ca3(PO4) 2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)

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

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Calculate the formula mass of rubidium carbonate,Rb2CO3.

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Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH3(g) + O2(g) → P4O10(s) + H2O(g) [unbalanced] Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

Correct AnswerverifiedShow Answer

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

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.) ___ Cr + ___ H2SO4 → ___ Cr2(SO4) 3 + ___H2

Correct AnswerverifiedShow Answer

Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH3 + 5O2 → __________4NO + 6H2O What is the maximum amount of water that may be produced if 40.0 g NH3 and 50.0 g O2 are mixed and allowed to react?

Correct AnswerverifiedShow Answer

The empirical formula of C6H6 is CH.

Correct AnswerverifiedShow Answer

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

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.) ___ Al + ___ H2SO4 → ___ Al2(SO4) 3 + ___ H2

Correct AnswerverifiedShow Answer

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 excess reactant remains at the end of the reaction if 90.0 g of SO2 are mixed with 100.0 g of O2? 2SO₂ + O₂ → 2SO₃

Correct Answer
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Which could represent the reaction mixture after the complete combustion of acetaldehyde,CH₃CHO?

Correct Answer
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Correct Answer
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Calculate the formula mass of (NH₄) ₃AsO₄.

Correct Answer
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Correct Answer
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Suppose white atoms (W) and black atoms (B) react according to the following balanced chemical equation. 2W + B → BW₂ If the initial reaction mixture is prepared as follows,what will the final reaction mixture be once the reaction is complete?

Correct Answer
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Calculate the molar mass of Ca(BO₂) ₂·6H₂O.

Correct Answer
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Correct Answer
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Correct Answer
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Balance the following equation: Ca₃(PO₄) ₂(s) + SiO₂(s) + C(s) → CaSiO₃(s) + CO(g) + P₄(s)

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

Correct Answer
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Phosphine,an extremely poisonous and highly reactive gas,reacts with oxygen gas to form tetraphosphorus decaoxide and water. PH₃(g) + O₂(g) → P₄O₁₀(s) + H₂O(g) [unbalanced] Calculate the mass of P₄O₁₀(s) formed when 225 g of PH₃ reacts with excess oxygen.

Correct Answer
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Correct Answer
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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.) _ Cr + _ H₂SO₄ → _ Cr₂(SO₄) ₃ + _H₂

Correct Answer
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Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor as follows: 4NH₃ + 5O₂ → __________4NO + 6H₂O What is the maximum amount of water that may be produced if 40.0 g NH₃ and 50.0 g O₂ are mixed and allowed to react?

Correct Answer
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The empirical formula of C₆H₆ is CH.

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

Correct Answer
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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.) _ Al + _ H₂SO₄ → _ Al₂(SO₄) ₃ + _ H₂

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

Correct Answer
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