One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na3(CO3)(HCO3)·2H2O. 2Na3(CO3)(HCO3)·2H2O(s) → 3Na2CO3(s) + CO2(g) + 5H2O(g) When 1.00 metric ton (1.00 × 103 kg) of trona is decomposed, 0.650 metric ton of Na2CO3 is recovered.What is the percent yield of this reaction?

A) 92.4% B) 72.1% C) 65.0% D) 48.1% E) 35.0% A) 92.4% B) 72.1% C) 65.0% D) 48.1% E) 35.0%

How much heat is released if 7.15 g CaO(s) is added to 152 g of H2O(l)? CaO(s) + H2O(l) → Ca(OH)2(s) heat of reaction = −64.8 kJ/mol

A) 7.68 kJ B) 8.26 kJ C) 508 kJ D) 547 kJ E) 555 kJ A) 7.68 kJ B) 8.26 kJ C) 508 kJ D) 547 kJ E) 555 kJ

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

A) 10.0 g B) 12.5 g C) 22.5 g D) 55.0 g E) 77.5 g A) 10.0 g B) 12.5 g C) 22.5 g D) 55.0 g E) 77.5 g

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

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

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? 8Fe(s) + S8(s) → 8FeS(s)

A) 186 g B) 142 g C) 119 g D) 14.8 g E) 0.169 g A) 186 g B) 142 g C) 119 g D) 14.8 g E) 0.169 g

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)

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

Exam 11: Using Balanced Chemical Equations

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na₃(CO₃)(HCO₃)·2H₂O. 2Na₃(CO₃)(HCO₃)·2H₂O(s) → 3Na₂CO₃(s) + CO₂(g) + 5H₂O(g) When 1.00 metric ton (1.00 × 10³ kg) of trona is decomposed, 0.650 metric ton of Na₂CO₃ is recovered.What is the percent yield of this reaction?

(Multiple Choice)

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Question 21

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

(Multiple Choice)

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Question 22

How much heat is released if 7.15 g CaO(s) is added to 152 g of H₂O(l)? CaO(s) + H₂O(l) → Ca(OH)₂(s) heat of reaction = −64.8 kJ/mol

(Multiple Choice)

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Question 23

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

(Multiple Choice)

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Question 24

What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 25

What volume of 0.307 M K₂SO₄ solution is required to react exactly with 85.0 mL of 0.100 M AgNO₃? K₂SO₄(aq) + 2AgNO₃(aq) → 2KNO₃(aq) + Ag₂SO₄(s)

(Multiple Choice)

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Question 26

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

(Multiple Choice)

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Question 27

How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

(Multiple Choice)

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Question 28

Magnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron.A mixture of 41.0 g of magnesium and 175.0 g of iron(III) chloride is allowed to react.Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

(Multiple Choice)

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Question 29

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?

(Multiple Choice)

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Question 30

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles).SO₂(g) + 2Cl₂(g) → SOCl₂(g) + Cl₂O(g) If 0.400 mol of Cl₂ reacts with excess SO₂, how many moles of Cl₂O are formed?

(Multiple Choice)

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Question 31

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

(Multiple Choice)

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Question 32

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

(Multiple Choice)

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Question 33

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

(Multiple Choice)

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Question 34

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

(Multiple Choice)

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Question 35

What volume of 0.233 M H₂SO₄ is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3H₂(g)

(Multiple Choice)

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Question 36

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

(Multiple Choice)

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Question 37

Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO₃)₂ solution. 2KI(aq) + Pb(NO₃)₂(aq) → PbI₂(s) + 2KNO₃(aq)

(Multiple Choice)

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Question 38

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)

(Multiple Choice)

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Question 39

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

(Multiple Choice)

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Question 40

Showing 21 - 40 of 61

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

How much heat is released if 7.15 g CaO(s) is added to 152 g of H₂O(l)? CaO(s) + H₂O(l) → Ca(OH)₂(s) heat of reaction = −64.8 kJ/mol

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

What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

What volume of 0.307 M K₂SO₄ solution is required to react exactly with 85.0 mL of 0.100 M AgNO₃? K₂SO₄(aq) + 2AgNO₃(aq) → 2KNO₃(aq) + Ag₂SO₄(s)

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

How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

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?

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

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

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

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

What volume of 0.233 M H₂SO₄ is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3H₂(g)

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO₃)₂ solution. 2KI(aq) + Pb(NO₃)₂(aq) → PbI₂(s) + 2KNO₃(aq)

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)

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Atoms and Elements

Electrons and the Periodic Table

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How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

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Exam 11: Using Balanced Chemical Equations

If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced?

How much heat is released if 7.15 g CaO(s) is added to 152 g of H2O(l)? CaO(s) + H2O(l) → Ca(OH)2(s) heat of reaction = −64.8 kJ/mol

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

What mass of KClO3 must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

What volume of 0.307 M K2SO4 solution is required to react exactly with 85.0 mL of 0.100 M AgNO3? K2SO4(aq) + 2AgNO3(aq) → 2KNO3(aq) + Ag2SO4(s)

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

How many grams of calcium metal is required to react with 7.75 g water to produce calcium hydroxide and hydrogen gas?

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?

Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles).SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g) If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?

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

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

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

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S8? 8Fe(s) + S8(s) → 8FeS(s)

What volume of 0.233 M H2SO4 is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO3)2 solution. 2KI(aq) + Pb(NO3)2(aq) → PbI2(s) + 2KNO3(aq)

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)

Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure.Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Solids, Liquids, and Phase Changes

Gases

Physical Properties of Solutions

Chemical Reactions and Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

How much heat is released if 7.15 g CaO(s) is added to 152 g of H₂O(l)? CaO(s) + H₂O(l) → Ca(OH)₂(s) heat of reaction = −64.8 kJ/mol

What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? (The other reaction product is solid KCl.) (R = 0.08206 L • atm/K • mol)

What volume of 0.307 M K₂SO₄ solution is required to react exactly with 85.0 mL of 0.100 M AgNO₃? K₂SO₄(aq) + 2AgNO₃(aq) → 2KNO₃(aq) + Ag₂SO₄(s)

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

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

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

What mass of FeS is formed if 9.42 g of Fe reacts with 68.0 g of S₈? 8Fe(s) + S₈(s) → 8FeS(s)

What volume of 0.233 M H₂SO₄ is needed to react exactly with 15.0 grams of aluminum? 2Al(s) + 3H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 3H₂(g)

Determine the mass of precipitate (in grams) that forms when 425.1 mL of 0.122 M KI solution is reacted with excess Pb(NO₃)₂ solution. 2KI(aq) + Pb(NO₃)₂(aq) → PbI₂(s) + 2KNO₃(aq)

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)