Deck 11: Using Balanced Chemical Equations

Question 1

How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?

A)5.82 g
B)14.33 g
C)0.086 g
D)11.64 g
E)16.52 g

Answer 1

11.64 g

Question 2

Aluminum reacts with bromine to form aluminum bromide (used as an acid catalyst in organic synthesis). Al(s) + Br₂(l) → Al₂Br₆(s) [unbalanced]
How many moles of Al are needed to form 2.43 mol of Al₂Br₆?

A)7.29 mol
B)4.86 mol
C)2.43 mol
D)1.62 mol
E)1.22 mol

Answer 2

4.86 mol

Question 3

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

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

Answer 3

12.9 g

Question 4

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)

A)1.0 mol
B)1.6 mol
C)2.0 mol
D)2.4 mol
E)4.0 mol

Question 5

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?

A)214 g
B)286g
C)321 g
D)428 g
E)643 g

Question 6

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.

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

Question 7

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

Question 8

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?

A)0.800 mol
B)0.400 mol
C)0.200 mol
D)0.100 mol
E)0.0500 mol

Question 9

What mass of sodium fluoride (used in water fluoridation and the manufacture of insecticides) is required to form 485 g of sulfur tetrafluoride? 3SCl₂(l) + 4NaF(s) → SF₄(g) + S₂Cl₂(l) + 4NaCl(s)

A)1.94 kg
B)1.51 kg
C)754 g
D)205 g
E)51.3 g

Question 10

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

A)8.62 g
B)34.5 g
C)4.31 g
D)40.1 g
E)17.2 g

Question 11

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

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

Question 12

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

Question 13

Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs). 2NH₃(g) + 5F₂(g) → N₂F₄(g) + 6HF(g)
How many moles of NH₃ are needed to react completely with 13.6 mol of F₂?

A)34.0 mol
B)27.2 mol
C)6.80 mol
D)5.44 mol
E)2.27 mol

Question 14

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?

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

Question 15

Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H₂SO₄(aq) → 2HCl(g) + Na₂SO₄(s) What mass of HCl can be prepared from 2.00 mol H₂SO₄ and 150.g NaCl?

A)2.57 g
B)46.8 g
C)93.6g
D)146 g
E)167g

Question 16

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?

A)28.1 g
B)14.04 g
C)4.96 g
D)7.02 g
E)400.0 g

Question 17

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

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

Question 18

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

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

Question 19

Potassium chlorate (used in fireworks, flares, and safety matches) forms oxygen and potassium chloride when heated. KClO₃(s) → KCl(s) + O₂(g) [unbalanced]
What mass of oxygen gas is formed if 26.4 g of potassium chlorate decomposes completely?

A)223 g
B)99.1 g
C)10.3 g
D)6.86 g
E)4.60 g

Question 20

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

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

Question 21

Methanol (CH₃OH) is converted to bromomethane (CH₃Br) as follows: CH₃OH + HBr → CH₃Br + H₂O If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield?

A)12.9%
B)33.8%
C)40.9%
D)59.1%
E)82.6%

Question 22

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

Question 23

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.

A)Chlorine is the limiting reactant; 1.14 g of potassium remain.
B)Potassium is the limiting reactant; 2.00 g of chlorine remain.
C)Potassium is the limiting reactant; 2.47 g of chlorine remain.
D)Chlorine is the limiting reactant; 3.07 g of potassium remain.
E)Potassium is the limiting reactant; 4.50 g of chlorine remain.

Question 24

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

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

Question 25

Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas.If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P₄O₆, what is the percent yield for the reaction?

A)57.5%
B)48.8%
C)38.0%
D)89.4%
E)16.3%

Question 26

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

Question 27

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?

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 produced

Question 28

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

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

Question 29

If 119.3 g of PCl₅ are formed from the reaction of 61.3 g Cl₂ with excess PCl₃, what is the percent yield? PCl₃(g) + Cl₂(g) → PCl₅(g)

A)94.6%
B)66.3%
C)57.3%
D)51.3%
E)48.6%

Question 30

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.

A)Limiting reactant is Mg; 7.4 g of FeCl₃ remain.
B)Limiting reactant is Mg; 46.5 g of FeCl₃ remain.
C)Limiting reactant is FeCl₃; 1.7 g of Mg remain.
D)Limiting reactant is FeCl₃; 37.8 g of Mg remain.
E)Limiting reactant is Mg; 134.0 g of FeCl₃ remain.

Question 31

What is the maximum number of grams of ammonia, NH₃, which can be obtained from the reaction of 10.0 g of H₂ and 80.0 g of N₂? N₂ + 3H₂ → 2NH₃

A)34.1 g
B)48.6 g
C)56.3 g
D)90.0 g
E)97.3 g

Question 32

Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions.A mixture of 82.49 g of aluminum and 117.65 g of oxygen 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.

A)Oxygen is the limiting reactant; 19.81 g of aluminum remain.
B)Oxygen is the limiting reactant; 35.16 g of aluminum remain.
C)Aluminum is the limiting reactant; 16.70 g of oxygen remain.
D)Aluminum is the limiting reactant; 35.16 g of oxygen remain.
E)Aluminum is the limiting reactant; 44.27 g of oxygen remain.

Question 33

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)

A)5.19 g
B)2.59 g
C)12.0 g
D)3.48 g
E)9.55 g

Question 34

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V₂O₅ with 40.0 g of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

A)11.2 g
B)5.6 g
C)22.4 g
D)40.0 g
E)20.3 g

Question 35

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?

A)1.56mol
B)1.88 mol
C)3.52 mol
D)3.91 mol
E)2.35 mol

Question 36

If 3.41 g of nitrogen react with 2.79 g of hydrogen to produce ammonia, what is the limiting reactant and what mass of ammonia is produced?

A)Hydrogen is the limiting reactant and 0.22 g of ammonia are produced.
B)Nitrogen is the limiting reactant and 2.07 g of ammonia are produced.
C)Nitrogen is the limiting reactant and 4.15 g of ammonia are produced.
D)Hydrogen is the limiting reactant and 23.5 g of ammonia are produced.
E)Hydrogen is the limiting reactant and 15.8 g of ammonia are produced.

Question 37

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%

Question 38

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?

A)Calcium is the limiting reactant and 47.2 g of calcium oxide are produced
B)Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced
C)Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced
D)Calcium is the limiting reactant and 23.6 g of calcium oxide are produced

Question 39

The first step in the Ostwald process for producing nitric acid is as follows: 4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g). If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction?

A)29.0%
B)32.9%
C)49.5%
D)61.8%
E)77.3%

Question 40

What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr₂O₃ with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr₂O₃ → Al₂O₃ + 2Cr

A)7.7 g
B)15.4 g
C)27.4 g
D)30.8 g
E)49.9 g

Question 41

What volume of CO₂ gas at 645 torr and 800.K could be produced by the decomposition of 45.0 g of CaCO₃? CaCO₃(s) → CaO(s) + CO₂(g) (R = 0.08206 L • atm/K • mol)

A)0.449 L
B)22.4 L
C)25.0 L
D)34.8 L
E)45.7 mL

Question 42

Magnesium metal (0.100 mol) and hydrochloric acid (0.500 mol HCl) are combined and react to completion.What volume of hydrogen gas, measured at STP, is produced? Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) (R = 0.08206 L • atm/K • mol)

A)2.24 L of H₂
B)4.48 L of H₂
C)5.60 L of H₂
D)11.2 L of H₂
E)22.4 L of H₂

Question 43

Given that CaO(s) + H₂O(l) → Ca(OH)₂(s), heat of reaction = −64.8 kJ/mol, how many grams of CaO must react in order to liberate 525 kJ of heat?

A)6.92 g
B)56.1 g
C)454 g
D)606 g
E)3.40× 10⁴ g

Question 44

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)

A)24.6 g
B)70.8 g
C)272 g
D)408 g
E)612 g

Question 45

What volume of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO₂ in excess HCl(aq)? MnO₂(s) + 4HCl(aq) → MnCl₂(aq) + 2H₂O(l) + Cl₂(g) (R = 0.08206 L • atm/K • mol)

A)5.36 × 10⁻³ L
B)0.138 L
C)0.282 L
D)3.09 L
E)3.55 L

Question 46

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)

A)52.2 mL
B)26.1 mL
C)55.4 mL
D)27.7 mL
E)13.8 mL

Question 47

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)

A)2.39 L
B)0.556 L
C)0.864 L
D)4.22 L
E)3.58 L

Question 48

What volume of 0.200 M H₂SO₄ solution is required to react exactly with 50.0 mL of 0.100 M KOH? H₂SO₄(aq) + 2KOH(aq) → 2H₂O(l) + K₂SO₄(aq)

A)62.5 mL
B)12.5 mL
C)50.0 mL
D)25.0 mL
E)75.0 mL

Question 49

When active metals such as magnesium are immersed in acid solution, hydrogen gas is evolved.Calculate the volume of H₂(g) at 30.1°C and 0.85 atm that can be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride. Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) (R = 0.08206 L • atm/K • mol)

A)3.4 × 10⁻³ L
B)2.2 L
C)2.9 L
D)5.8 L
E)11.7 L

Question 50

How much heat is evolved if 0.600 kg of SO₂ is burned in excess oxygen? 2SO₂(g) + O₂(g) → 2SO₃(g) heat of reaction = −198 kJ/mol

A)5.46 × 10⁻² kJ
B)927 kJ
C)1.85 × 10³ kJ
D)59,400 kJ
E)3.71 × 10³ kJ

Question 51

How much heat is released if 35.0 g of ethanol (C₂H₅OH) burns in excess oxygen? C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) heat of reaction = −1367 kJ/mol

A)1797 kJ
B)1367 kJ
C)9.61 × 10⁻⁴ kJ
D)4.78 × 10⁴ kJ
E)1040 kJ

Question 52

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

Question 53

Given the following reaction, how much AgCl (in g) can be formed from 25.0 mL of 0.115 M AgNO₃ and 45.0 mL of 0.0533 M MgCl₂? 2AgNO₃(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO₃)₂(aq)

A)0.344 g
B)0.688 g
C)1.10 g
D)0.412 g
E)0.276 g

Question 54

How many milliliters of 0.0150 M KOH are required to react exactly with 75.0 mL of 0.0150 M H₃PO₄? H₃PO₄(aq) + 3KOH(aq) → K₃PO₄(aq) + 3H₂O(l)

A)25.0 mL
B)1000 mL
C)225 mL
D)250 mL
E)75.0 mL

Question 55

Calculate the volume of H₂(g) at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with 50.0 g Zn(s) to give hydrogen gas and aqueous zinc chloride. (R = 0.08206 L • atm/K • mol)

A)0.56 L
B)1.12 L
C)2.23 L
D)4.47 L
E)3.54 L

Question 56

Zinc dissolves in hydrochloric acid to yield hydrogen gas as follows: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g) What mass of hydrogen gas is produced when a 7.35-g sample of zinc dissolves in 500.mL of 1.200 M HCl?

A)0.605 g
B)0.113 g
C)0.302 g
D)0.453 g
E)0.227 g

Question 57

Consider the following reaction.H₂(g) + I₂(s) → 2 HI(g) If the cylinder with a movable piston below contains 1 mol H₂(g) and 1 mol I₂(s), which represents the cylinder after the reaction is complete?

A)
B)
C)
D)
E)None of the above

Question 58

What mass of precipitate forms when 25.0 mL of 0.147 M NiCl₂ solution reacts with excess sodium phosphate according to the given balanced chemical equation. 3NiCl₂(aq) + 2Na₃PO₄(aq) → Ni₃(PO₄)₂(s) + 6NaCl(aq)

A)0.149 g
B)0.448 g
C)1.35 g
D)0.368 g
E)0.234 g

Question 59

The combustion of pentane produces heat according to the following thermochemical equation.C₅H ₁₂(l) + 8O₂(g) → 5CO₂(g) + 6H₂O(l) heat of reaction = −3510 kJ/mol How many grams of CO₂ is produced per 2.50 × 10³ kJ of heat released?

A)6.27 g
B)31.3 g
C)61.8 g
D)157 g
E)220 g

Question 60

What is the volume of NH₃ produced in the following reaction when 3.0 L of N₂ reacts with 4.0 L of H₂ ? N₂(g) + 3H₂(g) → 2NH₃(g)

A)1.5 L
B)2.7 L
C)6.0 L
D)7.5 L
E)12 L

Question 61

The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe₂O₃(s) → 2Fe(s) + Al₂O₃(s) heat of reaction = −847.6 kJ/mol What mass of iron is formed if 725 kJ of heat are released?

A)23.9 g
B)47.8 g
C)65.3 g
D)95.5 g
E)112 g