Deck 4: Stoichiometry

Question 1

A limiting reactant is completely consumed in the course of a reaction and may be used to determine how much product may be produced.

Answer 1

True

Question 2

Consider the following reaction: 4C + S₈→ 4CS₂. How much S₈ is required for the formation of 6.75 moles of CS₂?

A)15.0 moles
B)13.5 moles
C)1.69 moles
D)2.00 moles

Answer 2

1.69 moles

Question 3

If an 88.2 g charcoal briquette (assume pure carbon)is burned in an unlimited amount of oxygen, what mass of CO₂is produced by the reaction?

A)44.1 g
B)323 g
C)113.8 g
D)276 g

Answer 3

323 g

Question 4

Consider the following reaction: CH₄+ 2O₂→ CO₂+ 2H₂O. How much carbon dioxide is produced in the complete combustion of 100.0 g of methane (CH₄)?

A)6.25 moles
B)12.5 moles
C)200 moles
D)0.321 moles

Question 5

Consider the following reaction: Cl₂O₅+ H₂O →  2HClO₃. How much HClO₃ is produced from 2.5 moles of Cl₂O₅reacting with excess water?

A)1.3 moles
B)2.5 moles
C)5.0 moles
D)6.0 moles

Question 6

Consider this chemical reaction: NaClO( aq )+ HCl( aq )→ NaCl( aq )+ HClO( aq ). How many mL of 6.00 M HCl is required to neutralize 25.00 mL of 2.35 M NaClO?

A)9.79 mL
B)11.7 mL
C)63.8 mL
D)117 mL

Question 7

Nitroglycerin detonates according to the following balanced reaction: ​
4C₃H₅N₃O₉( l ) → 12CO₂( g )+ 6N₂( g )+ O₂( g )+ 10H₂O( g ).
​
If 1.00 kg of nitroglycerin is detonated, how many liters of products (assume all gases at standard temperature and pressure, so 1.00 mole = 22.4 L of volume)are released?

A)107 L
B)428 L
C)715 L
D)1000 L

Question 8

The presence of oxygenates such as MTBE in gasoline result in a more complete combustion and reduced unwanted emissions.

Question 9

Complete combustion of gasoline will yield carbon dioxide and water as the major products.

Question 10

Zinc reacts with oxygen to form ZnO. How many moles of ZnO can form from a reaction of 4.43 moles of Zn and 3.05 moles of oxygen?

A)3.05 moles
B)4.43 moles
C)6.10 moles
D)9.65 moles

Question 11

The following reaction illustrates the reaction of methanol with oxygen to form carbon dioxide and water: ​
2CH₃OH( l )+ 3O₂( g )→ 2CO₂( g )+ 4H₂O( l ).
​
How many moles of water are produced in a reaction of 15 moles of methanol with 30 moles of oxygen?

A)20 moles
B)30 moles
C)40 moles
D)50 moles

Question 12

How many moles of aluminum oxide can form if 26.2 moles of Al metal react with an unlimited amount of oxygen?

A)26.2 moles
B)3.28 moles
C)13.1 moles
D)4.91 moles

Question 13

Consider this chemical reaction: Sn + NaOH → Na ₂ SnO ₂ + H ₂ . How many moles of hydrogen are liberated from the complete reaction of 3.47 × 10 ⁴ kg of tin metal in excess sodium hydroxide?

A)3.47 × 10⁷ moles
B)8.15 × 10⁷ moles
C)2.47 × 10⁶ moles
D)2.92 × 10⁵ moles

Question 14

In alkanes, carbon atoms are linked with each other by single bonds.

Question 15

Consider the following reaction: 3NO₂( g )+ H₂O( l ) → 2HNO₃( aq )+ NO( g ). What quantity (L)of NO₂is required to completely react with 125 g of water? Assume that the gases are at standard temperature and pressure; hence, 1.00 mole occupies 22.4 L of volume.

A)466 L
B)155 L
C)311 L
D)4.82 L

Question 16

Methane is the major component by weight in gasoline.

Question 17

An SUV features a 60 L gas tank. Assuming complete combustion and a molecular formula of C ₈ H ₁₈ for gasoline, approximately what amount of oxygen is consumed per tank of gasoline. Assume a density of 0.78 g\mL for gasoline.

A)3,240 L
B)10,600 L
C)54,900 L
D)110,000 L

Question 18

Sulfuric acid can be manufactured using the following reaction: ​
2S( s )+ 3O₂( g )+ 2H₂O( l )→ 2H₂SO₄( aq ).
​
If a manufacturing site consumes 65 metric tons (1 metric ton = 1000 kg)of sulfur with unlimited access to O₂and H₂O, how many metric tons of sulfuric acid may be produced?

A)165 metric tons
B)233 metric tons
C)199 metric tons
D)117 metric tons

Question 19

Consider the reaction between NaCl and AgNO₃to form silver chloride. How much of the insoluble precipitate will be recovered if 582.4 g of AgNO₃reacts with excess NaCl?

A)432.25 g
B)291.4 g
C)257.3 g
D)472.83 g

Question 20

If 4.21 × 10 ^{− 3}moles of Ca²⁺react with excess PO₄^{3 −} to form calcium phosphate, how many moles of the solid can form?

A)3.04 × 10 ^{− 2} moles
B)6.74 × 10 ^{− 3} moles
C)1.40 × 10 ^{− 3} moles
D)4.21 × 10 ^{− 3} moles

Question 21

If 2.5 moles of each of these compounds are burned completely in O₂, which will produce the largest amount of CO₂?

A)C₂H₅OH
B)CH₄
C)C₂H₆
D)C₃H₈

Question 22

The titration of 25.00 mL of 0.2215 M HCl required 28.84 mL of NaOH for neutralization. What is the molarity of NaOH?

A)0.2555 M
B)0.03255 M
C)4.004 M
D)0.1920 M

Question 23

If liquid mercury and oxygen combine to make mercury(II)oxide, what is the percentage yield of HgO if 350.0 g of Hg( l )react with 150.0 g of O₂( g )to produce 272.3 g of the product?

A)72.07%
B)44.03%
C)13.39%
D)66.76%

Question 24

Ammonia is manufactured using the following reaction: ​
N₂+ 3H₂→ 2NH₃.
​
How much ammonia can be produced in the reaction of 2.04 × 10 ^{− 3}moles of nitrogen and 6.83 × 10 ^{− 3}moles of hydrogen?

A)4.08 × 10 ^{− 3}moles
B)5.20 × 10 ^{− 3}moles
C)6.83 × 10 ^{− 3}moles
D)7.47 × 10 ^{− 3}moles

Question 25

If 15.00 mL of a 1.00 M HCl solution is mixed with 25.00 mL of a 0.250 M NaOH solution in a process that produces 273 mg of NaCl, what is the percentage yield of NaCl?

A)19.8%
B)37.7%
C)60.0%
D)74.8%

Question 26

If 92.8 g of sodium nitrite is dissolved in 2.3 L of water, the resulting solution has a molarity of:

A)1.3 M.
B)0.89 M.
C)0.58 M.
D)1.9 M.

Question 27

If 8.42 × 10 ^{− 2}moles of aluminum react with 1.77 × 10 ^{− 2}moles of chlorine gas, how many moles of AlCl₃ can form?

A)6.50 × 10 ^{− 2}
B)8.42 × 10 ^{− 2}
C)1.77 × 10 ^{− 2}
D)1.18 × 10 ^{− 2}

Question 28

If 60.6 g of aluminum powder reacts with 125 g of iron(III)oxide, how much iron metal can be recovered?

A)124.8 g
B)93.7 g
C)87.4 g
D)104.9 g

Question 29

An ethanol plant begins a production run with sufficient reactants and predicts a theoretical yield of 1250 metric tons of ethanol. The process produces 1178.6 metric tons. What is the percentage yield for this production run?

A)94.29%
B)82.10%
C)106.1%
D)99.23%

Question 30

A 118.63 g of SrCl₂∙ 6H₂O was heated and 34.81 g of water was recovered from the sample. What percent of the original H₂O remains in the sample following this heating process?

A)27.61%
B)38.15%
C)72.38%
D)86.19%

Question 31

A meat preservation technique requires sodium nitrite. The preservative is prepared by streaming NO( g )and O₂( g )through Na₂CO₃( aq )as seen in the reaction below . What is the percentage yield for this reaction if the addition of 12.73 g of NO( g ), 16.49 g of O₂( g ), and 35.82 g of Na₂CO₃( aq )result in the formation of 16.81 g of NaNO₂. ​
NO( g )+ O₂( g )+ Na₂CO₃( aq )→ NaNO₂( aq )+ CO₂( g )

A)57.43%
B)49.51%
C)58.50%
D)70.28%

Question 32

A 25.00 mL sample of vinegar is titrated to neutralization with 22.64 mL of 2.00 M NaOH. What is the molarity of the vinegar?

A)1.66 M
B)2.21 M
C)2.83 M
D)1.81 M

Question 33

A series of ant bites inject 45 μ g of formic acid (HCOOH)into a patient's skin. Considering formic acid is a monoprotic acid (donates one H⁺), how much baking soda (NaHCO₃)is required to neutralize the acid?

A)458 μ g
B)54 μ g
C)135 μ g
D)82 μ g

Question 34

Limestone (CaCO₃)emits CO₂gas when exposed to HCl as shown in the reaction below . What is the theoretical yield of CO₂if 9.45 g of limestone is completely dissolved in HCl? ​
CaCO₃( s )+ 2HCl( aq )→ CaCl₂( aq )+ CO₂( g )+ H₂O( l )

A)21.5 g
B)4.16 g
C)9.53 g
D)24.7 g

Question 35

During a tuning test, an automobile engine consumes 4.40 × 10 ^{− 3}moles of octane and 5.50 × 10 ^{− 2}moles of oxygen. What condition best describes the fuel mix?

A)too lean (too much oxygen)
B)reasonably correct
C)too rich (too little oxygen)

Question 36

A 2.0 L vessel is filled with 7.3 × 10 ^{− 4}moles of hydrogen and 6.8 × 10 ^{− 4}moles of oxygen. How much water can be produced?

A)7.3 × 10 ^{− 4}moles
B)1.4 × 10 ^{− 3}moles
C)3.7 × 10 ^{− 4}moles
D)6.6 × 10 ^{− 3}moles

Question 37

Phosgene is produced in the reaction of carbon monoxide with chlorine gas in the following reaction: ​
CO( g )+ Cl₂( g )→ COCl₂( g ).
​
What is the theoretical yield of phosgene if 0.767 moles of CO react with excess Cl₂gas?

A)76.0 g
B)1.8 × 10 ^{− 2}g
C)31.9 g
D)210 mg

Question 38

The Haber process is used to synthesize ammonia from hydrogen and nitrogen. How much hydrogen gas is required to produce 42.8 kg of ammonia?

A)5.02 kg
B)4.8 kg
C)2.25 kg
D)3.8 kg

Question 39

What is the theoretical yield of AgCl if 30.2 mL of 0.1000 M AgNO₃reacts with an excess of 0.10000 M HCl?

A)220 mg
B)433 mg
C)43.8 mg
D)915 mg

Question 40

Automobile airbags employ a chemical reaction involving the rapid decomposition of sodium azide (NaN₃)into sodium metal and nitrogen gas to inflate in a collision. How much sodium azide is required to decompose to inflate a 20.0 L air bag? Assume that the gas is at standard temperature and pressure, and thus occupies 22.4 L per mole.

A)76.3 g
B)42.8 g
C)38.7 g
D)62.7 g

Question 41

If 10 g of hydrogen gas reacts with 50 g of oxygen gas to produce water, it is evident that the oxygen gas is the limiting reactant.

Question 42

The reactant that is in excess in a chemical reaction is called the limiting reactant .

Question 43

What is the percentage yield of potassium nitrate if 100 g of nitric acid reacts with 100 g of potassium hydroxide to produce 140 g of potassium nitrate ?

A)87.25%
B)90.36%
C)12.75%
D)9.64%

Question 44

If 30 mL of 0.625 M NaOH solution is used to titrate a 20 mL sample of sulfuric acid, H ₂ SO ₄ , what is the concentration of the acid?

A)0.63 M
B)0.58 M
C)0.47 M
D)0.39 M

Question 45

How much zinc sulfate is formed if 200 g of zinc chloride reacts with 250 g of copper sulfate ?

A)1.56 moles
B)1.46 moles
C)1.75 moles
D)1.85 moles