Deck 9: Chemical Quantities

Question 1

Consider the following reaction, where X represents an unknown element: 6X(s) + 2B₂O₃(s) B₄X₃(s) + 3XO₂(g)
If 165 grams of X reacts completely with diboron trioxide to produce 2.29 mol of B₄X₃, what is the identity of X?

A) C
B) Mg
C) Ge
D) Si
E) N

Answer 1

C

Question 2

Refer to the following equation: How many molecules of NO₂ are produced when 5.38 mol of ammonia is completely reacted?

A) 21.52
B)
C)
D) 247
E) none of these

Answer 2

Question 3

What mass of carbon dioxide will be produced when 29.9 g of butane reacts with an excess of oxygen in the following reaction?

A) 181.1 g CO₂
B) 90.6 g CO₂
C) 11.32 g CO₂
D) 119.6 g CO₂
E) none of these

Answer 3

90.6 g CO₂

Question 4

Refer to the following unbalanced equation: What mass of oxygen (O₂) is required to react completely with 11.7 g of C₆H₁₄?

A) g
B) 20.6 g
C) 4.34 g
D) 41.3 g
E) 0.136 g

Question 5

Calculate the mass of water produced when 9.47 g of methane, CH₄, reacts with an excess of oxygen in the following unbalanced reaction.

A) 10.64 g H₂O
B) g H₂O
C) 21.3 g H₂O
D) 0.526 g H₂O
E) 1.18 g H₂O

Question 6

The balanced equation tells us that 5.0 mol H₂

A) reacts with 2.5 mol P₄
B) produces 10.0 mol PH₃
C) cannot react with phosphorus
D) produces 3.3 mol PH₃
E) reacts with 5.0 mol P₄

Question 7

For the reaction if 5.5 mol of CO₂ are produced, how many moles of O₂ were reacted?

A) 3.6 mol
B) 6.8 mol
C) 8.2 mol
D) 13.7 mol
E) none of these

Question 8

The rusting of iron is represented by the equation . If you have a 1.45-mol sample of iron, how many moles of Fe₂O₃ will there be after the iron has rusted completely?

A) 0.483 mol
B) 0.725 mol
C) 0.97 mol
D) 1.45 mol
E) 2.18 mol

Question 9

The equation can be interpreted by saying that 1 mol of N₂ reacts with 3 mol of H₂ to form 2 mol of NH₃.

Question 10

Refer to the following unbalanced equation: What mass of carbon dioxide (CO₂) can be produced from 25.0 g of C₆H₁₄ and excess oxygen?

A) g
B) 12.8 g
C) 76.6 g
D) 38.3 g
E) 0.290 g

Question 11

Refer to the following equation: How many moles of ammonia will be required to produce 11.9 mol of water?

A) 4.76 mol
B) 11.9 mol
C) 7.93 mol
D) 5.95 mol
E) none of these

Question 12

A 3.1-mol sample of KClO₃ was decomposed according to the equation How many moles of O₂ are formed assuming 100% yield?

A) 2.1 mol
B) 2.6 mol
C) 3.1 mol
D) 1.6 mol
E) 4.7 mol

Question 13

The balanced equation tells us that 4.0 mol of Cu

A) reacts with 4.0 mol of O₂
B) produces 4.0 mol of CuO
C) must react with 128 g of O₂
D) cannot react with oxygen
E) produces 8.0 mol of CuO

Question 14

An excess of Al and 7.9 mol of Br₂ are reacted according to the equation How many moles of AlBr₃ will be formed assuming 100% yield?

A) 2.6 mol
B) 4.0 mol
C) 5.3 mol
D) 7.9 mol
E) 11.9 mol

Question 15

A mole ratio is used to convert the moles of a starting substance to the moles of a desired substance.

Question 16

How many molecules of carbon dioxide will be formed if 2.21 g of propane is burned in the following reaction?

A) molecules
B) molecules
C) molecules
D) molecules
E) molecules

Question 17

A balanced chemical equation is one that has the same number of moles of molecules on each side of the equation.

Question 18

Which of the following reaction mixtures would produce the greatest amount of product, assuming all went to completion? Each involves the reaction symbolized by the equation

A) 3 moles of N₂ and 3 moles of H₂
B) 1 mole of N₂ and 6 moles of H₂
C) 5 moles of N₂ and 3 moles of H₂
D) 1 mole of N₂ and 3 moles of H₂
E) All would produce the same amount of product.

Question 19

Refer to the following equation: How many molecules of water are produced if 9.12 mol of NO₂ is given off?

A)
B)
C) 164.2
D)
E) none of these

Question 20

In the reaction how many moles of ammonia would be produced from 1.21 mol of hydrogen and excess nitrogen?

A) 1.57 mol
B) 3.63 mol
C) 0.807 mol
D) 2.42 mol
E) 0.403 mol

Question 21

Calculate the molecules of oxygen required to react with 25.0 g of sulfur in the following reaction.

A)
B)
C)
D)
E)

Question 22

In the reaction how many grams of sodium chloride can be produced from 37.2 g of NaOH?

A) 45.3 g NaCl
B) 65.2 g NaCl
C) 54.4 g NaCl
D) 21.2 g NaCl
E) 14.0 g NaCl

Question 23

When 3.4 mol of Fe reacts with Cl₂ according to the equation how many moles of Cl₂ are required to react with all of the iron?

A) 2.3 mol
B) 3.4 mol
C) 5.1 mol
D) 0.9 mol
E) none of these

Question 24

How many atoms of aluminum can be produced by the decomposition of 31.5 g of Al₂O₃? (Hint: Write and balance the equation first.)

A)
B)
C)
D)
E) none of these

Question 25

For the reaction how many moles of SO₃ will be produced from 2.2 mol O₂ and excess S?

A) 3.3 mol SO₃
B) 1.5 mol SO₃
C) 2.2 mol SO₃
D) 0.7 mol SO₃
E) none of these

Question 26

If 19.2 g of CO₂ is produced in the reaction of C₂H₂ with O₂ to form CO₂ and H₂O, how many grams of H₂O are produced in this reaction?

A) 7.86 g
B) 3.93 g
C) 15.7 g
D) 2.62 g
E) none of these

Question 27

In the reaction how many molecules of water can be produced starting with 19.8 kilograms of sodium hydroxide and excess Cl₂?

A)
B)
C)
D)
E) none of these

Question 28

Nitrogen and hydrogen gases are combined at high temperatures and pressures to produce ammonia, NH₃. If 104.7 g of N₂ are reacted with excess H₂, how many moles of NH₃ will be formed?

A) 3.737 mol
B) 2.491 mol
C) 7.473 mol
D) 5.605 mol
E) none of these

Question 29

For the reaction how many moles of SO₃ can be produced from 7.2 g O₂ and excess S?

A) 0.30 mol SO₃
B) 4.8 mol SO₃
C) 0.15 mol SO₃
D) 0.34 mol SO₃
E) none of these

Question 30

Consider the reaction If 11.9 g of iron(III) oxide (rust) is produced from a certain amount of iron, how many grams of oxygen are needed for this reaction?

A) 3.58 g
B) 7.15 g
C) 1.59 g
D) 2.38 g
E) none of these

Question 31

Calculate the mass of carbon dioxide produced from 22.3 g of octane, C₈H₁₈, in the following reaction.

A) 68.7 g CO₂
B) 137 g CO₂
C) 77.3 g CO₂
D) 1.074 g CO₂
E) 1.562 g CO₂

Question 32

In the reaction what number of grams of silver can be produced from the reaction of 55.0 g of copper?

A) 187 g Ag
B) 93.4 g Ag
C) 46.7 g Ag
D) 64.8 g Ag
E) 0.87 g Ag

Question 33

For the reaction how many grams of CaCl₂ can be obtained if 14.6 g HCl is allowed to react with excess CaCO₃?

A) 44 g CaCl₂
B) 89 g CaCl₂
C) 0.200 g CaCl₂
D) 22.2 g CaCl₂
E) none of these

Question 34

Methane, CH₄, the major component of natural gas, burns in air to form CO₂ and H₂O. What mass of water is formed in the complete combustion of 7.07 *10³ g of CH₄?

A)
B)
C)
D)
E) none of these

Question 35

How many moles of O₂ are required for the complete reaction of 43.5 g of C₂H₄ to form CO₂ and H₂O?

A) 0.775 mol
B) 3.10 mol
C) 6.20 mol
D) 4.65 mol
E) none of these

Question 36

How many moles of oxygen are produced by decomposing 28.5 g of H₂O₂ (molar mass = 34.0 g/mol) according to the equation:

A) 0.838 mol O₂
B) 485 mol O₂
C) 0.419 mol O₂
D) 1.68 mol O₂
E) none of these

Question 37

In the reaction how many molecules of hydrogen are required to react with 3.66 g of nitrogen?

A)
B)
C)
D)
E) none of these

Question 38

For the reaction how many moles of Cl₂ are needed to react with 11.6 g NaOH?

A) 0.58 mol Cl₂
B) 0.290 mol Cl₂
C) 0.193 mol Cl₂
D) 0.073 mol Cl₂
E) 0.145 mol Cl₂

Question 39

What number of moles of ammonia can be produced from 7.46 g of hydrogen gas and excess nitrogen gas?

A) 1.233 mol NH₃
B) 7.40 mol NH₃
C) 4.93 mol NH₃
D) 5.55 mol NH₃
E) 2.47 mol NH₃

Question 40

In the reaction how many moles of chlorine molecules are needed to react with 13.3 g of NaOH?

A) 1.00 mol Cl₂
B) 0.333 mol Cl₂
C) 0.67 mol Cl₂
D) 0.166 mol Cl₂
E) none of these

Question 41

For the reaction how many molecules of H₂O can be produced from 32.7 g of NaOH and excess Cl₂?

A)
B)
C)
D)
E)

Question 42

For the reaction of C₂H₄(g) with O₂(g) to form CO₂(g) and H₂O(g), what number of moles of CO₂ can be produced by the reaction of 5.00 mol C₂H₄ and 12.1 mol O₂?

A) 18.2 mol
B) 12.1 mol
C) 8.07 mol
D) 10.0 mol
E) none of these

Question 43

For the reaction how many grams of NaCl can be produced from 19.3 g of Cl₂ and excess NaOH?

A) 23.9 g NaCl
B) 10.6 g NaCl
C) 15.9 g NaCl
D) 7.95 g NaCl
E) none of these

Question 44

Consider the reaction If 416.3 g NH₃ is reacted with excess CH₄ and O₂, what mass of HCN can be produced?

A) 660.5 g HCN
B) 1321.1 g HCN
C) 330.3 g HCN
D) 440.4 g HCN
E) none of these

Question 45

Sodium and water react according to the equation What number of moles of H₂ will be produced when 4.0 mol Na is added to 1.2 mol H₂O?

A) 0.6 mol
B) 2.4 mol
C) 2.0 mol
D) 1.2 mol
E) 8.0 mol

Question 46

For the reaction of C₂H₄(g) with O₂(g) to form CO₂(g) and H₂O(g), what number of moles of CO₂ can be produced by the reaction of 0.480 mol C₂H₄ and 1.01 mol O₂?

A) 1.52 mol
B) 0.960 mol
C) 0.673 mol
D) 1.01 mol
E) none of these

Question 47

For the reaction 45.9 g solid CaCO₃ is mixed with 51.6 g HCl. What number of grams of CO₂ will be produced?

A) 16.3 g CO₂
B) 40.4 g CO₂
C) 10.1 g CO₂
D) 31.1 g CO₂
E) 20.2 g CO₂

Question 48

For the reaction 11.9 g Cl₂ is reacted with 12.0 g NaOH. How many moles of NaCl are produced?

A) 0.300 mol NaCl
B) 0.400 mol NaCl
C) 0.150 mol NaCl
D) 0.252 mol NaCl
E) 0.225 mol NaCl

Question 49

Fe₂O₃ (molar mass = 159.7 g/mol) reacts with CO (molar mass = 28.0 g/mol) according to the equation When 470.0 g Fe₂O₃ reacts with excess CO, what number of moles of Fe (iron) is produced?

A) 8.829 mol Fe
B) 5.886 mol Fe
C) 1.472 mol Fe
D) 11.772 mol Fe
E) none of these

Question 50

For the reaction if 5.42 g of S is reacted with 10.0 g of O₂, how many grams of SO₃ will be produced?

A) 27.1 g
B) 6.77 g
C) 16.7 g
D) 13.5 g
E) none of these

Question 51

Look at the reaction below: Suppose 0.55 g of water were produced from 1.2 g of aluminum hydroxide and a certain amount of hydrochloric acid. Which of the following statements is true? Choose the best answer.

A) Aluminum hydroxide is the limiting reactant because 1.2 g of aluminum hydroxide produces 0.55 g of water.
B) Aluminum hydroxide is the limiting reactant because it has a smaller coefficient than the hydrochloric acid.
C) Aluminum hydroxide is not the limiting reactant because more than 0.55 g of water could have been produced from 1.2 g of aluminum hydroxide.
D) Aluminum hydroxide is not the limiting reactant because we are given an amount of leftover aluminum hydroxide.
E) There is not enough information given to answer this question.

Question 52

For the reaction of C₂H₄(g) with O₂(g) to form CO₂(g) and H₂O(g), what number of grams of CO₂ could be produced from 2.0 g of C₂H₄ and 5.2 g of O₂?

A) 10.7 g
B) 4.8 g
C) 7.2 g
D) 6.3 g
E) none of these

Question 53

Consider the reaction Calculate the number of grams of silane gas, SiH₄, formed when 35.9 g of Mg₂Si reacts with excess H₂O.

A) 30.1 g SiH₄
B) 10.1 g SiH₄
C) 15.0 g SiH₄
D) 19.5 g SiH₄
E) none of these

Question 54

Determine the mass of CO₂ produced when 75.5 g of CaO is reacted with 50.0 g of C according to the unbalanced equation

A) 29.6 g CO₂
B) 119 g CO₂
C) 59.3 g CO₂
D) 36.6 g CO₂
E) none of these

Question 55

Consider the reaction How many moles of excess reactant are left over if we start with 39.1 g of each reactant?

A) 0.13 mol
B) 2.04 mol
C) 1.66 mol
D) 2.17 mol
E) none of these

Question 56

How many moles of SbCl₃ is formed when 4.00 mol Sb are reacted with 4.43 mol Cl₂ according to the unbalanced equation

A) 6.65 mol SbCl₃
B) 4.43 mol SbCl₃
C) 2.95 mol SbCl₃
D) 4.00 mol SbCl₃
E) Cannot be determined based on the information given.

Question 57

Fe₃O₄ reacts with CO according to the equation If 335.2 g Fe₃O₄ is reacted with excess CO, what mass of CO₂ will be produced?

A) 63.71 g CO₂
B) 191.1 g CO₂
C) 127.42 g CO₂
D) 254.8 g CO₂
E) none of these

Question 58

Fe₃O₄ reacts with CO according to the equation If 482.3 g CO is reacted with excess Fe₃O₄, what mass of CO₂ will be produced?

A) 1515.6 g CO₂
B) 378.9 g CO₂
C) 1010.4 g CO₂
D) 568.4 g CO₂
E) 757.8 g CO₂

Question 59

Consider the equation: . If 3.0 moles of A is reacted with 6.0 moles of B, which of the following is true after the reaction is complete?

A) A is the leftover reactant because you need only 2 moles of A and have 3.
B) A is the leftover reactant because for every 1 mole of A, 4 moles of C are produced.
C) B is the leftover reactant because you have more moles of B than A.
D) B is the leftover reactant because 3 moles of B react with every 1 mole of A.
E) Neither reactant is leftover.

Question 60

Fe₂O₃ (molar mass = 159.7 g/mol) reacts with CO (molar mass = 28.0 g/mol) according to the equation When 185.5 g of CO reacts with excess Fe₂O₃, how many moles of Fe (iron) will be produced?

A) 13.25 mol Fe
B) 2.208 mol Fe
C) 4.415 mol Fe
D) 9.93 mol Fe
E) 3.311 mol Fe

Question 61

Consider a reaction in which two reactants make one product (for example, consider the unbalanced reaction ). You know the following: 2.0 mol A (with an excess of B) can produce a maximum of 2.0 mol C
3)0 mol B (with an excess of A) can produce a maximum of 4.0 mol C
If you react 2.0 mol A with 3.0 mol B, what is the maximum amount of C that can be produced?

A) 2.0 mol
B) 4.0 mol
C) 5.0 mol
D) 6.0 mol
E) More information is needed to answer this question.

Question 62

Consider the equation: A + 4B 3C + 3D When equal masses of A and B are reacted, which is limiting?

A) If the molar mass of A is less than the molar mass of B, then B must be limiting.
B) If the molar mass of A is greater than the molar mass of B, then A must be limiting.
C) If the molar mass of A is greater than the molar mass of B, then B must be limiting.
D) If the molar mass of A is less than the molar mass of B, then A must be limiting.
E) Neither reactant is limiting.

Question 63

Consider the following unbalanced equation: If 1.86 g of ethanol reacts with 14.3 g of oxygen, how many moles of water are produced?

A) 0.0404 mol
B) 0.121 mol
C) 0.0135 mol
D) 0.447 mol
E) 0.894 mol

Question 64

Consider the following reaction at 1.10 atm and 19^°C: 0.228 mol of sodium chloride, 3.03 L of ammonia, 2.00 L of carbon dioxide, and an unlimited amount of water react to form aqueous ammonium chloride and solid sodium bicarbonate. How many moles of ammonium chloride are formed in the reaction?

A) 0.139 mol
B) 0.278 mol
C) 0.228 mol
D) 6.06 mol
E) 0.0918 mol

Question 65

Consider the equation: . The molar mass of B is 50.0 g/mol. Which of the following statements is true when equal masses of A and B are reacted?

A) If the molar mass of A is greater than the molar mass of B, then A must determine how much C is produced.
B) If the molar mass of A is less than the molar mass of B, then A must determine how much C is produced.
C) If the molar mass of A is the same as the molar mass of B, then A and B react in a perfect stoichiometric ratio and both determine how much C is produced.
D) If the molar mass of A is greater than the molar mass of B, then B must determine how much C is produced.
E) If the molar mass of A is less than the molar mass of B, then B must determine how much C is produced.

Question 66

Consider the following unbalanced equation: How many grams of sodium are required to completely react with 0.300 mol Na₂SiF₆?

A) 0.300 g
B) 1.20 g
C) 1.72 g
D) 6.90 g
E) 27.6 g

Question 67

Which of the following statements is always true concerning a reaction represented by the following balanced chemical equation?

A) If we have equal masses of C₂H₆ and O₂, there is no limiting reactant.
B) If we have an equal number of moles of C₂H₆ and O₂, there is no limiting reactant.
C) If we have more mass of C₂H₆, then O₂ must be the limiting reactant.
D) If we have more mass of O₂, then C₂H₆ must be the limiting reactant.
E) None of these statements (a-d) are true.

Question 68

For the titration of sulfuric acid (H₂SO₄) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

A) 0.750 mol
B) 0.375 mol
C) 1.50 mol
D) 3.00 mol
E) none of these

Question 69

When 10.0 mol of calcium metal is reacted with 3.9 mol of oxygen gas, how much calcium oxide is produced?

A) 3.9 mol
B) 10.0 mol
C) 7.8 mol
D) 20.0 mol
E) 2.0 mol

Question 70

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 5.66 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of oxygen left over after the reaction is complete.

A) 2.83 mol O₂
B) 1.66 mol O₂
C) 1.17 mol O₂
D) 4.00 mol O₂
E) none of these

Question 71

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.17 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium left over after the reaction is complete.

A) 1.83 mol Ca
B) 0.00 mol Ca
C) 3.09 mol Ca
D) 2.06 mol Ca
E) none of these

Question 72

Consider the following unbalanced equation: If 3.09 moles of Si were produced, how many moles of NaF were also created?

A) 0.515 mol
B) 3.09 mol
C) 2.06 mol
D) 18.5 mol
E) Impossible to determine without the moles of reactants.

Question 73

In the reaction between CO and Fe₃O₄, the theoretical yield in an experiment is calculated to be 47.2 g Fe. When a careless chemistry student carries out the experiment, the actual yield is 37.0 g Fe. Calculate the percentage yield.

A) 78.4%
B) 21.6%
C) 52.3%
D) 39.2%
E) none of these

Question 74

Equal masses of hydrogen gas and oxygen gas are reacted to form water. Which substance is limiting?

Question 75

Consider the following unbalanced equation: If 1.70 g of ethanol reacts with 11.2 g of oxygen, how many moles of carbon dioxide are produced?

A) 0.0369 mol
B) 0.233 mol
C) 0.0738 mol
D) 0.350 mol
E) 0.0185 mol

Question 76

Consider that calcium metal reacts with oxygen gas in the air to form calcium oxide. Suppose we react 6.02 mol calcium with 4.00 mol oxygen gas. Determine the number of moles of calcium oxide produced after the reaction is complete.

A) 6.02 mol CaO
B) 3.01 mol CaO
C) 4.01 mol CaO
D) 8.00 mol CaO
E) none of these

Question 77

Ammonia reacts with oxygen to form nitrogen dioxide and water according to the following equation: You react ammonia and oxygen, and at the end of the experiment you find that you produced 23.0 g of water and have 8.52 g of ammonia left over. Determine the mass of oxygen reacted.

A) 35.0 g O₂
B) 17.7 g O₂
C) 40.9 g O₂
D) 71.5 g O₂
E) 47.7 g O₂

Question 78

You react 25.0 g hydrogen gas with 73.7 g oxygen gas. Determine the mass of water that can be produced from these reactants.

A) 41.49 g H₂O
B) 20.7 g H₂O
C) 9.3 g H₂O
D) 83.0 g H₂O
E) 223 g H₂O

Question 79

Consider the reaction of magnesium metal with hydrochloric acid to produce magnesium chloride and hydrogen gas. If 4.52 mol of magnesium and 4.52 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are produced?

A) 9.04 mol
B) 2.26 mol
C) 4.52 mol
D) 6.52 mol
E) none of these

Question 80

Reacting 3.00 mol nitrogen gas with 3.50 mol hydrogen gas will produce how many moles of ammonia according to the following balanced chemical equation?

A) 3.50 mol NH₃
B) 5.25 mol NH₃
C) 2.33 mol NH₃
D) 7.00 mol NH₃
E) 6.00 mol NH₃