Deck 8: Chemical Reactions and Chemical Quantities

Question 1

Determine the limiting reactant (LR)and the mass (in g)of nitrogen that can be formed from 50.0 g N₂O₄ and 45.0 g N₂H₄.Some possibly useful molar masses are as follows: N₂O₄ = 92.02 g/mol,N₂H₄ = 32.05 g/mol. N₂O₄(l)+ 2 N₂H₄(l)→ 3 N₂(g)+ 4 H₂O(g)

A) LR = N₂H₄, 59.0 g N₂ formed
B) LR = N₂O₄, 105 g N₂ formed
C) LR = N₂O₄, 45.7 g N₂ formed
D) LR = N₂H₄, 13.3 g N₂ formed
E) No LR, 45.0 g N₂ formed

Answer 1

LR = N₂O₄, 45.7 g N₂ formed

Question 2

Give the theoretical yield,in moles,of CO₂ from the reaction of 4.00 moles of C₈H₁₈ with 4.00 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A) 0.640 moles
B) 64.0 moles
C) 2.56 moles
D) 16.0 moles

Answer 2

2.56 moles

Question 3

Consider the following reaction.How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C₃H₇SH present.
C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A) 1.55 moles O₂
B) 3.50 moles O₂
C) 2.33 moles O₂
D) 4.14 moles O₂
E) 6.21 moles O₂

Answer 3

3.50 moles O₂

Question 4

Consider the following balanced reaction.What mass (in g)of CO₂ can be formed from 288 mg of O₂? Assume that there is excess C₃H₇SH present.
C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A) 0.396 g CO₂
B) 0.209 g CO₂
C) 0.792 g CO₂
D) 0.126 g CO₂
E) 0.198 g CO₂

Question 5

A physical change

A) occurs when iron rusts.
B) occurs when sugar is heated into caramel.
C) occurs when glucose is converted into energy within your cells.
D) occurs when water is evaporated.
E) occurs when propane is burned for heat.

Question 6

According to the following reaction,how many grams of sulfur are formed when 37.4 g of water are formed?
2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2H₂O(l)

A) 99.8 g S
B) 66.6 g S
C) 56.1 g S
D) 44.4 g S
E) 14.0 g S

Question 7

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol.
4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

A) 0.290 mol O₂
B) 0.580 mol O₂
C) 18.5 mol O₂
D) 0.724 mol O₂
E) 1.73 mol O₂

Question 8

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl₃).If it is the only product,what mass of PCl₃ is formed?

A) 30.15 g
B) 54.93 g
C) 140.01 g
D) 79.71 g
E) 91.86 g

Question 9

Two samples of potassium iodide are decomposed into their constituent elements.The first sample produced 13.0 g of potassium and 42.3 g of iodine.If the second sample produced 24.4 kg of potassium,how many kg of iodine were produced?

A) 13.3 kg
B) 22.5 kg
C) 79.4 kg
D) 44.4 kg
E) 92.4 kg

Question 10

Determine the theoretical yield of HCl if 60.0 g of BCl₃ and 37.5 g of H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl₃ = 117.16 g/mol. BCl₃(g)+ 3 H₂O(l)→ H₃BO₃(s)+ 3 HCl(g)

A) 75.9 g HCl
B) 132 g HCl
C) 187 g HCl
D) 56.0 g HCl
E) 25.3 g HCl

Question 11

Which of the following represents a physical property?

A) Sodium metal is extremely reactive with chlorine gas.
B) Mercury is a silvery liquid at room temperature.
C) Aluminum has a tendency to "rust."
D) Butane is highly flammable.
E) Argon has an unreactive nature.

Question 12

Two samples of calcium fluoride are decomposed into their constituent elements.The first sample produced 0.154 g of calcium and 0.146 g of fluorine.If the second sample produced 294 mg of fluorine,how many g of calcium were formed?

A) 0.280 g
B) 3.09 × 10² g
C) 3.13 g
D) 0.309 g
E) 2.80 × 10² g

Question 13

Which of the following represents a chemical property of hydrogen gas?

A) It is gaseous at room temperature.
B) It is less dense than air.
C) It reacts explosively with oxygen.
D) It is colorless.
E) It is tasteless.

Question 14

Global warming is thought to be caused by the increase of one particular gas.Name the gas.

A) oxygen
B) carbon monoxide
C) carbon dioxide
D) nitrogen
E) helium

Question 15

A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃).If ammonia is the only product,what mass of ammonia is formed?

A) 17.03 g
B) 1.10 g
C) 14.01 g
D) 3.02 g
E) 23.07 g

Question 16

Consider the following balanced reaction.How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present.The molar masses are as follows: H₂O = 18.02 g/mol,HNO₃ = 63.02 g/mol.
3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 38.0 g H₂O
B) 21.7 g H₂O
C) 43.4 g H₂O
D) 10.9 g H₂O
E) 26.5 g H₂O

Question 17

How many molecules of H₂S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO₂.
2 H₂S(g)+ SO₂(g)→ 3 S(s)+ 2H₂O(l)

A) 1.48 × 10²⁴ molecules H₂S
B) 9.89 × 10²³ molecules H₂S
C) 5.06 × 10²⁵ molecules H₂S
D) 3.17 × 10²⁵ molecules H₂S
E) 2.44 × 10²³ molecules H₂S

Question 18

How many grams of Li₃N can be formed from 1.75 moles of Li? Assume an excess of nitrogen.
6 Li(s)+ N₂(g)→ 2 Li₃N(s)

A) 18.3 g Li₃N
B) 20.3 g Li₃N
C) 58.3 g Li₃N
D) 61.0 g Li₃N
E) 15.1 g Li₃N

Question 19

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol.
4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

A) 0.290 mol N₂
B) 0.580 mol N₂
C) 18.5 mol N₂
D) 0.724 mol N₂
E) 1.73 mol N₂

Question 20

A chemical change

A) occurs when methane gas is burned.
B) occurs when paper is shredded.
C) occurs when water is vaporized.
D) occurs when salt is dissolved in water.
E) occurs when powdered lemonade is stirred into water.

Question 21

Balance the following equation. B₂H₆(g)+ O₂(g)→ B₂O₃(s)+ H₂O(g)
What is the stoichiometric coefficient for oxygen?

A) 1
B) 2
C) 3
D) 4
E) 6

Question 22

Why are the halogens among the most active nonmetals?

A) Their valence electrons are more effectively shielded.
B) All halogens have low electron affinities.
C) They all have smaller diameters than other nonmetals.
D) Their d orbitals are completely filled.
E) They only need one electron needed to attain a nobel gas configuration

Question 23

What is one of the products of a combustion reaction?

A) graphite
B) hydrogen
C) oxygen
D) heat
E) ethanol

Question 24

How many grams of the excess reagent are left over if 37.8g of Cl₂ react with 39.4 g of NaF?
Cl₂(g)+ 2 NaF(aq)→ 2 NaCl(aq)+ F₂(g)

A) 8.40 g
B) 29.4 g
C) 1.43 g
D) 12.6 g
E) 4.47 g

Question 25

Give the percent yield when 28.16 g of CO₂ are formed from the reaction of 8.000 moles of C₈H₁₈ with 4.000 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%

Question 26

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe₂O₃ react with excess Al according to the following reaction. Fe₂O₃(s)+ 2 Al(s)→ Al₂O₃(s)+ 2 Fe(s)

A) 61.03 %
B) 28.65 %
C) 57.30 %
D) 20.02 %
E) 81.93 %

Question 27

How many moles of SnCl₂ will be produced if 85.3 g of FeCl₃ is reacted with an excess of Sn for the following reaction: 2 FeCl₃(s)+ 3 Sn(s)→ 3 SnCl₂(s)+ 2 Fe(s)

A) 0.526 mol
B) 0.789 mol
C) 1.20 mol
D) 1.58 mol
E) 2.43 mol

Question 28

What is the percent yield of H₂ if 58.94g of methane yields 14.61g of H₂ for the following reaction: CH₄(g)+ 2 H₂O(g)→ 4 H₂(g)+ CO₂(g)

A) 2.017%
B) 72.88%
C) 49.21%
D) 64.29%
E) 24.47%

Question 29

What is the percent yield of C₂H₂ if 62.80g of water yields 15.38g of C₂H₂ using the following equation. CaC₂(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ C₂H₂(g)

A) 13.84%
B) 33.90%
C) 91.47%
D) 48.10%
E) 68.52%

Question 30

Which should give the most vigorous reaction when dropped in water?

A) C
B) K
C) Zn
D) Ca
E) Si

Question 31

Determine the theoretical yield of ethanol when 100.0g g of glucose is used according to the following fermentation reaction. C₆H₁₂O₆(aq)→ 2 C₂H₅OH(l)+ 2 CO₂(g)

A) 51.09g
B) 35.21g
C) 87.32g
D) 68.34g
E) 45.37g

Question 32

All of the following are examples of chemical properties EXCEPT

A) the low pH of stomach acid.
B) chlorophyll being responsible for the green color of leaves.
C) heat being given off by the burning of natural gas in a kitchen stove.
D) the rusting of an iron nail left out in the rain.
E) the ability of a drain opener to unclog a drain using sodium hydroxide.

Question 33

Give the percent yield when 28.16 g of CO₂ are formed from the reaction of 4.000 moles of C₈H₁₈ with 8.000 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%

Question 34

Give the percent yield when 28.16 g of CO₂ are formed from the reaction of 4.000 moles of C₈H₁₈ with 4.000 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

A) 20.00%
B) 25.00%
C) 50.00%
D) 12.50%

Question 35

Which should give the least vigorous reaction when dropped in water?

A) Li
B) Na
C) K
D) Rb
E) Cs

Question 36

Which one of the following halogen reaction contains a product with covalent bonds?

A) Mg(s) + F₂(g) → MgF₂(s)
B) C(s) + O₂(g) → CO₂(g)
C) 2Cu(s) + I₂(g) → 2CuI(s)
D) Br₂(l) + Cl₂(g) → 2BrCl(g)
E) V(s) + 2Cl₂(g) → VCl₄(l)

Question 37

Aluminum metal reacts with aqueous iron( III)oxide to form aqueous aluminum oxide and iron metal.What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest,whole-number stoichiometric coefficients?

A) 1
B) 2
C) 3
D) 4

Question 38

According to the following reaction,what amount of Al₂S₃ remains when 20.00 g of Al₂S₃ and 2.00 g of H₂O are reacted? A few of the molar masses are as follows: Al₂S₃ = 150.17 g/mol,H₂O = 18.02 g/mol.
Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

A) 28.33 g
B) 14.00 g
C) 8.33 g
D) 19.78 g
E) 17.22 g

Question 39

Choose the reaction that represents the combustion of C₆H₁₂O₂.

A) C₆H₁₂O₂(l) + 8 O₂(g) → 6 CO₂(g) + 6 H₂O(g)
B) Mg(s) + C₆H₁₂O₂(l) → MgC₆H₁₂O₂(aq)
C) 6 C(s) + 6 H₂(g) + O₂(g) → C₆H₁₂O₂(l)
D) C₆H₁₂O₂(l) → 6 C(s) + 6 H₂(g) + O₂(g)
E) None of the above represent the combustion of C₆H₁₂O₂.

Question 40

How many moles of PCl₅ will be produced if .331 moles of P₄ is reacted with an excess of Cl₂ using the following equation. P₄(s)+ 10 Cl₂(g)→ 4 PCl₅(g)

A) .331 mol
B) .662 mol
C) .993 mol
D) 1.324 mol
E) 1.655 mol

Question 41

How many moles of BCl₃ are needed to produce 5.00 g of HCl(aq)in the following reaction?
BCl₃(g)+ 3 H₂O(l)→ 3 HCl(aq)+ B(OH)₃(aq)

A) 0. 0457 mol
B) 0. 137 mol
C) 0.411 mol
D) 21.9 mol

Question 42

According to the following balanced reaction,how many moles of KO are required to exactly react with 4.33 moles of H₂O?
4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

A) 4.33 moles H₂O
B) 8.66 moles H₂O
C) 17.3 moles H₂O
D) 2.17 moles H₂O
E) 1.08 moles H₂O

Question 43

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: (s)→ 2Na(s)+ (g) How many moles of are produced by the decomposition of 1.25 mol of sodium azide?

A) 0.833
B) 3.75
C) 1.88
D) 0.417
E) 0.625

Question 44

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas.How many grams of oxygen are formed when 20.0 g of dinitrogen monoxide decomposes?

A) 0. 138 g
B) 7.27 g
C) 14.5 g
D) 29.1 g

Question 45

Carbonic acid can form water and carbon dioxide upon heating.How much carbon dioxide is formed from 12.4 g of carbonic acid?
H₂CO₃ → H₂O + CO₂

A) 8.80 g
B) 17.5 g
C) 12.4 g
D) 3.60 g
E) 42.7 g

Question 46

How many molecules of HCl are formed when 90.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃.
2 ICl₃ + 3 H₂O → ICl + HIO₃ + 5 HCl

A) 5.00 × 10²⁴ molecules HCl
B) 3.00 × 10²⁴ molecules HCl
C) 9.00 × 10²⁴ molecules HCl
D) 6.00 × 10²⁴ molecules HCl
E) 5.00 × 10²⁵ molecules HCl

Question 47

Balance the chemical equation given below,and determine the number of grams of MgO are needed to produce 15.0 g of Fe₂O₃. ________ MgO(s)+ ________ Fe(s)→ ________ Fe₂O₃(s)+ ________ Mg(s)

A) 0.0877 g
B) 1.26 g
C) 3.78 g
D) 11.4 g

Question 48

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ (g)→ 2MgO(s)
How many moles of are consumed when 1.90 mol of magnesium burns?

A) 0.0782
B) 1.05
C) 1.90
D) 3.80
E) 0.950

Question 49

How many grams of oxygen are formed when 5.30 moles of KOH are formed?
4 KO(s)+ 2 H₂O(l)→ 4 KOH(s)+ O₂(g)

A) 5.30 g O₂
B) 21.2 g O₂
C) 42.4 g O₂
D) 170 g O₂
E) 84.8 g O₂

Question 50

Lithium and nitrogen react to produce lithium nitride: 6Li(s)+ (g)→ N(s)
How many moles of are needed to react with 0.450 mol of lithium?

A) 2.70
B) 0.450
C) 0.150
D) 1.35
E) 0.0750

Question 51

According to the following balanced reaction,how many moles of NO are formed from 8.44 moles of NO₂ if there is plenty of water present?
3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 25.32 moles NO
B) 12.66 moles NO
C) 8.44 moles NO
D) 5.63 moles NO
E) 2.82 moles NO

Question 52

Lithium and nitrogen react to produce lithium nitride: 6Li(s)+ (g)→ N(s)
How many moles of lithium nitride are produced when 0.550 mol of lithium react in this fashion?

A) 0.183
B) 1.10
C) 0.0917
D) 1.65
E) 0.275

Question 53

If the density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 20.0 g of CO₂ according to the following chemical equation?
C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(l)

A) 8.26 mL
B) 13.3 mL
C) 26.5 mL
D) 53.1 mL

Question 54

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: (s)→ 2Na(s)+ (g) How many grams of sodium azide are required to produce 25.0 g of nitrogen?

A) 1.34
B) 0.595
C) 58.0
D) 38.7
E) 87.0

Question 55

Consider the following reaction.How many moles of oxygen are required to produce 4.00 moles of water? Assume that there is excess C₃H₇SH present.
C₃H₇SH(l)+ 6 O₂(g)→ 3 CO₂(g)+ SO₂(g)+ 4 H₂O(g)

A) 2.67 moles O₂
B) 6.00 moles O₂
C) 4.00 moles O₂
D) 16.0 moles O₂
E) 1.00 moles O₂

Question 56

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ (g)→ N(s)
How many moles of lithium are needed to produce 0.45 mol of N when the reaction is carried out in the presence of excess nitrogen?

A) 0.23
B) 1.4
C) 0.15
D) 0.30
E) 2.7

Question 57

Strontium phosphate reacts with sulfuric acid to form strontium sulfate and phosphoric acid.What is the coefficient for sulfuric acid when the equation is balanced using the lowest,whole-numbered coefficients?

A) 1
B) 2
C) 3
D) none of these

Question 58

Balance the chemical equation given below,and determine the number of moles of iodine that reacts with 20.0 g of aluminum. ________ Al(s)+ ________ I₂(s)→ ________ Al₂I₆(s)

A) 0.494 mol
B) 1.11 mol
C) 1.48 mol
D) 2.22 mol

Question 59

How many moles of CuO can be produced from 2.25 mol of Cu₂O in the following reaction?
2 Cu₂O(s)+ O₂(g)→ 4 CuO(s)

A) 1.12 mol
B) 2.25 mol
C) 4.50 mol
D) 9.00 mol

Question 60

How many grams of calcium chloride are needed to produce 5.00 g of potassium chloride?
CaCl₂(aq)+ K₂CO₃(aq)→ 2 KCl(aq)+ CaCO₃(aq)

A) 0.269 g
B) 3.72 g
C) 7.44 g
D) 14.9 g

Question 61

Determine the theoretical yield of H₂S (in moles)if 16 mol Al₂S₃ and 16 mol H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is Al₂S₃ = 150.17 g/mol. Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

A) 48 mol H₂S
B) 16 mol H₂S
C) 32 mol H₂S
D) 24 mol H₂S
E) 8.0 mol H₂S

Question 62

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

A) 14.04 g
B) 17.94 g
C) 30.42 g
D) 31.98 g

Question 63

When 14.0 g of calcium metal is reacted with water,5.00 g of calcium hydroxide is produced.Using the following balanced equation,calculate the percent yield for the reaction?
Ca(s)+ 2 H₂O(l)→ Ca(OH)₂(aq)+ H₂(g)

A) 9.67%
B) 19.3%
C) 35.7%
D) 66.0%

Question 64

Describe the greenhouse effect.

Question 65

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

A) 8.61 g
B) 9.40 g
C) 12.1 g
D) 18.8 g

Question 66

Balance the following equation.
________ C₁₀H₁₂ + ________ O₂ → ________ H₂O + ________ CO₂

Question 67

Which substance is the limiting reactant when 8.0 g of sulfur reacts with 12 g of oxygen and 16 g of sodium hydroxide according to the following chemical equation: 2 S(s)+ 3 O₂(g)+ 4 NaOH(aq)→ 2 Na₂SO₄(aq)+ 2 H₂O(l)

A) S(s)
B) O₂(g)
C) NaOH(aq)
D) None of these substances is the limiting reactant.

Question 68

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ (g)→ N(s)
In a particular experiment,1.00-g samples of each reagent are reacted.The theoretical yield of lithium nitride is ________ g.

A) 1.01
B) 0.84
C) 5.0
D) 1.67
E) 2.50

Question 69

If the percent yield for the following reaction is 75.0%,and 25.0 g of NO₂ are consumed in the reaction,how many grams of nitric acid,HNO₃(aq)are produced?
3 NO₂(g)+ H₂O(l)→ 2 HNO₃(aq)+ NO(g)

A) 17.1 g
B) 22.8 g
C) 30.4 g
D) 38.5 g

Question 70

8.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below.Which one of the following statements is FALSE?
N₂(g)+ 3 H₂(g)→ 2 NH₃(g)

A) 3.3 g of hydrogen are left over.
B) Hydrogen is the excess reactant.
C) Nitrogen is the limiting reactant.
D) The theoretical yield of ammonia is 15 g.

Question 71

If 588 grams of FeS₂ is allowed to react with 352 grams of O₂ according to the following unbalanced equation,how many grams of Fe₂O₃ are produced?
FeS₂ + O₂ → Fe₂O₃ + SO₂

Question 72

9.0 g of iron is reacted with 9.0 g of water according to the chemical equation shown below.Which one of the following statements is FALSE?
3 Fe(s)+ 4 H₂O(l)→ Fe₃O₄(s)+ 4 H₂(g)

A) 12.4 g of Fe₃O₄ are produced.
B) 5.13 g of H₂O are left over.
C) Mass is conserved in this reaction.
D) Water is the limiting reactant.

Question 73

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ O(l)→ (s)
A 5.00-g sample of CaO is reacted with 4.83 g of O.How many grams of water remain after the reaction is complete?

A) 0.00
B) 0.00991
C) 3.22
D) 1.04
E) 0.179

Question 74

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s)+ O(l)→ (s)
In a particular experiment,a 5.50-g sample of CaO is reacted with excess water and 6.77 g of is recovered.What is the percent yield in this experiment?

A) 123
B) 1.23
C) 7.91
D) 93.1
E) 81.3

Question 75

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ (g)→ 2MgO(s)
When 3.00 g of magnesium burns,the theoretical yield of magnesium oxide is ________ g.

A) 3.00
B) 4.98
C) 0.123
D) 2.49
E) 10.0

Question 76

Balance the following equation.
________ C₉H₂₀ + ________ O₂ → ________ H₂O + ________ CO₂

Question 77

Define a limiting reagent.

Question 78

When 8.00 × 10²² molecules of ammonia react with 7.00 × 10²² molecules of oxygen according to the chemical equation shown below,how many grams of nitrogen gas are produced?
4 NH₃(g)+ 3 O₂(g)→ 2 N₂(g)+ 6 H₂O(g)

A) 1.86 g
B) 2.17 g
C) 4.88 g
D) 7.44 g

Question 79

If the percent yield for the following reaction is 65.0%,how many grams of KClO₃ are needed to produce 42.0 g of O₂?
2 KClO₃(s)→ 2 KCl(s)+ 3 O₂(g)

A) 69.7 g
B) 107 g
C) 165 g
D) 371 g