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Stoichiometry Practice Test

Total questions: 100

Worksheet time: 6hrs 46mins

Name
Class
Date
1.

How many moles of water will be produced from 6.5 moles of octane?

a)mol H2O
b)mol C8H18
1
2
1)
2)
2.

Solid zinc oxide (ZnO) is added to hydrochloric acid (HCl) to form zinc chloride (ZnCl2) in water. How many moles of zinc chloride will be produced when 112 grams of zinc oxide is used?

ZnO + 2HCl --> ZnCl2 + H2O

a)

1.38 moles

b)

3.07 moles

c)

56.0 moles

d)

112 moles

3.

A student burns 1.50 mol C3H8 according to the following reaction:
C3​H8​ + 5O2​ → 3CO2​ + 4H2​O
How many grams of carbon dioxide are produced?

a)

44 g

b)

66 g

c)

132 g

d)

198 g

4.

Antimony is burned in oxygen to form antimony oxide.

4 Sb + 3 O2→2Sb2O3

How many moles of Sb2O3 will be formed when you have 20.0 moles of oxygen gas?

a)

10 moles

b)

13.3 moles

c)

15.5 moles

d)

40.8 moles

5.

Potassium chlorate decomposed into potassium chloride and oxygen gas.

2KClO3 → 2 KCl + 3O2

How many grams of oxygen gas will be given off from 50.0 grams of potassium chlorate?

a)

9.84 g

b)

19.7 g

c)

33.3 g

d)

75.0 g

6.

Nitrogen and hydrogen react to produce ammonia.

N2​(g) + 3H2​(g) → 2NH3​(g)

How many grams of hydrogen are needed to produce 15.0 mol of ammonia if the reaction goes to completion?

a)

15.0 g

b)

22.5 g

c)

45.0 g

d)

90.0 g

7.

In 1860, Robert Boyle was the first to use phosphorus to ignite sulfur-tipped wooden splints that gave rise to our modern matches. One of the ways it can be made involves the chemical reaction of calcium phosphate with carbon and silicon dioxide in a furnace:

2Ca3(PO4)2 + 6SiO2 + 10C → 6CaSiO3 + P4 + 10CO


If you use 100.0 grams of calcium phosphate and an excess of silicon dioxide and carbon, how many moles of phosphorus will be produced?

a)

0.1612 moles

b)

0.3224 moles

c)

15510 moles

d)

1.551 moles

8.

3Cl2 + 6NaOH --> 5NaCl + NaClO3 + 3H2O

What is the mole ratio of chlorine (Cl2) to sodium hydroxide (NaOH)?

a)

1:2

b)

1:3

c)

2:3

d)

6:3

9.

A tank contains 2.46 moles of propane gas. If the whole amount of gas reacts with a sufficient amount of oxygen gas, how many grams of water will be produced?

C3H8 + 5O2 --> 3CO2 + 4H2O

a)

9.84 g

b)

12.3 g

c)

177 g

d)

221 g

10.

How many moles of sodium oxide (Na2O) would be produced from 174 g of sodium?

a)23 g Na
b)1 mole Na
c)10 mole Na
d)6 moles Na2O
e)2 mole Na
f)174 g Na
1
2
3
4
1)
2)
3)
4)
11.

What would be the mass of aluminum aluminum sulfide (Al2S3) produced from 8 moles of aluminum?

16Al + 3S8 --> 8 Al2S3

a)16 mol Al
b)8 mol Al2S3
c)1 mol Al2S3
d)150 g Al2S3
e)27 g Al
f)2 mol Al
1
2
3
4
1)
2)
3)
4)
12.

How many moles of carbon dioxide would be produced from 156 g of benzene?

2C6H6 + 15O2 --> 12CO2 + 6H2O

a)78 g C6H6
b)1 mol C6H6
c)2 mol C6H6
d)12 mol CO2
e)2 mol CO2
f)44 g CO2
1
2
3
4
1)
2)
3)
4)
13.

2C2H2 + 5O2 --> 4CO2 + 2H2O

How many moles of acetylene will be required to produce 200 L of carbon dioxide (CO2)?

a)22.4 L CO2
b)1 mole CO2
c)4 moles CO2
d)2 moles C2H2
1
2
3
4
1)
2)
3)
4)
14.

When sulfur dioxide reacts with oxygen, sulfur trioxide is formed.

2SO2 + O2 → 2SO3

How many grams of sulfur trioxide will be produced from 64.0 grams of sulfur dioxide?

a)

256 g

b)

160 g

c)

128 g

d)

80.0 g

15.

Ammonia is synthesized from nitrogen and hydrogen gases.

N2 + 3H2 → 2NH3

If 10.0 moles of nitrogen are used, how many moles of ammonia will be produced?

a)

40.0 moles

b)

30.0 moles

c)

20.0 moles

d)

10.0 moles

16.

Calcium carbonate decomposes into calcium oxide and carbon dioxide.

CaCO3 → CaO + CO2

How many grams of calcium oxide will be produced from 200.0 grams of calcium carbonate?

a)

168 g

b)

56.0 g

c)

112 g

d)

200 g

17.

Determine the volume of carbon dioxide gas produced at STP when 2.5 g of nitroglycerin (C3H5N3) decomposes by this balanced equation. Round your answer to two decimal points.

4C3H5N3O9(l) → 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)

18.

Use the reaction to answer these stoichiometry questions.

3Cl2 + 6NaOH --> 5NaCl + NaClO3 + 3H2O

What is the mole ratio of chlorine to sodium hydroxide?

a)

1:1

b)

1:2

c)

2:1

d)

2:3

19.

C3H8 + 5O2 --> 3CO2 + 4H2O

A tank containing 55 L of propane gas contains 2.46 moles of the gas. If the whole amount of gas reacts with a sufficient amount of oxygen gas, how many grams of water will be produced?

a)

9.84 g

b)

12.3 g

c)

177 g

d)

221 g

20.

Suppose we have the following pizza recipe:

1 crust + 5 ounces tomato sauce + 2 cups cheese → 1 pizza

Let's assume that we currently have 4 crusts and 10 cups of cheese. What is the minimum number of ounces of tomato sauce would you need in order to make 3 pizzas?

a)

10

b)

15

c)

20

d)

25

21.

Predict the mass of iron filings required to completely react with 2.5 g of yellow sulfur solid, S8(s), to yield iron (III) sulfide.

3S8 + 16Fe --> 8Fe2S3

a)

0.54 g Fe

b)

1.5 g Fe

c)

2.9 g Fe

d)

4.3 g Fe

22.

What is the volume of 1.0 mole of hydrogen gas at standard temperature and pressure?

a)

5.5 L

b)

11 L

c)

22 L

d)

44 L

23.

Chocolate Chip Cookie Recipe:
1 cup of flour
100 chocolate chips
1 cup sugar
1/2 cup milk
Yields 10 cookies


You and your sister want to bake chocolate chip cookies. You go to the store and buy 5 cups of flour, three bags of chips, each containing 100 chocolate chips, 6 cups of sugar, and 10 cups of milk. You want to make as many cookies as possible. What is your limiting reactant, the ingredient that would run out first?

a)

milk

b)

flour

c)

sugar

d)

chocolate chips

24.

4Al + 3O2 → 2Al2O3

How many grams of aluminum are required to produce 3.5 moles Al2O3 in the presence of excess O2?

a)

94.5 g

b)

108 g

c)

189 g

d)

378 g

25.

The reaction between solid white phosphorous and oxygen produces solid tetraphosphorous decaoxide (P4O10). The balanced equation is given below:

P4 + 5O2 → P4O10

What is the limiting reactant if you are using 25.0 grams of phosphorus and 50.0 grams of oxygen?

a)

O2

b)

P4

c)

P4O10

d)

P4O2

26.


In the chemical reaction NaHCO3 + CH3COOH → CH3COONa + H2O +CO2, 83 g of sodium bicarbonate reacts with 70 g of acetic acid. Which of these is correct?

a)

Amount of NaHCO3 is in excess.

b)

Amount of CH3COOH is in excess.

c)

CH3COOH is the limiting reagent.

d)

Amount of CH3COONa is in excess.

27.


In a reaction 4 NH3 + 5 O2 → 4 NO + 6 H2O, 1 mole of ammonia reacts with 2 moles of oxygen. Which of these is correct after the reaction is complete?

a)

All the oxygen is consumed.

b)

All the ammonia is consumed.

c)

1 mole of oxygen remains.

d)

1 mole of water is produced.

28.

Hydrogen gas (H2) reacts with oxygen gas (O2) and produces water. If one mol of hydrogen reacts with one mol of oxygen, what is the limiting reactant?

a)

oxygen gas

b)

water vapor

c)

hydrogen gas

d)

liquid water

29.

4Al + 3O2 → 2Al2O3

How many grams of aluminum are required to produce 3.5 moles Al2O3 in the presence of excess O2? Round your answer to the whole number.

30.

Hydrazine (N2H4), a rocket fuel , reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation:
N2H4(l) + O2(g) → N2(g) + 2H2O(g)

How many grams of hydrazine (N2H4) are needed to produce 96.0g water?

Round your answer to one decimal point.

31.

Zn + 2HCl → ZnCl2 + H2

At conditions of Standard Temperature and Pressure, determine how many liters of hydrogen gas are produced by placing a zinc nail with a mass of 2.2g into an excess of hydrochloric acid.

a)

6.42 L

b)

1.33 L

c)

0.75 L

d)

0.0015 L

32.


C3H8 + 5O2 → 3CO2 + 4H2O

In the chemical reaction for the combustion of propane, determine, at standard temperature and pressure, how many liters of carbon dioxide gas are produced if 15 liters of oxygen gas are completely consumed.

a)

3

b)

5

c)

6

d)

9

33.
2Na + S -->Na2S
What is the total number of moles of Na2S produced when 8.0 moles of Na were completely consumed?
4 lines
34.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
35.

The Reactant that is NOT used up is called the ..............

a)

Limiting Reactant

b)

Excess Reactant

36.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
37.

B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 20.0 g of B2H6 ?

a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
38.

Identify the limiting and excess reactants in the reaction shown.

a)

N2 is limiting and H2 is excess. 

b)

H2 is limiting and N2 is excess. 

c)

NH3 is both limiting and excess.

d)

There is no limiting reactant. 

39.

This reactant determines the maximum amount of product you could produce.

a)

Limiting Reactant

b)

Excess Reactant

40.

Identify the limiting and excess reactants in the reaction shown.

a)

O2 is limiting and H2 is excess. 

b)

H2 is limiting and O2 is excess. 

c)

O2 is both limiting and excess.

d)

There is no limiting reactant. 

41.

If 23 g KCl are obtained,

what is the percent yield for the reaction?

a)

44%

b)

102%

c)

98%

d)

43%

42.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
43.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)

6 mol H

b)

2 mol H

c)

3 mol H

d)

1 mol H

44.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
45.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
46.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
47.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
48.
Mg(s) + 2 HCl(aq)  -->  MgCl₂(aq)   + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?
a)
3.8 moles
b)
15 moles
c)
7.5 moles
d)
23 moles
49.
 CaC₂(s) + 2H₂O(l)   -->   C₂H₂(g)   + Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed with 3.20 moles of CaC₂?
a)
119 g
b)
21.2 g
c)
114 g
d)
237 g
50.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of iodine can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
51.
Using the following equation:
4NH3(g) + 5O2(g) --> 4NO(g) + 6H2O(l)
How many grams of oxygen gas are needed to react with 56.8 grams of ammonia?
a)
45.08 g O2
b)
133.33 g O2
c)
260.77 g O2
d)
75.92 g O2
52.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
53.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
54.
2 CO (g) + O2(g) → 2 CO2 (g)
In the formation of CO2 from CO and oxygen, how many Liters of CO2 are produced by the reaction of 8 mols of O2 with an excess of carbon monoxide?
a)
0.178 L
b)
358.4 Liters
c)
704 grams
d)
0.36 grams
55.
Cl2 + 2 KBr → Br2 + 2 KCl
How many grams of potassium chloride can be produced from 356 g of chlorine and 356 g of potassium bromide?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
56.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
57.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
58.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
59.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
60.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
61.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
62.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
63.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
64.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
65.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
66.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
67.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
68.

When magnesium reacts with nitrogen gas, magnesium nitride is formed.

3Mg + N2 → Mg3N2

How many grams of magnesium nitride will be produced from 48.6 grams of magnesium?

a)

100.0 g

b)

74.6 g

c)

162.0 g

d)

200.0 g

69.

In the reaction of aluminum with chlorine gas, aluminum chloride is formed.

2Al + 3Cl2 → 2AlCl3

If 5.0 moles of aluminum are used, how many moles of aluminum chloride will be produced?

a)

10.0 moles

b)

7.5 moles

c)

5.0 moles

d)

15.0 moles

70.

Calcium carbonate decomposes into calcium oxide and carbon dioxide gas.

CaCO3 → CaO + CO2

How many grams of calcium oxide will be produced from 200 grams of calcium carbonate?

a)

200.0 g

b)

168.0 g

c)

112.0 g

d)

56.0 g

71.

What is the formula for percent yield?

a)

ActualTheoretical×100\frac{Actual}{Theoretical}\times100

b)

TheoreticalActual×100\frac{Theoretical}{Actual}\times100

c)

Actual×Theoretical100\frac{Actual\times Theoretical}{100}

d)

100Actual×Theoretical\frac{100}{Actual\times Theoretical}

72.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
73.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
74.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

75.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
76.

The theoretical yield of a reaction is 237 grams, but the reaction actually yields 26 less grams than expected. What is the percent yield?

a)

17.6%

b)

82.4%

c)

89.0%

d)

121.3%

77.

Which of the following reactions has the lowest percent yield?

a)

Theoretical yield 25.7 g; actual yield 23.2 g

b)

Theoretical yield 42.1 g; actual yield 39.9 g

c)

Theoretical yield 18.2 g; actual yield 15.6 g

d)

Theoretical yield 93.4 g; actual yield 87.9 g

78.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
79.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
80.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

15.5

81.

3FeCl2 + 2Na3PO4 → Fe3(PO4)2 + 6NaCl

If 23 grams of iron (II) chloride reacts with 41 grams of sodium phosphate. Determine the limiting reactant

a)

Fe3(PO4)2

b)

Na3PO4

c)

FeCl2

d)

NaCl

82.

Cu + 2AgNO3 → 2Ag + Cu(NO3)2

When 160 g of copper reacts with 200 g of silver nitrate according to the equation above, the limiting reactant of copper (II) nitrate is ​ (a)   and the theoretical yield is ​ (b)  

Choose from the below words

Cu(NO3)2 Cu\left(NO_3\right)_{2\ }  

110.4 g110.4\ g  

AgAg
CuCu
AgNO3AgNO_3
472.2 g472.2\ g
441.6 g441.6\ g
83.

Using the following equation:

Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H2O(l)

How many grams of iron can be made from 6.00 grams of H2 and excess Fe2O3?



(a)  

84.

2 Al + 3 Cl2 ---> 2 AlCl3. 

If 2 moles of aluminum and 2 moles of chlorine are reacted,

identify the limiting reactant ​​ (a)  

Identify the excess reactant ​ ​ ​ ​ ​ (b)  

Choose from the below words
Aluminum
Chlorine
Aluminum Chloride
85.

P4 + 3 O2 --> P4O6 
How many grams of product is made when 12 grams of P4 react with 15 grams of O2?

(a)  

86.

Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.

If 2.00 moles of aluminum and 3.00 moles of chlorine are reacted, how much ,in grams, AlCl3 can be made?

a)

133

b)

0.00750

c)

9.88

d)

267

87.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
88.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
89.

The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield?

C6H6 + HNO3 → C6H5NO2 + H2O

a)

100%

b)

27.39%

c)

54.29%

d)

85.62%

90.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

91.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
92.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
d)
None
93.

The balanced chemical equation for the reaction of sodium with iron (III) oxide is:

6Na + Fe2O3 → 3Na2O + 2Fe

If 80.0g of sodium (Na) reacts with 72.0g of iron (III) oxide (Fe2O3) , what is the limiting reactant?

a)

Na

b)

Fe2O3

c)

Na2O

d)

Fe

94.

The balanced chemical equation for the reaction of sodium with iron (III) oxide is:

6Na + Fe2O3 → 3Na2O + 2Fe

If 80.0g of sodium (Na) reacts with 72.0g of iron (III) oxide (Fe2O3) , what is the theoretical yield of iron (Fe)?

a)

50.4 g Fe

b)

64.9 g

c)

8.0 g

d)

44.2 g

95.

Which is true of the reaction shown here?

a)

two molecules of Substance Y will be left over when this reaction goes to completion

b)

Substance Y is the limiting reactant in this reaction

c)

the mole ratio of this reaction is 6:5:6

d)

adding more molecules of Substance X will not affect the amount of Substance Z produced

96.

Nitrogen acts as a(n) ​ (a)   reactant when 2 mol of nitrogen and 5 mol of hydrogen react in the production of ammonia.

N2 + 3H2 --> 2NH3

Choose from the below words
limiting
product
excess
97.

In this chemical reaction, 6 moles of each of the reactants is combined.

3Mg + N2 → Mg3N2

Which is the limiting reagent?

a)

Mg

b)

N2

98.

In this chemical reaction, 6 moles of each of the reactants is combined.

3Mg + N2 → Mg3N2

Which is the excess reagent?

a)

Mg

b)

N2

99.

In this chemical reaction, 6 moles of each of the reactants is combined.

3Mg + N2 → Mg3N2

What is the theoretical yield?

a)

600 g

b)

200 g

c)

400 g

d)

800 g

100.

Which molecule is the excess reactant?

a)

hydrogen

b)

nitrogen

c)

ammonia

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