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Stoichometry

Total questions: 37

Worksheet time: 9hrs 15mins

Name
Class
Date
1.

The rusting of iron is represented by the equation

4Fe + 3O2 --> 2 Fe2O3

If you have a 1.45 mol sample of iron, how many moles of Fe2O3 will form after the iron has rusted completely?

a)

0.483 mol

b)

0.725 mol

c)

0.97 mol

d)

1.45 mol

2.

For the reaction

C2H4 + 3 O2 --> 2 CO2 + H2O

If 5.5 mol of CO2 are produced, how many moles of O2 reacted?

a)

3.6 mol

b)

6.8 mol

c)

8.2 mol

d)

13.7 mol

3.

For the following equation

4NH3 + 7 O2 --> 4 NO2 + 6 H2O

How many moles of ammonia are required to produce 11.9 moles of water?

a)

4.76 mol

b)

11.9 mol

c)

7.93 mol

d)

5.95 mol

4.

For the following equation

4NH3 + 7 O2 --> 4 NO2 + 6 H2O

How many molecules of NO2 are produced when 5.38 moles of ammonia react completely?

a)

21.52

b)

6.48 x 1024

c)

3.24 x 1024

d)

247

5.

For the reaction

2Cl2 + 4NaOH -> 3NaCl + NaClO2 + 2H2O

How many moles of Cl2 are needed to react with 11.6 g of 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

6.

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

2 C4H10 + 13 O2 --> 8 CO2 + 10 H2O

a)

181.1 g CO2

b)

90.6 g CO2

c)

11.32 g CO2

d)

119.6 g CO2

7.

Consider the reaction

Mg2Si + 4 H2O --> 2 Mg(OH)2 + SiH4

Calculate the number of grams of silane, SiH4, formed when 35.9 g of Mg2Si reacts with excess water.

a)

30.1 g

b)

10.1 g

c)

15.0 g

d)

19.5 g

8.

what is actual yield

a)

a complete product actual product

b)

Chemical reaction is greater than one component

c)

a short reaction

d)

how much is statistically yielded

e)

The relationship of chemicals

9.

what is excess reactant

a)

a complete product actual yield

b)

Chemical reaction is greater than one component

c)

how much is statistically yielded

d)

a short reaction

10.

What is limiting reactant

a)

The substance is completely gone after the reaction has finished

b)

how much is statistically yielded

c)

The relationship of chemicals

d)

The formula to solve the chemistry

11.

percent yield

a)

The substance is completely gone after the reaction has finished

b)

the percentage ratio to the original yield

c)

a relationship taking place in a reaction to form a compound

d)

the amount of product gathered from the original reaction

12.

what is stoichiometry

a)

a relationship taking place in a reaction to form a compound

b)

the amount of product gathered from the original reaction

c)

The substance is completely gone after the reaction has finished

d)

The amount of product solved by the finished reaction

13.

what is theoretical yield

a)

The amount of product solved by the finished reaction

b)

the amount of product gathered from the original reaction

c)

The substance is completely gone after the reaction has finished

d)

The amount of product solved by the finished reaction

14.
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
15.
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
16.
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
17.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
18.
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
19.
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
20.
1. What is a limiting reagent?
a)
any reactant used up first in a reaction.
b)
any reactant left over at the end of a reaction.
c)
the maximum amount of product formed from a given amount of reactant.
d)
the purity of the reactant.
21.

The reactant that is not completely used up in a chemical reaction is called the __________ .

a)

spectator reagent

b)

limiting reagent

c)

excess reagent

d)

catalyst

22.
When 12 moles of O2 reacts with 6 moles of C10H8, what is the limiting reactant?  
1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
23.
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
24.
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
25.

Which reactant is the limiting reagent and why?

2H2(g) + O2(g) → 2H2O(l)

a)

Hydrogen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

b)

Oxygen is the limiting reagent because two moles of hydrogen is required for every one mole of oxygen to produce two water.

26.

4NH3 + 5O2 --> 4NO + 6H2O


How many Liters of NO are formed if 6.30g of ammonia react with 1.80g of oxygen?

a)

1.5 L

b)

2.02 L

c)

1.01 L

d)

8.30 L

27.
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
28.
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
29.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04
30.
What does percent yield indicate?
a)
The amount of product we should get
b)
The efficiency of the lab
c)
The amount of product we actually got
d)
nothing
31.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
32.
Percent yield = 100%
Theoretical yield = 88 grams
What is your actual yield?
a)
88 grams
b)
88%
c)
100 grams
d)
22%
33.
Which of the following do you get through measuring its mass? (No calculations)
a)
percent yield
b)
theoretical yield
c)
actual yield
d)
limiting reagent
34.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
35.
Zn  +  CuCl​2​​  →  ZnCl​2​  ​+  Cu
How many moles of ZnCl2 will be produced from 23.0 g of Zn
a)
0.354 moles
b)
1495 moles
c)
47.76 g
36.
Zn  +  CuCl​2​​  →  ZnCl​2​  ​+  Cu
How many grams of ZnCl2 will be produced from 23.0 g of Zn
a)
0.354 moles
b)
1495 moles
c)
47.76 g
37.
Zn + 2HCl → ZnCl​2 ​​+ H​2​​
15 grams of HCl should theoretically produce 0.42 grams of H2. The reaction actually produced 0.15 grams of H2. What is the percent yield of H2?
a)
2.8%
b)
280%
c)
1%
d)
36%

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