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Review Activity 8 - Stoichiometry

Total questions: 50

Worksheet time: 2hrs 40mins

Name
Class
Date
1.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
2.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
3.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
4.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
5.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
6.

Calculate the molar mass of water (H2O).

a)

10 g/mol

b)

17 g/mol

c)

18 g/mol

d)

34 g/mol

7.
What is the mass of 2.50 mol of oxygen gas O2?
a)
40 g
b)
80 g
c)
16 g
d)
32 g
8.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
9.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
10.
How many moles are in 22g of argon?
a)
0.55mol
b)
1.8mol
c)
8.8x102mol
11.
N2 + 3H2 --> 2NH3
How many moles of N2 is needed to react with 6 moles of H2?
a)
6.7
b)
2.0
c)
3.0
d)
15.0
12.
2Na + S -->Na2S
What is the total number of moles of S that reacts when 4.0 moles of Na were completely consumed?
a)
1
b)
2
c)
0.5
d)
4
13.

Where are the numbers for a mole ratio found?

a)

They are part of the chemical formulas for the reactants / products.

b)

They are given in the problem.

c)

They are found on the periodic table for those elements.

d)

They are found as coefficients in the reaction's balanced chemical equation.

14.

The ratio of moles of each reactant and product in a reaction is known as what?

a)

mole

b)

mole ratio

c)

mole constant

d)

molecular theory

15.

The number 6.02 x 1023 is called...

a)

Lewis's number

b)

Bohr's number

c)

Pauling's number

d)

Avogadro's number

16.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
17.
How many moles are 2.85 x 1020 atoms of iron?
a)
4.73 x 10-4 moles
b)
1.72 x 104 moles
c)
1.72 x 10-42 moles
d)
4.73 x 104 moles
18.

How many molecules are there in 5.5 moles potassium chloride?

a)

4.08 x 10-24

b)

3.31 x 1024

c)

33.11

d)

0.98

19.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
20.
How many moles of methane (CH4) are in 1.24 x 1023 molecules of methane?
a)
6.02 x 1023
b)
7.46 x 1046
c)
978
d)
0.206
21.

If I need 2.4 moles of sodium chloride (NaCl), how much should I weigh out?

a)

24 g

b)

60 g

c)

141 g

d)

1.5 x 1024 g

22.
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
23.

2H2 + O2 --> 2H2O How much O2 is required to fully react 12 g of H2?

a)

95 g

b)

12 g

c)

6 g

d)

48 g

24.

Given the equation:

2NaClO3 (s) → 2NaCl (s) + 3O2 (g)


When 2.00 moles of NaClO3 react, how many grams of O2 is produced?

a)

56 g of O2

b)

96 g of O2

c)

64 g O2

d)

32 g O2

25.

2 NaClO3 (s) → 2NaCl (s) +3 O2 (g)

How many grams of O2 will be produced from 12.00 moles of NaClO3?

a)

256 g of O2

b)

576 g of O2

c)

288 g O2

d)

32 g O2

26.

2Na + 2H2O → 2NaOH+ H2

How many grams of hydrogen are produced if 60 g of Na are available?

a)

5.27 g

b)

2.6 g

c)

690 g

d)

45 g

27.

2H2 + O2 → 2H2O

How many grams of H2O can be produced from 3.91 g of O2?

a)

1.905

b)

4.4

c)

2.2

d)

1.1

28.

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

29.

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

30.
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
31.
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
32.

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%

33.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
34.
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
35.
Percent yield = 100%
Theoretical yield = 88 grams
What is your actual yield?
a)
88 grams
b)
88%
c)
100 grams
d)
22%
36.
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
37.

In a chemical reaction a theoretical yield of 4.55 g or ammonia is calculated. After running the experiment in the lab only 3.86 g of ammonia was actually produced. What was the percent yield from the lab experiment?

a)

0.848%

b)

1.17%

c)

117%

d)

84.8%

38.

The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.

a)

actual

b)

theoretical

c)

percent

39.

C3H8 + 5 O2 →3 CO2 + 4 H2O

b) I got a percent yield of 75%, and I started with 5 grams of C3H8. How many grams of water did I make?

a)

6.2 grams

b)

1.5 grams

c)

8.3 grams

d)

4.2 grams

40.

The reaction was supposed to yield 50 g of product. Instead, we measured our product at a mass of only 47.5 g. What was our percent yield?

a)

105%

b)

2.5%

c)

97.5%

d)

95%

41.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
42.
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
43.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
44.
P4 + 3O2 --> P4O6 
What is the limiting reactant is 12 moles of P4 react with 15 moles of O2?
a)
P4
b)
O2
c)
P4O6 
d)
none of the above
45.
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
46.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
47.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
48.

The Formula to make S'mores is:

2C + 1M + G2 → C2MG2. If you have 5 Marshmallows (M), 9 Chocolate Pieces (C), and 9 Graham Cracker Halves (G), how many S'mores can you make?

a)

5

b)

4

c)

8

d)

42

49.
A reactant that remains after a chemical reaction stops
a)
stoichiometry
b)
mole ratio
c)
excess reactant
d)
limiting reactant
50.
1 Body + 4 Tires --> 1 car
How many cars can you make with 92 tires and 34 bodies? 
a)
23
b)
34
c)
68
d)
46

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