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2nd Semester Midterm Review

Total questions: 65

Worksheet time: 3hrs 32mins

Name
Class
Date
1.

What is the molar mass (NH4)2SO4?

a)

132.14 g/mol

b)

132.14 amu

c)

114.10 g/mol

d)

114.10 amu

2.
How many grams are in 5.38 moles of Na2S?
a)
419.8850052 g
b)
420. g
c)
0.068934112 g
d)
0.0689 g
3.

What is the percentage of iron in Fe(OH)3?

a)

52.257% Fe

b)

90.784% Fe

c)

62.148% Fe

d)

76.656% Fe

4.

What is the empirical formula of a compound that contains 56.34% Copper and 43.66% Sulfur?

a)

Cu2S3

b)

CuS

c)

CuS1.5

d)

Cu3S2

5.
The empirical formula of a molecule is CH.  If its molar mass is 78.11364, what is its molecular formula?
a)
C6H6
b)
CH
c)
C4H4
d)
C8H8
6.
The number in red is what?
2Mg + O2 -> 2MgO
a)
Subscript
b)
Coefficient
c)
Mole ratio
7.
True or false: Reactants are on the right side of the chemical equation
a)
False
b)
True
8.
What is the amount produced in a perfect reaction called?
a)
Theoretical yield
b)
Actual yield
c)
Percent Yield
d)
Stoichiometry
9.

What does percent yield compare?

a)

Percent Yield

b)

Actual Yield

c)

Theoretical Yield

d)

Concentration

10.
What is the amount produced from experimentation called?
a)
Actual Yield
b)
Theoretical Yield
c)
Percent Yield
11.
What's the percent yield of a reaction where through experimentation 34.2g of Rb are produced?  Theoretical yield is 39.7 g
a)
86.14609572%
b)
86.1%
c)
116%
d)
116.08187135%
12.
Using the pictured equation, how many moles of hydrogen can you make with 7.9 g Zn?
a)
.12 g
b)
.121 g
c)
520 g
d)
517 g
13.
Using the pictured equation, how many moles of ZnCl2 are in 13 moles of HCl?
a)
6.5
b)
26
14.
Using the pictured equation, how many grams of zinc chloride are produced from 7.89 moles of zinc?
a)
1075 g ZnCl2
b)
1080 g ZnCl2
c)
.05789 g ZnCl2
d)
.0579 g ZnCl2
15.
What is the mole ratio of Sulfur to Oxygen? (Hint: Balance the equation first!)
a)
1/8
b)
8/8
c)
1/1
d)
8/1
16.
What is the term for the compounds on the left side of the arrow?
a)
Products
b)
Reactants
17.
Which of the following is the reactant that you have enough of?
a)
Excess reactant
b)
Limiting reactant
c)
Stoichiometric reactant
d)
Theoretical reactant
18.
The amount of product formed depends on the excess reactant
a)
True
b)
False
19.
A solution that has not reached limit of solute is
a)
Unsaturated
b)
Saturated
c)
Supersaturated
d)
Concentrated
20.
Something that is supersaturated:
a)
has more solute than it can hold at a certain temp
b)
has not reached its limit of solute
c)
can dissolve more solute
d)
can be dissolved
21.
The substance that is present in the largest amount (typically water) is
a)
Solute
b)
Solvent
c)
Solution
d)
Soluble
22.
Something that is soluble
a)
can be dissolved
b)
cannot be dissolved
23.

14.83 g of CuO is dissolved in 250. mL of solution. What is the molarity of the solution? Remember 1000 mL = 1L

a)

0.746 M

b)

0.7457 M

c)

0.75 M

d)

0.8 M

24.

If the mass percent of a NaCl solution was 38.5%, what mass of NaCl was added to make 300.g of NaCl solution?

a)

115 g

b)

116 g

c)

115.5 g

d)

120 g

25.

How many moles of HCl are needed to prepare 2.0 L of a .50 M HCl solution?

a)

1.0 mol

b)

1 mol

c)

0.2 mol

d)

0.25 mol

26.

Moles solute/Liters solution

a)

Molarity

b)

Mass Percent

c)

Molality

d)

Dilute

27.

Large amount of solute in a solvent

a)

Concentrated

b)

Dilute

c)

Saturated

d)

Supersaturated

28.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
29.
A solution that is considered dilute would be....
a)
Dark in color
b)
Have a strong scent
c)
Have a large amount of solute
d)
Have a small amount of solute
30.

What is the empirical formula of the compound whose molecular formula is P4O10?

a)

PO

b)

PO2

c)

P2O5 ..

d)

P8P20

31.
A compound is 86% carbon and 14% hydrogen by mass.  What is the empirical formula for this compound 
a)
CH
b)
CH2 ..
c)
CH3
d)
CH4
32.
What is the molarity of KF (aq) solution containing 116 grams of KF in 1.00 Liter of solution? 
a)
1.00 M
b)
2.00 M ..
c)
3.00 M
d)
4.00 M
33.

What is the mass in grams of 3.0 x 1023 molecules of CO2?

a)

22g ..

b)

44g

c)

66g

d)

88g

34.

Give the reaction

CH4 + 202 --> C02 + 2H20, What amount of oxygen is needed to completely react with 3 moles of CH4?

a)

2 moles

b)

6 moles ..

c)

2 grams

d)

6 grams

35.

What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0M solution?

a)

2.5

b)

5.0

c)

10 ..

d)

20

36.
How many total atoms are in 4 Ca3(PO4)2? 
a)
20
b)
36
c)
40
d)
52
37.
The number that appears before a chemical formula indicating how many molecules of that compound are present.
a)
subscript
b)
superscript
c)
coefficient
d)
squared
38.
Number of units in one mole of any substance, equal to 6.02 x 1023
a)
mole
b)
molar volume
c)
Avogadro's number
d)
Law of Conservation of Mass
39.
Pain medications can be made as powders or tablets.  The powders tend to work faster than tablets with the same ingredients because powder –
a)
dissolves faster in solution than a single tablet
b)
has more total mass than a single tablet
c)
travels through the bloodstream more easily than a tablet
d)
is easier to swallow than tablets
40.
Power plants that discharge warm water into rivers have a negative effect on aquatic life.  This is because the higher water temperature —
a)
increases the pressure of the river water
b)
increases the pH value of the river water
c)
decreases sediment solubility in the river water
d)
decreases the dissolved oxygen in the river water
41.
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
42.
What is a Limiting Reagent?
a)
speeds up a reaction
b)
what you run out of first
c)
what you have left over
d)
slows down a reaction
43.
What is a Excess Reagent?
a)
amount you end with
b)
what you run out of first
c)
what you have left over
d)
what you start with
44.
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
45.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg 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
46.
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
47.
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
48.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
49.
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
50.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
51.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
52.
11.
LiOH + KCl → LiCl + KOH 

b)  I actually produced 6 grams of lithium chloride and I began this reaction with 20 grams of lithium hydroxide. What is my percent yield?
a)
16.9%
b)
5.91%
c)
1.88%
d)
12.3%
53.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
54.
How many particles (atoms) 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
55.
How many atoms are in 6.3 mol Zn?
a)
6.0x1023atoms Zn
b)
3.8x1024atoms Zn
c)
1.0x10-23atoms Zn
d)
410atoms Zn
56.

Colligative properties of solutions are those properties that depend on ___

a)

the number of solute only

b)

the nature of solute only

c)

both the number and nature of solute

57.

The freezing point of a solution is ___________ that of a pure solvent

a)

more than

b)

equal to

c)

less than

58.

Colligative properties depend on the _____ of solute particles in solution.

a)

Type

b)

pH

c)

Number

d)

Nature

59.

Which part in the diagram describes freezing point depression?

a)

A - B

b)

C - D

c)

E - F

d)

D - G

60.

Amount of ion in CaCl2 is ...

a)

1

b)

2

c)

3

d)

4

61.

Which solution below has the highest boiling point?

a)

NaCl 1 m

b)

CaCl2 1 m

c)

C6H12O6 1 m

d)

AlCl3 1 m

62.

Which one of the following diagrams has the lowest vapor pressure?

a)

1

b)

2

c)

3

d)

4

e)

5

63.
Which technique could increase or speed up the rate of dissolving?
a)
Allowing the mixture to settle
b)
Stirring the mixture
c)
Adding more powder
d)
Adding more water
64.

How many particles will CH3OH produce when it dissolves in water?

a)

1

b)

3

c)

6

d)

9

65.

How many particle will Na2SO4 produce when it dissolves in water?

a)

1

b)

3

c)

5

d)

7

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