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WorksheetsChem Final Review
Total questions: 55
Worksheet time: 5hrs 35mins
Name
Class
Date
1.
PCl5 + ___ H2O → ___ HCl + H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
2.
__ Al + __ FeO → Al2O2 + __ Fe
a)
1, 1, 2
b)
2,1,2
c)
2, 2, 2
d)
2,4,2
3.
Which side of a chemical equation is the reactant side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
4.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
5.
What is the little number after an element in a chemical equation called.
Example: H2
Example: H2
a)
Coefficient
b)
Subscript
c)
Atom
d)
Equation
6.
4Si + S8 --> 2Si2S4
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
7.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
8.
Which reaction type is the following: C5H10O4 + O2 --> CO2 + H2O
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Double Replacement
9.
Which of the following is the general formula for a decomposition reaction?
a)
A + B → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
10.
C4H12 + O2 --> CO2 + H2O
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
11.
This is used to represent the number of each atom being represented.
a)
A Exponent
b)
The Coefficient
c)
A Molecule
d)
The Subscript
12.
This appears on the left side of a chemical formula, and represents how many molecules there are.
a)
An Atom
b)
The Subscript
c)
A Molecule
d)
The Coefficient
13.
How many TOTAL atoms are on the REACTANT side of this equation?
CH4 + 2O2 → CO2 + 2H2O
CH4 + 2O2 → CO2 + 2H2O
a)
5
b)
7
c)
9
d)
11
14.
What is the molar mass of Mg3N2?
a)
191.6 g/mol
b)
76.64 g/mol
c)
38.32 g/mol
d)
100.95 g/mol
15.
How many moles of (NH4)2O are present in 74.9 g?
a)
3,907.0 moles
b)
1.44 moles
c)
8.67x1023moles
d)
0.79 moles
16.
What is Avogadro's Number?
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
17.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
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
18.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
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
19.
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
20.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
21.
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%
22.
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
23.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
24.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
25.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
26.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L
b)
7.81 L
c)
4.63 L
d)
4.36 L
27.
You have a gas that has a pressure of 2 ATM and a volume of 10L. What would be the new volume if the pressure was changed to 1 ATM?
a)
5 L
b)
20 L
c)
It would stay at 10L
d)
1 L
28.
A sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?
a)
60.0 mL
b)
15.0 mL
c)
27.5 mL
d)
32.5 mL
29.
When the temperature is constant (k) inside a balloon, if you add pressure on it, the volume will .....
a)
Decrease
b)
Increase
c)
Not Change at all
d)
Particles will solidify
30.
What is the name of the law that involves these two variables:
Temperature increases // Pressure increases
Temperature increases // Pressure increases
a)
Gay-Lussac's Law
b)
Boyle's Law
c)
Charles' Law
d)
Ideal Gas Law
31.
What is the name of the law that involves these two variables:
Pressure decreases // Volume increases
Pressure decreases // Volume increases
a)
Boyle's Law
b)
Charles' Law
c)
Gay-Lussac's Law
d)
Ideal Gas Law
32.
What three variables are in the Ideal Gas Law?
a)
Pressure, Temperature, Volume
b)
Pressure, Kelvin, # of moles
c)
# of moles, Temperature, Volume
d)
Volume, Heat, and Greenhouse Gases
33.
What of these is always soluble?
a)
Nitrates
b)
Phosphates
c)
Carbonates
d)
Hydroxides
34.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
35.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
36.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
37.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
38.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105 M
b)
1.0 x 109 M
c)
5.0 x 101 M
d)
1.0 x 10-5 M
39.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
40.
If the [H3O+] of a solution is 1 x 10-8 mol/L the [OH-] is
a)
1.0 x 10-6
b)
1.0 x 106
c)
1.0 x 10-8
d)
1.0 x 108
41.
If the [OH-] of a solution is 2.7 x 10-4 mol/L the pOH of the solution is
a)
10.44
b)
3.56
c)
1.00
d)
-4.43
42.
if the [H+] of a solution is 8.4 x 10-3 mol/L the pOH of the solution will be
a)
2.08
b)
11.92
c)
1.02
d)
12.98
43.
Limes have a [H3O+] of 1.3 x 10-2 mol/L. Their pOH is
a)
1.89
b)
12.11
c)
1.03
d)
12.97
44.
An acid’s pH is between :
a)
0 to 6
b)
7
c)
8-14
d)
6-14
45.
If [H] = 0.00001
a)
pH = 5
b)
pH = 7
c)
pH = 9
d)
pH cannot be found with what is given.
46.
phosphorous acid
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
47.
lead (II) phosphate
a)
PbPO4
b)
Pb2PO4
c)
Pb3(PO4)2
d)
Pb2(PO4)3
48.
bromic acid
a)
HBr
b)
HBrO2
c)
HBrO3
d)
H3BrO3
49.
H3PO4
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
50.
H3PO3
a)
hydrophosphoric acid
b)
phosphorous acid
c)
phosphoric acid
d)
phosphoric hydroxide
51.
Barium hydroxide
a)
BaOH
b)
Ba2OH
c)
Ba(OH)2
52.
Do the reactants in an exothermic reaction have a higher or lower energy than the products?
a)
Higher
b)
Lower
53.
The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?
a)
0.13 J/(g°C)
b)
17,000 J/(g°C)
c)
1600 J/(g°C)
d)
0.065 J/(g°C)
54.
A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?
a)
12.7 kg
b)
2.25 kg
c)
110 kg
d)
1.97 kg
55.
Durning a phase change the temperature of a substance_________.
a)
always increases
b)
always decreases
c)
always stays the same
d)
varies
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