WorksheetsChemistry Semester Review
Total questions: 100
Worksheet time: 3hrs 45mins
Name
Class
Date
1.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)
12.00 moles of NaClO3 will produce how many grams of O2?
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
2.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
What mass of O2 will be needed to burn 36.1 g of B2H6?
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
3.
2CO + O2 −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
4.
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
5.
2CO + O2 −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide at STP?
How many liters of carbon dioxide are produced from 10L of carbon monoxide at STP?
a)
10
b)
20
c)
1
d)
5
6.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
7.
Consider the Equation:
2H2 + O2 −−〉 2H2O
How many moles of water can be formed from 3.91 g of O2?
2H2 + O2 −−〉 2H2O
How many moles of water can be formed from 3.91 g of O2?
a)
1.905
b)
.244
c)
2.2
d)
1.1
8.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
9.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
10.
What is the molar mass of C6H12O6?
a)
180.18
b)
180.12
c)
180.24
d)
180.06
11.
2H2 + O2 → 2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
12.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Ask for help
13.
How many grams are in 3.3 mol of Potassium Sulfide (K2S)?
a)
363 g
b)
454 g
c)
238 g
d)
132 g
14.
Which of the following has the greatest amount of movement at a given temperature?
a)
Gas
b)
Liquid
c)
Solid
d)
They all have the same movement
15.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
16.
What will happen to the volume of a gas under constant temperature if the pressure increases?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
17.
If you increase the pressure of a constant volume of gas, what will happen to the temperature?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
18.
How do you convert Celsius to Kelvin?
a)
Add 273
b)
Subtract 273
c)
You can't convert those
d)
They are the same thing
19.
What about gasses can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
20.
Which is a quality that only gasses display
a)
Spread out to fill all available space
b)
Take the shape of their container
c)
Can't be compressed
d)
All of these
21.
What is 0.00 degrees Kelvin known as
a)
No such thing
b)
Very cold
c)
Freezing point of Water
d)
Absolute Zero
22.
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
23.
Which of the following would increase the pressure on a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
24.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
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
25.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
26.
What law combines all 3 factors (pressure, temperature, and volume)
a)
Combined Gas Law
b)
Charle's Law
c)
Boyle's Law
d)
Avagadros Ideal Gas Law
27.
3. According to Boyle's law, at constant temperature, as the pressure of a given sample of gas is increased, the volume will –
a)
Increase
b)
Decrease
c)
Remains the same
28.
5. As per Charles' Law if temperature of any gas is increased its volume will -
a)
increase
b)
decrease
c)
remains the same
29.
Boyle's law : When _______ is held constant, the pressure and volume of a gas are ________ proportional
a)
temperature, equally
b)
mass, inversely
c)
temperature, inversely
d)
mass, equally
30.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
31.
Gases have...
a)
A definite shape and volume
b)
A definite shape but no definite volume
c)
No definite shape but a definite volume
d)
No definite shape or volume
32.
Boyle's law : The pressure and volume of a gas show a _____ relationship.
a)
No relationship
b)
Direct
c)
Inverse
d)
Equal
33.
What is the equation for Charles' Law?
a)
P1V1=P2V2
b)
V1/T1=V2/T2
c)
V1/n1=V2/n2
d)
P1/T1=P2/T2
34.
What is the equation for Boyle's Law?
a)
P1V1=P2V2
b)
V1/T1=V2/T2
c)
V1/n1=V2/n2
d)
P1/T1=P2/T2
35.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
36.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
37.
The molecules of a gas are in constant and random motion.
a)
TRUE
b)
FALSE
c)
DEPENDS UPON THE KIND OF MOLECULE
38.
What type of molecule is water
a)
polar
b)
nonpolar
c)
neither
39.
It requires a lot of heat input in order to raise the temperature of water. This is because water has a high
a)
surface tension
b)
density
c)
specific heat
d)
RBI
40.
As water freezes
a)
its mass goes up
b)
its mass goes down
c)
its volume goes up
d)
its volume goes down
41.
How does the density of water compare as a solid to as a liquid?
a)
solid water is more dense
b)
solid water is less dense
c)
liquid water is less dense
d)
none of the above
42.
This is the quality that allows water gliders to walk on water
a)
specific heat
b)
capillarity
c)
surface tension
d)
super solvent
43.
Water travels up plants because of
a)
capillarity
b)
surface tension
c)
density
d)
specific heat
44.
If you heat equal masses of water and metal with the same amount of heat,
a)
the water will get hotter faster
b)
the metal will get hotter faster
c)
the metal will get hotter slower
d)
they heat up at the same rate
45.
Water has a ____________ specific heat
a)
high
b)
low
c)
none of the above
46.
Energy required to raise the temperature of 1 gram of a substance by one degree
a)
super solvent
b)
specific heat
c)
intermolecular forces
d)
capillarity
47.
What is the concentration of a solution that has 8 moles of solute in 2 liters of solution?
a)
4 moles/liter
b)
2 moles/liter
c)
1 mole/liter
d)
16 moles/liter
48.
What is the concentration of a solution which has 4 moles of solute and 2 moles of solvent?
a)
2 moles/liter
b)
4 moles/liter
c)
1 mole/liter
d)
4 moles
49.
This is the term of a solution that could still dissolve more of a certain solute (below the line on the graph)
a)
unsaturated
b)
saturated
c)
supersaturated
d)
none of the above
50.
This is the term of a solution that has dissolved the maximum amount of a specific solute (at the line on the graph)
a)
unsaturated
b)
saturated
c)
supersaturated
d)
none of the above
51.
This is the term of a solution that has dissolved the more than the maximum amount of a specific solute (above the line on the graph)
a)
unsaturated
b)
saturated
c)
supersaturated
d)
none of the above
52.
What is the solubility of KNO3 in 100 grams of water at 50° C?
a)
80 grams
b)
35 grams
c)
160 grams
d)
60 grams
53.
What kind of solution is 100 grams of KBr at 30° C?
a)
supersaturated
b)
unsaturated
c)
saturated
d)
none of the above
54.
What kind of solution is 100 grams of NaClO3 at 30° C?
a)
supersaturated
b)
unsaturated
c)
saturated
d)
none of the above
55.
What kind of solution is 60 grams of KBr at 10° C?
a)
supersaturated
b)
unsaturated
c)
saturated
d)
none of the above
56.
A solution where a relatively small amount of solute is dissolved
a)
dilute
b)
concentrated
c)
neither
57.
A solution where water is the solvent
a)
aqueous
b)
(g)
c)
(s)
d)
(l)
58.
This is the name for a compound that when dissolved conducts electricity
a)
electrolyte
b)
molecular
59.
What is the molarity of a solution which contains 1 mole of solute and 2 liters of solution?
a)
1 mole/liter
b)
0.5 moles/liter
c)
2 moles/liter
d)
3 moles/liter
60.
What is the pOH of a 0.027 M KOH solution?
a)
12.92
b)
1.57
c)
14.11
d)
6.47
61.
Bases taste
a)
bitter
b)
sour
c)
soapy
d)
sweet
62.
What is the hydronium concentration of a solution whose pH is 7.30?
a)
7.1 x 10-6 M
b)
1.4 x 10-11 M
c)
3.8 x 10-8 M
d)
5.0 x 10-8 M
63.
What characterizes a strong acid or base?
a)
ionic bonding
b)
presence of a hydroxide or hydrogen ion
c)
complete ionization in water
d)
polar covalent bonding
64.
What is the pH of a solution whose hydronium ion concentration is 5.03 x 10-1 M?
a)
0.5133
b)
1.542
c)
0.2984
d)
5.031
65.
Bases feel
a)
slippery
b)
dry
c)
rough
d)
moist
66.
Acids react with
a)
water to produce bases and salts
b)
salts to produce bases and water
c)
neither bases, salts nor water
d)
bases to produce salts and water
67.
Which of the following liquids is acidic?
a)
milk of magnesis
b)
seawater
c)
ammonia
d)
orange juice
68.
Acids taste
a)
salty
b)
sweet
c)
sour
d)
bitter
69.
What is the hydronium ion concentration of a solution whose pH is 4.12?
a)
7.6 x 10-5 M
b)
5.1 x 10-6 M
c)
6.4 x 10-5 M
d)
4.4 x 10-8 M
70.
What is the pH of a 10-4 M HCl solution?
a)
6
b)
8
c)
10
d)
4
71.
The pH scale in general use ranges from
a)
0 to 7
b)
-1 to 1
c)
0 to 14
d)
0 to 1
72.
The pH of a basic solution is
a)
less than 0
b)
less than 7
c)
greater than 7
d)
greater than 14
73.
The pH of an acidic solution is
a)
less than 0
b)
less than 7
c)
greater than 7
d)
greather than 14
74.
Acetic acid is found in
a)
sour milk
b)
vinegar
c)
apples
d)
lemons
75.
Amount of energy required to increase the temperature of 1 g of a substance by 1'C
a)
joules
b)
specific heat
c)
Calorie
d)
calorie
76.
124 joules of heat are added to a piece of lead (specific heat = 0.128 J/goC). It is heated to 100.0oC, and then lowered into a calorimeter filled with water. The lead’s temperature decreases to 28.8oC. What is the mass?
a)
150 g
b)
13.6 g
c)
4 g
d)
1130 g
77.
What is the specific heat capacity of silver metal if 55 grams of the metal absorbs 47.3 joules of heat and the temperature rises 15 degrees Celcius?
a)
0.033 J/gC
b)
0.057 J/gC
c)
39000 J/gC
d)
.0455 J/gC
78.
Determine the energy (in kJ) required to raise the temperature of 100.0 g of water from 20.0 C to 85.0 C? The specific heat of water is 4.184 J/(gxC)
a)
5kJ
b)
4,182 J
c)
27,196 J
d)
27.20kJ
79.
How much energy would be needed to heat 450 grams of copper metal from a temperature of 25.0ºC to a temperature of 75.0ºC? (The specific heat of copper at 25.0ºC is 0.385 J/g ºC.)
a)
4,000 J
b)
8,700 J
c)
5,000 J
d)
3,578 J
80.
If ΔH = -95 J
Then...
Then...
a)
The system is losing 95 J to the surroundings
b)
Both the system and surroundings are losing 95 J
c)
The system is gaining 95 J from the surroundings
d)
Both the system and surroundings are gaining 95 J
81.
What kind of reaction has a positive heat of reaction (ΔHr)?
a)
endothermic
b)
exothermic
82.
Exothermic reactions are reactions that
a)
release heat
b)
do not involve heat
c)
absorb heat
d)
take place instantaneously
83.
For the formula:
Q= m c ∆T
The units for specific heat are:
Q= m c ∆T
The units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
84.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is .900J/goC
a)
450
b)
-450
c)
225
d)
-225
85.
A 24.0 gram sample of copper was heated from 25.0oC to 500.0oC, 4378J of heat were absorbed, what is the specific heat of copper?
a)
.384
b)
49909200
c)
2.60
d)
8.77
86.
What happens to particles as they heat up?
a)
They slow down
b)
Nothing
c)
They don't move
d)
They speed up
87.
Water molecules have the greatest kinetic energy in
________________
________________
a)
Ice at 0 °C.
b)
Water at 373 K.
c)
Water at 98 °C
d)
Steam at 150 °C.
88.
How can you convert Kelvin to Celcius?
a)
add 273
b)
subtract 273
c)
multiply by 273
d)
divide by 273
89.
What type of heat transfer is a beaker on a hot plant an example of?
a)
Conduction
b)
Covection
c)
Radiation
d)
Chemical
90.
How can you convert Kelvin to Celcius?
a)
add 273
b)
subtract 273
c)
multiply by 273
d)
divide by 273
91.
Energy transfered between samples of matter because of a difference in their temperature.
a)
Temperature
b)
Enthalpy
c)
Entropy
d)
Heat
92.
Durning a phase change the temperature of a substance_________.
a)
always increases
b)
always decreases
c)
always stays the same
d)
varies
93.
A measure of the average kinetic energy of a substance.
a)
heat
b)
temperature
c)
enthalpy
d)
entropy
94.
.
.
.
.
.
.
What letter represents boiling?
.
.
.
.
.
What letter represents boiling?
a)
B
b)
C
c)
D
d)
E
95.
.
.
.
.
.
.
What letter represents melting?
.
.
.
.
.
What letter represents melting?
a)
A
b)
B
c)
C
d)
D
96.
.
.
.
.
.
.
What letter represents a gas being cooled?
.
.
.
.
.
What letter represents a gas being cooled?
a)
B
b)
C
c)
D
d)
E
97.
.
.
.
.
.
.
What letter represents a liquid being heated?
.
.
.
.
.
What letter represents a liquid being heated?
a)
A
b)
B
c)
C
d)
D
98.
In an exothermic process, the surroundings are are gaining energy.
a)
True
b)
False
99.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
100.
How much energy does it take to freeze 39.2 g of liquid benzene? (ΔHfus = 126 J/g, ΔHvap = 394 J/g) (Show your work)
a)
4940 J
b)
-4940 J
c)
15400 J
d)
-15400 J
100 %
