WorksheetsTest 7 Review
Total questions: 40
Worksheet time: 36mins
Name
Class
Date
1.
Which intermolecular force comes from the fact that electrons are in constant, random motion?
a)
Dispersion forces
b)
Dipole-dipole forces
c)
Hydrogen bonding
d)
Ionic bonding
e)
Covalent bonding
2.
In fizzy water, the water is the ____ and the carbon dioxide gas is the ____.
a)
solute; solute
b)
solvent; solvent
c)
solvent; solute
d)
solute; solvent
3.
What is the definition of molarity?
a)
moles of solvent per liters of solute
b)
moles of solute per liters of solute
c)
moles of solvent per liters of solvent
d)
moles of solute per liters of solvent
e)
moles of solute per liters of solution
4.
In a dilution, the moles of solute _____ and the moles of solvent _____.
a)
increases; stays the same
b)
stays the same; increases
c)
increases; decreases
d)
decreases; increases
e)
increases; increases
5.
A saturated solution contains
a)
more solvent molecules than solute molecules
b)
more solute molecules than solvent molecules
c)
the maximum expected amount of solvent molecules
d)
the maximum expected amount of solute molecules
6.
Which solutions will conduct electricity? (I) Mg(OH)2; (II) C6H12O6; (III) HCl
a)
(I) only
b)
(I) and (II)
c)
(I) and (III)
d)
(II) and (III)
e)
(I), (II), and (III)
7.
A 1M solution of calcium chloride will conduct more electricity than a 1M solution of potassium chloride because...
a)
calcium has a greater ionization energy than potassium
b)
calcium chloride has a larger molar mass than potassium chloride
c)
calcium has two valence electrons, but potassium only has one
d)
calcium chloride dissociates into more particles than potassium chloride
8.
When solute is added to a solvent, the boiling point of the solvent...
a)
decreases because adding the solute pushes the solvent molecules out of the way, making them easier to leave
b)
decreases because now the solvent has more energy
c)
increases because there is a larger mass than before
d)
increases because more energy has to be added to break the new bonds that were formed
9.
A beaker of water is boiling. What is inside the bubbles?
a)
Air
b)
Water
c)
Hydrogen gas and oxygen gas
d)
Hydrogen gas only
e)
Oxygen gas only
10.
Which solution (if any) has the highest freezing point?
a)
1 M NaCl
b)
2 M NaCl
c)
1 M MgCl2
d)
2 M MgCl2
e)
All of these have the same freezing point, because they are all solutions (meaning dissolved in water)
11.
A net ionic equation shows:
a)
All of the ions that are present when two solutions are combined
b)
Only the products when two solutions are combined
c)
The spectator ions when two solutions are combined
d)
Only the ions which were involved in precipiation
12.
Using the solubility rules, which of these choices (if any) will NOT dissolve in water?
a)
NaNO3
b)
Na2S
c)
CaF2
d)
(NH4)3PO4
e)
All of these will dissolve.
13.
What are the spectator ions when calcium nitrate reacts with sodium sulfate?
a)
Na+ and Ca2+
b)
Na+ and NO3-
c)
Ca2+ and NO3-
d)
Na+ and NO3-
14.
In order to evaporate, a molecule must...
a)
lose enough energy to make new intermolecular forces
b)
gain enough energy to make new intermolecular forces
c)
lose enough energy to break intermolecular forces
d)
gain enough energy to break intermolecular forces
15.
____ is energy that is transferred between objects with different ____.
a)
Temperature; specific heats
b)
Specific heat; temperatures
c)
Heat; temperatures
d)
Temperature; potential energies
e)
Temperature; specific heats
16.
What are the units of specific heat capacity (also called specific heat)?
a)
J
b)
°C
°C
c)
J/°C
d)
°C/J
e)
J/g°C
17.
Which constant must be used to calculate how much energy is needed to condense 5 grams of steam at 100°C to water at 100°C?
a)
4.184 J/g°C only
b)
2260 J/g only
c)
334 J/g only
d)
4.184 J/g°C AND 2260 J/g
e)
4.184 J/g°C AND 334 J/g
18.
What is the approximate ΔH of the reaction 2H2 (g) + O2 (g) --> 2H2O (g) ?
a)
-242 kJ/mol
b)
242 kJ/mol
c)
-483 kJ/mol
d)
483 kJ/mol
19.
Which of the following has the highest entropy?
a)
1 mol of He gas at 100 K
b)
1 mol of He gas at 200 K
c)
2 mol of He gas at 100 K
d)
2 mol of He gas at 200 K
e)
All of these are 1 mol of He gas, so they all have the same entropy.
20.
2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of liquid water and the release of heat. Which of the following is true for this reaction?
a)
ΔH>0 and ΔS>0
b)
ΔH>0 and ΔS<0
c)
ΔH<0 and ΔS>0
d)
ΔH<0 and ΔS<0
e)
This is impossible to predict with the given information.
21.
A particular endothermic process corresponds to an increase in entropy. This process is
a)
Never spontaneous
b)
Always spontaneous
c)
Spontaneous, but only at high temperatures
d)
Spontaneous, but only at low temperatures
e)
This is impossible to predict with the given information.
22.
This sealed bottle of water has been sitting in a hot room for hours. It appears that nothing is happening inside. Which of the following best describes the motion of the molecules?
a)
All of the molecules have stopped moving.
b)
All of the molecules are moving. The gas molecules stay in the gas and the liquid molecules stay in the liquid.
c)
All of the molecules are moving. The molecules in the liquid are turning into a gas, and the molecules in the gas are turning into a liquid.
d)
The molecules are reacting to turn into hydrogen gas and liquid oxygen.
e)
The molecules in the droplets are moving. There is no gas in the bottle.
23.
An endothermic reaction is at equilibrium. What will happen if the temperature is increased?
a)
The system will shift right to increase the temperature
b)
The system will shift right to decrease the temperature
c)
The system will shift left to increase the temperature
d)
The system will shift left to decrease the temperature
e)
Nothing will happen because this system is at equilibrium.
24.
If this reaction causes an increase in entropy, will it be spontaneous?
a)
Yes, because it is exothermic
b)
Yes, because any process that increases entropy is always spontaneous
c)
No, because energy must be added for this reaction to occur
d)
No, because any process that increases entropy is never spontaneous
25.
Which of these changes would shift this reaction as far right as possible? (I) Add nitrogen (II) Remove ammonia (III) Decrease pressure
a)
(I) only
b)
(II) only
c)
(III) only
d)
(I) and (II) only
e)
(I), (II) and (III)
26.
Addition of a catalyst ___ the reaction rate by ____ the activation energy.
a)
increases; increasing
b)
increases; decreasing
c)
decreases; increasing
d)
decreases; decreasing
27.
Activation energy
a)
Is always positive
b)
Is always negative
c)
Can be positive, or zero
d)
Can be negative, or zero
e)
Can be positive, negative, or zero
28.
Which of these molecules could have dipole-dipole attraction?
a)
Br2
b)
I2
c)
P4
d)
PCl3
29.
What is the strongest intermolecular force experienced by NH3?
a)
London/dispersion
b)
dipole-dipole
c)
hydrogen
d)
metallic
30.
Which of these has the lowest boiling point?
a)
methanol
b)
ethanol
c)
propanol
d)
butanol
31.
0.45 moles of NaCl are dissolved in 95.0 mL of water. Calculate the molarity of the NaCl solution.
a)
0.0047 M
b)
0.21 M
c)
2.1 M
d)
4.7 M
e)
none of these
32.
45.0 g of Ca(NO3)2 was used to create a 1.3 M solution. What is the volume of the solution?
a)
0.21 mL
b)
210 mL
c)
360 mL
d)
4.7 mL
e)
none of these
33.
How do you make 500.0 mL of 0.500 M NaCl?
a)
Fill a 500 mL volumetric flask to the line, then add 29.25 g of NaCl.
b)
Place 29.25 g of NaCl in a 500 mL volumetric flask, and then add water to the line.
c)
Fill a 500 mL volumetric flask to the line, then add 0.00855 g of NaCl.
d)
Place 0.00855 g of NaCl in a 500 mL volumetric flask, and then add water to the line.
34.
Approximately how many mL of water must be added to 300 mL of 0.75 M HCl to dilute the solution to 0.25 M?
a)
100 mL
b)
300 mL
c)
600 mL
d)
900 mL
e)
930 mL
35.
How many particles will each formula unit of calcium nitrate produce when dissolved in water?
a)
1
b)
2
c)
3
d)
9
36.
Where on this heating curve is kinetic energy increasing?
a)
from A to B
b)
from C to D
c)
from D to E
d)
none of these
e)
more than one of these
37.
There are more product molecules than reactant molecules in an exothermic reaction. It is
a)
spontaneous
b)
not spontaneous
c)
not enough information to determine
38.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of .10 J/g°C, what is the mass of the iron sample?
a)
20. g
b)
25 g
c)
30. g
d)
50. g
39.
What is the amount of heat required to completely melt a 200. g sample of ice?
a)
334 J
b)
836 J
c)
66,800 J
d)
452,000 J
40.
In the reaction N2O4 (g) <-->2NO2 (g),an increase in pressure (by reducing the volume) would make the reaction
a)
form more products
b)
form more reactants
c)
no effect
100 %
