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Worksheets26 Week CCA Review
Total questions: 20
Worksheet time: 10mins
Name
Class
Date
1.
What happens to the average kinetic energy of matter when it is heated?
a)
It increases.
b)
It decreases.
c)
It remains the same.
d)
It cannot be determined.
2.
During a phase change, the temperature...
a)
increases.
b)
decreases.
c)
stays the same.
3.
What is NOT one of the assumptions of the Kinetic Molecular Theory (KMT)?
a)
Particles have no volume.
b)
Particles move randomly.
c)
Particles have inelastic collisions
d)
Particles lose no energy in collisions
4.
At what point(s) is a phase change occurring?
a)
A
b)
A & C
c)
B & D
d)
E
5.
Point "B" is known as the:
a)
Melting Point
b)
Boiling Point
c)
Freezing Point
d)
Melting & Freezing Point
6.
At which point is this substance a liquid?
a)
A
b)
C
c)
E
7.
At which point is the substance a solid?
a)
A
b)
C
c)
E
8.
True or false: The lower the temperature, the more the atoms move.
a)
True
b)
False
9.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
air molecules speed up and collide with the tire walls more often
c)
rubber in the tires reacts with oxygen in the atmosphere
d)
air molecules diffuse rapidly through the walls of the tire.
10.
What are the products for this DR reaction
NaOH + Fe(NO3)3 -->
NaOH + Fe(NO3)3 -->
a)
NaFe(s) + OH(NO3)3(aq)
b)
NaNO3(aq) + Fe(OH)3(s)
c)
No Reaction
d)
Na(NO3)3(aq) + FeOH(s)
11.
What are the products when a solution of sodium phosphate is mixed with a solution of calcium chloride?
a)
calcium phosphate and sodium chloride
b)
calcium phosphide and sodium chlorite
c)
sodium calcide and phosphorous chloride
d)
No reaction
12.
What is the molarity of a solution made from 325.4g of AlCl3 with enough water to make 500.0 mL? (MM of AlCl3 = 133.34 g/mol)
a)
4.88 M
b)
2.44 M
c)
0.651M
d)
0.00488M
13.
Find the molarity of 186.55 g of sugar (C12H22O11) in 250. mL of water. (MM of sugar = 342.30 g/mol)
a)
2.18M
b)
2.17M
c)
1.18M
d)
.00218 M
14.
How many grams of solute are dissolved in 125.0 mL of 5.00M NaCl? (MM NaCl= 58.44 g/mol
a)
0.625 g NaCl
b)
36.5 g NaCl
c)
10.7 g NaCl
d)
502 g NaCl
15.
What is the concentration of a solution made by diluting 120mL of a 0.30M solution of NaCl to a final volume of 1.5L?
a)
24M
b)
0.024M
c)
0.60M
d)
3.75M
16.
How many grams of potassium dichromate will dissolve in 100 g of water at 50oC forming a saturated solution?
a)
20g
b)
30g
c)
40g
d)
50g
17.
Which of the following ionic compounds will remain as an aqueous solution and not form an insoluble precipitate?
a)
PbSO4
b)
PbPO4
c)
CaCO3
d)
CaS
18.
What would you do to change a saturated solid/liquid solution to an unsaturated solution?
a)
Add more solute
b)
Add more solvent
c)
Lower the temperature.
d)
Agitate the solution
19.
What distinguishes a saturated solution from a supersaturated solution?
a)
A saturated solution contains more solute than is theoretically possible at a given temperature.
b)
A supersaturated solution contains less than the maximum amount of solute that is possible at a given temperature.
c)
A saturated solution contains more solute than the same volume of supersaturated solution at the same temperature.
d)
A supersaturated solution contains more solute than is theoretically possible at a given temperature.
20.
A student is planning an investigation to determine how the average kinetic energy of the particles of four different liquids changes over time as conditions change. Which tool does he need to measure average kinetic energy?
a)
balance
b)
calorimeter
c)
thermometer
d)
manometer
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