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Unit 1: Matter

Total questions: 57

Worksheet time: 57mins

Name
Class
Date
1.

Which answer below is an example of two physical properties of matter?

a)

weight and toxicity

b)

mass and reactivity

c)

mass and volume

d)

mass and pH

2.

Which state of matter has an indefinite shape and a definite volume?

a)

liquid

b)

solid

c)

gas

d)

plasma

3.

Which state of matter has a definite shape and a definite volume?

a)

liquid

b)

solid

c)

gas

d)

plasma

4.

Mixtures are

a)

physically combined and can usually be separated.

b)

physically combined and can never be separated.

c)

chemically combined.

d)

We have no way of knowing how they combine.

5.

A salt water solution can be separated by

a)

filtration

b)

a sieve

c)

a centrifuge

d)

evaporation

6.

_________ is the amount of space an object takes up.

a)

Mass

b)

Matter

c)

Volume

d)

Density

7.

Which type of matter can not be broken down into simpler substances by a chemical change?

a)

an element

b)

a solution

c)

a mixture

d)

a compound

8.

Two grams of potassium chloride are completely

dissolved in a sample of water in a beaker. This

solution is classified as

a)

an element

b)

a compound

c)

a homogeneous mixture

d)

a heterogeneous mixture

9.

Which statement describes a chemical property of sodium?

a)

Sodium has a melting point of 371 K.

b)

Sodium has a molar mass of 23 grams.

c)

Sodium can conduct electricity in the liquid phase.

d)

Sodium can combine with chlorine to produce a salt.

10.

When a chemical change occurs, the substances you start and finish with have

a)

the same chemical properties

b)

different chemical properties

11.

Which particle diagram represents a mixture of element X and element Z, only?

a)
b)
c)
d)
12.

Which sample of matter is a mixture?

a)

soil

b)

ammonia

c)

water

d)

calcium

13.

When a mixture of water, sand, and salt is filtered, what remains at the top of the filter paper?

a)

salt and sand, only

b)

sand, only

c)

salt and water, only

d)

salt, only

14.

A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different

a)

densities

b)

particle sizes

c)

boiling points

d)

solubilities

15.
Frank has a paper clip. It has a mass of 9g and a volume of 3cm3. What is its density?
a)
3 g/cm3
b)
1/3 g/cm3
c)
27 g/cm3
d)
39 g/cm3
16.

What units are used to measure mass?

a)

g

b)

cm3

c)

g/cm3

d)

cm3/g

17.

A beaker is used to measure volume in which metric unit?

a)

Milliliters (mL)

b)

Grams (g)

c)

Meters (m)

d)

Kilograms (kg)

18.

Which is the best example of a pure substance?

a)

peanut

b)

milk

c)

gold

d)

air

19.

An object has a density of 1.4 g/cm3. It is slowly lowered into a graduated cylinder whose water level was 65 mL. When the object is completely submerged the water level rises to 90 mL. What is the mass of the object?

a)

25 g

b)

15 g

c)

35 g

d)

18 g

20.

Find the density of a block with a length of 4 cm, a width of 6 cm, a height of 0.5 cm, and a mass of 23 grams.

a)

0.192 g/cm3

b)

1.917 g/cm3

c)

5.750 g/cm3

d)

12.00 g/cm3

21.

Filtration can be used to separate mixtures based on

a)

boiling point

b)

their densities

c)

their melting points

d)

the size of their particles

22.

The chart lists the densities of various gemstones. A gemstone has a mass of 6.24 grams and a volume of 1.98 cm3. What is the identity of the gemstone?

a)

opal

b)

diamond

c)

garnet

d)

topaz

23.
What is the energy that an object has because it is moving?
a)
kinetic
b)
potential
c)
electric
d)
wind
24.

What is the Average Kinetic Energy of a substance called?

a)

volume

b)

temperature

c)

pressure

d)

movement

25.

Phase change going from a Solid to a Gas...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Recombination

26.

What is happening to the particles in the substance between points D and E?

a)

Melting

b)

Freezing

c)

Vaporizing

d)

Sublimating

27.

Is the substance gaining or losing energy?

a)

Gaining

b)

Losing

28.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
29.

Between which two points is the solid cooling?

a)

A <---- B

b)

B <----> C

c)

C <---- D

d)

D <----> E

e)

E <---- F

30.

Between which two points is the gas heating up?

a)

A ----> B

b)

B <---- C

c)

C ----> D

d)

D ----> E

e)

E ----> F

31.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
32.
The graph shows a cooling curve for an unknown substance.  What is happening during segment DE?
a)
boiling
b)
condensation
c)
freezing
d)
melting
33.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
34.
Exothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
35.
Endothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
36.
Put the liquids in order from most dense to least dense?
a)
4, 3, 2, 1
b)
1, 2, 3, 4
c)
3, 4, 2, 1, 
d)
4, 3, 1, 2
37.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
38.
Frank has an eraser. It has a mass of 4g, and a volume of 2cm3. What is its density?
a)
8 g/cm3
b)
2 g/cm3
c)
1/2 g/cm3
d)
24 g/cm3
39.
What is the volume of Object X?
a)
10.0 cm3
b)
15.0 cm3
c)
20.0 cm3
d)
25.0 cm3
40.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
41.

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 0.10 J/g°C, what is the mass of the iron sample?

a)

25 g

b)

30 g

c)

20 g

d)

50 g

42.
Using the heat equation, what would the formula look like if we were solving for change in temperature?
a)
Q m = ∆T Cp
b)
Q / (m Cp)  =  ∆T
c)
Q m / Cp  =  ∆T
d)
m c Q  =  ∆T
43.
The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?
a)
12.82 °C
b)
24.12°C
c)
351 °C
44.

What is the symbol for Thermal Energy?

a)

Q

b)

T

c)

m

d)

Cp

45.

What unit do you use to measure Thermal Energy?

a)

J/Kg ºC

b)

Kg

c)

ºC

d)

J

46.
You have 20 g of water with specific heat of 4.18 J/gŸ°C.  The temperature changes from 25° C to 20° C.  How much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
47.

The temperature of an unknown piece of metal with a mass of 30.00 g changes from 25.0 °C to 35.0 °C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?

a)

1.17 J/g°C

b)

-1.17 J/g°C

c)

0.857 J/g°C

d)

-0.857 J/g°C

48.

How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g•°C)]

a)

6.45 J/(g•°C)

b)

6.45 J

c)

16.1 J/(g•°C)

d)

d.16.1 J

49.
Object A has a specific heat of 4.45 J/g⁰C and object B has a specific heat of 1.82 J/g⁰C. Which object will heat up faster?
a)
Object A, it has a lower spefici heat
b)
Object B, it has a lower specific heat
c)
Object A, it has a higher specific heat
d)
Object B, it has a higher specific heat
50.
For the formula:
 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
51.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

52.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
53.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
54.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

55.

What is the mathematical relationship between the Celsius and Kelvin scales of temperature?

a)

C = K + 273

b)

K = C - 273

c)

9/5C + 32 = K - 273

d)

K = C + 273

56.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J
57.

How many Joules of energy are required to make 100 grams of ice at 0 οC completely melt? Ice has a heat of fusion of 334 J/g

a)

200 J

b)

400 J

c)

33,400 J

d)

2,000,000 J

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