Quiz

1. Chapter-3
Heat and Properties of Matter

2. Temperature
• Temperature is a measure of the hotness or
coldness of an object.
• it could be measured by using your hand to
sense the hotness or coldness of an object.
• But your hand is not precise enough to
measure temperature adequately.
• Therefor other methods are used for measuring
temperature.

3. Temperature
Is measured with a thermometer and can be measured in
Kelvin, Celsius, Fahrenheit, and Rankin
Absolute zero-temperature at which particles stop
moving 0°
𝐾
• is a measure of how hot or cold an object is compared to
another object.
• indicates that heat flows from the object with a higher
temperature to the object with a lower temperature.
• Temperature Scales

5. Temperature
1. What is the temperature of freezing water?
1) 0 °F 2) 0 °C 3) 0 K
2. What is the temperature of boiling water?
1) 100 °R 2) 32 °F 3) 373 K
3. How many Celsius units are between the boiling and
freezing points of water?
1) 100 2) 180 3) 273
.4.How many Fahrenheit's units are between the boiling and
freezing points of water?
1) 100 2) 180 3) 273

6. Temperature Conversions
𝑻𝑲 = 𝑻𝑪 + 𝟐𝟕𝟑. 𝟏𝟓
𝑻𝑪 = 𝑻𝑲 − 𝟐𝟕𝟑. 𝟏𝟓
𝑻𝑭 =
𝟗
𝟓
× 𝑻𝒄 + 𝟑𝟐
𝑻𝒄 =
𝟓
𝟗
𝑻𝑭 − 𝟑𝟐
Celsius to Fahrenheit
Fahrenheit to Celsius
Celsius to Kelvin
Kelvin to Celsius
Rankin to Fahrenheit
TR = TF + 460

7. Temperature Conversions
Ex 1: Express the temperature 105.8 °F to Celsius scale?
Ex 2: On a cold winter day, the temperature is –15°C.
What is that temperature in °F?
Ex 3: change 180c to kelvin. and change 5350R to degrees
Fahrenheit?

8. Heat
Definition of heat:
Heat: is energy transferred from one object to another because
of a difference in temperature.
Heat is measured in energy units -- Joules or calories
(1calorie = 4.19 joules).
•Remember that the temperature of a gas is a measure of the
kinetic energy of its molecules.
Hot water Cold
(90. ℃) (10. ℃)
Water Water
(50. ℃) (50. ℃)

9. Specific Heat
• Is amount of energy required to raise the temp. of
one kg of material by one degree Kelvin
• Units : J/(kg·K) or J/(kg·°C)
.
Q: heat (J)
m: mass (kg)
T (𝑻𝒇 − 𝑻𝒊): change in temperature (K or
°C)
C: specific heat (J/kg·K)
The specific heat, c, is characteristic of the material
– Q = heat loss
+ Q = heat gain
 
initial
final T
T
m
c
T
m
c
Q 




10. Specific Heat
• Which sample will
take longer to heat to
100°C?
50 g Al 50 g Cu
Specific Heat Values
(J/(kg·K))
Water
Alcohol
Aluminum
Carbon (graphite)
Sand
Iron
Copper
Silver
4184
2450
920
710
664
450
380
235
• Al - It has a higher specific heat.
• Al - will also take longer to cool down.

11. Ex 1: A 2.0-kg aluminum pan is heated on the stove from
20°C to 110°C. How much heat had to be transferred to the
aluminum? The specific heat capacity of aluminum is 900
J/kg°C.
𝑸 = 𝒄. 𝒎. 𝚫𝑻
Q = (900 J/kg °C ) (2.0 kg) (110 °C – 20 °C)
Q = 162,000 J
𝑄 = 1.62 × 105𝐽

12. Ex 2: A 32-g silver spoon cools from 60°C to 20°C. How
much heat is lost by the spoon
𝐶 = 235J/kg°C.
ans. Q = – 301 J
Ex 3: How many joules of heat must be absorbed
to cool 5 kg of water from 750c to 100c ?
C = 4190 j/kg.c
Ans. Q = 1.36 ×106j.

13. Change of Phase
• Is a change in a substance from one form of
matter (solid, liquid, or gas) to other.
• The change of phase from solid to liquid is
called melting or fusion.
• Heat of fusion Lf =
𝑸
𝒎
• Lf ≡ heat of fusion, Q ≡ amount of heat, m ≡ mass of object.
• The change of phase from liquid to solid is
called freezing or solidification.

14. Change of Phase
• The change of phase from liquid to a gas or
vapor is called vaporization.
• Heat of vaporization Lv =
𝑸
𝒎
Lv ≡ heat of vaporization, Q ≡ amount of heat, m ≡ mass of object.
The change of phase from gas to a liquid is called
condensation.

15. Change of Phase
• Ex 1: If 1340 kJ of heat is required to melt 4 kg of
ice at 0oc into water at 0oc, what is the heat of fusion
of water?
• Ans. Lf = 335 kJ/kg
• Ex 2: If 15.8 MJ of heat is required to vaporize 18.5
kg ethyl alcohol at 78.5oc (its boiling point), what is
the heat of vaporization of ethyl alcohol?
• Ans. Lv = 854 kj/kg

16. Change of Phase
Description of Phase
Change
Term for Phase Change
Heat Movement During
Phase Change
Solid to liquid Melting
Heat goes into the solid as it
melts.
Liquid to solid Freezing
Heat leaves the liquid as it
freezes.
Liquid to gas
Vaporization, which
includes boiling and
evaporation
Heat goes into the liquid as
it vaporizes
Gas to liquid Condensation Heat leaves the gas as it
condenses
Solid to gas Sublimation Heat goes into the solid as it
sublimates

17. Properties of Solids
•Particles of solids are tightly packed.
•They are vibrating about a fixed position.
•Solids have:
• a definite shape
•a definite volume.
Elasticity: is a measure of a deformed objects ability to return to its
original size and shape once the outside forces are removed.

18. Properties of Solids
𝑺 =
𝒂𝒑𝒑𝒍𝒊𝒆𝒅 𝒇𝒐𝒓𝒄𝒆
𝒂𝒓𝒆𝒂 𝒐𝒗𝒆𝒓 𝒘𝒉𝒊𝒄𝒉 𝒕𝒉𝒆 𝒇𝒐𝒓𝒄𝒆 𝒂𝒄𝒕𝒔
=
𝑭
𝑨
𝑵
𝒎𝟐
𝐴=area 𝑚2
𝑆 = 𝑠𝑡𝑟𝑒𝑠𝑠 𝑖𝑛 𝑁/𝑚2
𝐹=Force applied (N)
Stress: is the ratio of the outside applied force, which tends to cause a distortion, to the
area 𝑜𝑣𝑒𝑟 𝑤ℎ𝑖𝑐ℎ 𝑡ℎ𝑒 𝑓𝑜𝑟𝑐𝑒 𝑎𝑐𝑡𝑠
𝟏
𝑵
𝒎𝟐 = 𝟏 𝑷𝒂(𝑷𝒂𝒔𝒄𝒂𝒍)

19. Properties of Solids
Compression: is a stress caused by two forces acting directly toward each
other.
Tension : is a stress caused by two forces acting directly opposite each other.
Shearing: is a stress caused by two forces applied in parallel, opposite
directions.
There are five basic types of stresses:
Torsion: is a stress related to a twisting motion.
Bending: consists of both tension and compression stresses.

20. Properties of Solids
Hooke's Law: One of the most basic principles related to the elasticity of solids is
Hooke's Law.
𝒌 =
𝑭
∆𝒍
𝑵
𝒎
, 𝑭 = 𝒌. ∆𝒍
𝐹 = 𝑎𝑝𝑝𝑙𝑖𝑒𝑑 𝑓𝑜𝑟𝑐𝑒 ∆𝑙= change in length 𝑘 = 𝑒𝑙𝑎𝑠𝑡𝑖𝑐 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡
Example 1: A force of 5 N is applied to a spring whose elastic constant is 0.250 N/cm .
Find its change in length.
Example 2: What is the force required to stretch a spring whose constant value is 100
N/m by an amount of 0.50 m?

21. Properties of Liquids
Surface Tension: is the ability of the surface of a liquid to act like a thin.
Viscosity: is the internal friction of a fluid caused by molecular attraction,
which makes it resist a tendency to flow.
Capillary Action: is the behavior of the liquids that causes the liquid level in
very small-diameter tubes to be different than that in larger-diameter tubes .
• Particles of liquids are tightly packed…
• but are far enough apart to slide over one another.
Liquids have:
• An indefinite shape
• a definite volume.

22. Properties of Gases
Expansion: is a property of a gas in which the rapid random movement of its
molecules causes the gas to completely occupy the volume of its container.
Diffusion: is the process by which molecules of a gas mix with the molecules
of a solid, a liquid, or another gas.
Particles of gases are very far apart.
They move freely and have a lot of energy.
Gases have:
an indefinite shape
an indefinite volume.

23. Properties of Plasma
A plasma is a gas with
charged particles.
A plasma is a very good
conductor of electricity
Plasmas, like gases have
 an indefinite shape
an indefinite volume.

24. Match: (1) solid, (2) liquid, or (3) gas.
__ A. Has a definite volume, but shape of the
container.
__ B. Its particles are moving rapidly.
__ C. Fills the volume of a container.
__ D. Particles are in a fixed structure.
__ E. Particles are close together, but mobile.
Learning Check

25. Density
Density : is the measure of the amount of mas in a given
amount of volume
𝐷 =
𝑚
𝑣
(
𝑔
𝑐𝑚3)
𝑚 = 𝑚𝑎𝑠𝑠 (𝑔) 𝑣 = 𝑣𝑜𝑙𝑢𝑚𝑒 (𝑐𝑚3
)
• Density is the ratio of mass to volume
• If the volume stays the same and the mass increases
. . . the density will increase
• If the mass stays the same and the volume increases
. . . The density will decrease
𝐷 = 𝑑𝑒𝑛𝑠𝑖𝑡𝑦 (
𝑔
𝑐𝑚3)

26. Ex : An ice cube has a volume of 36 𝒄𝒎𝟑. If the ice cube has a mass
of 33.2 g, what is the density of the ice cube?
What is the density of water?
Ex : What is the volume of a silver metal that has a mass of 2500.0 g.
The density of silver is 10.5 g/𝐜𝐦𝟑
Ex : If the density of a diamond is 𝟑. 𝟓 𝒈/𝒄𝒎𝟑 , what would be the
mass of a diamond whose volume is 𝟎. 𝟓 𝒄𝒎𝟑
?
EX.BOOK
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