Gaseous, liquid and solid phase of matter.

1. STATES OF
MATTER

3. PHASE CHANGES

4. PHASE CHANGES
X(s) + heat  X(l) (melting, endothermic)
X(l)  X(s) + heat (freezing, exothermic)
X(l) + heat  X(g) (evaporation, endothermic)
X(g)  X(l) + heat (condensation, exothermic)
X(s) + heat  X(g) (sublimation, endothermic)
X(g)  X(s) + heat (decomposition, exothermic)
Endothermic process: Heat energy is
absorbed. Heat (Q) is shown in
reactant side on a chemical equation.
Exothermic process: Heat energy is
released. Heat (Q) is shown in product
side on a chemical equation.

5. Gets weaker
Evaporation
Endothermic
Increases

6. Difference
between boiling
and evaporation
?

7. WATER CYCLE

8. GASES
The particles of a gas
are relatively apart and
they are in a totally
random motion.
The intermolecular
forces between gas
particles are so small
that each molecule
moves freely.

9. PRESSURE
Pressure =
𝐹𝑜𝑟𝑐𝑒
𝐴𝑟𝑒𝑎
 P =
𝐹
𝐴
Atm Torr (mmHg) Bar Milibar(mbar) Pa
1 atm 1 760 1,013 1013 101325
- Gas pressure are most commonly expressed by chemists in units of atm
or mmHg.

10. PRESSURE

11. VOLUME
• Volume of gases can be
generally stated in unit cm3
(mL) and Liter (L )
•
1 cm3 = 1 mL
•
1 L = 1000 mL = 1 dm3

12. TEMPERATURE

13. Freezing Point of
water
Boiling point of
water
Fahrenheit scale 32 F 212 F
Celsius scale 0 C 100 C
Kelvin scale 273 K 373 K
T(C) = (F -32) / 1,8
T(K) = t(C) + 273
0 K or -273C is known as absolute zero.

14. TEMPERATURE
• Convert
a) 127C to K b) 233 K to C c) 100 C to F d) 32 F to C
• Solution:
• a) 127 C + 273 = 400 K b) 233 K – 273 = - 40 C
• c) 100C = (F -32) / 1,8 → 212 F d) T(C) = (32F -32) / 1,8 = 0 C

15. AMOUNT (MOLE)
• 1 mole of substances includes
6,02 x 1023 particles.
•
• 6,02 x 1023 = Avogadro’s
Number (NA)
• mole (n) =
𝒎𝒂𝒔𝒔 (𝒈)
𝑴𝒐𝒍𝒂𝒓 𝒎𝒂𝒔𝒔 (𝒈/𝒎𝒐𝒍𝒆)

16. GAS LAWS
As T (in Kelvin) increases, average kinetic energy increases.

17. 1) BOYLE- MARIOTTE LAW

18. BOYLE’S LAW
P x V
P
Volume and pressure are
inversely proportional
P x V is always constant at
constant T.

19. BOYLE’S LAW

20. CHARLES’S LAW
• Charles’ Law states that temperature (in Kelvin) and volume of a gas are directly
proportional to each other at constant pressure and number of mole
V = kT 
𝑽
𝑻
= k
(constant)
For a gas sample at constant P,
when two different conditions of
volume and temperature are
compared, we can write a
relation as given aside:

21. CHARLES’S LAW
 V and T are directly proportional
at constant P and n
 -273.15 C or 0 K is absolute zero

22. CHARLES’S LAW

23. GAY- LUSSAC’S LAW
• Temperature and pressure of a gas are
directly proportional to each other when
number of mole and volume of the gas are
kept constant
P  T or P = kT 
𝑷
𝑻
= k (constant)
- For a gas sample at constant
volume, when two different
conditions of pressure and
temperature are compared,
we can write a relation as
given aside

24. GAY-LUSSAC’S LAW

25. AVOGADRO’S LAW
• Volume of a gas is directly proportional to number of moles of the gas when pressure
and temperature are kept constant.
The relation for a gas at
two different volume and
mol number conditions
at constant T and P:
V a T or V = kn (k is constant)
According to Avogadro’s Law: “Equal volumes of different gases contain the same number of
molecules.”

27. COMBINED GAS EQUATION