State of matter

1. IIIrd Semesester B. pharmacy
Physical Pharmaceutics-I
Unit-III
Sublimation Critical Point
Student Name:
Gokul Daulat Ugale
Roll No.: 57(DSP)

2. ❑ Gases
• Gases are compressible fluid and has no definite shape.
• Properties of gases:
1. Asample of gas assumes both the shape and volume of the container.
2. Gases are compressible.
3. The densities of gases are much smaller than those of liquid and highly
variable depending on temperature and pressure.
4. Gases form homogeneous mixture (solution) with one another in any
proportion.

3. Kinetic Molecular Theory of Ideal Gases:
1. The volume occupied by the individual particles of a gas is negligible
compared to the volume of the gas itself/.
2. The particles of an ideal gas exert no attractive forces of each other or on
their surroundings.
3. Gas particles are in constant state of random motion and move in straight
lines until they collide with another body.
4. The collision exhibited by gas particles are completely elastic; when two
molecules collide, total kinetic energy is conserved.
5. The average kinetic energy of gas molecules is directly proportional to
absolute temperature only; this implies that all molecular motion ceases if
the temperature

4. ❖The Gas laws:
1. Boyle’s Law ( The Pressure – Volume relationship) : This law states
that the volume of a fixed amount of gas at a constant temperature is
inversely proportional to the gas pressure.
The pressure volume relationship.
Robert Boyle, in 1662
V α 1/P
V = k/P
For a given sample of gas under two different sets of condition at constant
P1 V1 = P2 V2

6. 2. Charles’s law( The Temperature- Volume
relationship)
• Charles in 1787 investigated that the gas such as hydrogen, carbon and
oxygen expand to an equal amount upon heating from 0°C to 80°C at
constant pressure .However, Gay-Lussac in 1802 showed that volume of all
gases increases with each 1°C was approximately equal to 1/273.15 volume
of gas at 0°C

7. • Charles’s law state that the pressure of a fixed amount of gas at a
constant at a fixed pressure, the volume of gas is proportional to
temperature of gas.
Vα T
V = kT
For a given sample of gas under two different sets of condition at constant
V1 /T1 = V2 / T2 = K
• At any given pressure, the plot of volume vs temperature. Yields a
straight line.
• The temperature increases, the gas expand ( volume increases )
• The temperature decreases, the gas expand ( volume decreases)

8. 3. Gay- Lussac’s law( The Pressure- Temperature
relationship
• This law is a special case of ideal gas law. This law applies to ideal
gases held at a constant volume allowing only the pressure and
temperature to change.
P1 / T1 = P2 / T2

9. 3. Avogadro’s Law ( The Volume – Amount
relationship
• Amedeo Avogadro- complemented the studies of Bolyle, Charles and
Gay- Lussac. He published a hypothesis that started:
• At the same temperature and pressure, equal volume of different gases
contain the same number of molecules.
• The Volume of any given gas must be proportional to the number of
molecules present

10. • Avogadro law : this law states that the volume of a sample gas is
directly proportional the number of moles in the sample at constant
temperature and pressure.
Vα n
Or, V1 / n1 = V2 / n2

11. 1. Boyles Law = Vα
1
𝑃
( constant temperature)
2. Charles’s Law = Vα T ( constant pressure )
3. Avogadro’s Law = Vα n ( constant temperature and pressure)
GAS LAW

13. • The ideal gas law relates to the volume and pressure of a gas at constant
temperature. On combining Boyle’s law, Charles’s law, Gay- Lussac law and
Avogadro’s law we find that the volume of gas depends on pressure,
temperature and number of moles of gas in the container.
• Summary:
Boyle’s Law : V α 1
𝑃
Charles’s Law: V α T
( when n and T are held constant)
(when n and P are held constant)
Avogadro’s Law: V α T (when P and T are held constant)
❖Ideal Gas Law:

14. • Therefore, volume should be proportional to the product of these three
term as:
V α 1
x T x n
𝑃
• Replacing proportionality symbol (α) with equal to symbol (=) and adding
the proportionality constant (R), we get;
𝑃
V = R x 1
x T x n
PV = nRT
Where, P represent pressure of the gas
V represent volume of the gas
n represent number of moles of the gas
R represent molar gas constant which is always 0.08205 L atm/K.moles
T represent the temperature of the gas.