States of matter, Changes in states of matter, Measurable properties of gases, Gas Laws

1. STATES OF MATTER & PROPERTIES OF
MATTER
Ms. Punam Dilip Bagad
Assistant Professor, Dept. of Pharmaceutics
GES’s Sir Dr. M. S. Gosavi College of Pharm. Edu. & Research,
Nashik-422005, INDIA
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3. Content as per syllabus
 State of matter, changes in the state of matter,
 Latent heats, vapour pressure, sublimation critical point, eutectic
mixtures,
 Gases, Liquefaction of gases, aerosols– inhalers,
 Relative humidity, liquid complexes, liquid crystals, glassy states, solid
crystalline, amorphous(Methods of crystal analysis: X-Ray Diffraction,
Bragg’s equation)
 Polymorphism (Definition, Different shapes of polymorphs, Example
and its Pharmaceutical applications, Brief introduction of Detection
techniques).
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4. STATE OF MATTER
 Matter is the Stuff of the universe- the atoms, molecules and ions that make-
up all physical substances.
 Matter is anything that has mass and takes up space.
 There are 5 known phases or states:
 Solids
 Liquids
 Gases
 Plasma
 Bose-Einstein Condensates
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5. STATE OF MATTER
 Solid, liquid, and gases are the three primary states of matter or phases.
 The factors which usually determine the state in which matter exists are
 Intensity of intermolecular forces
 Temperature
 Pressure
 Solids have the strongest intermolecular forces and gases have the weakest.
 As the temperature of solid increased, the molecules acquire sufficient
energy to break the ordered structure and pass into the liquid form.
 On further increasing the temperature, liquid changes to the gaseous state.
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6. STATE OF MATTER
 Solid ice, liquid water, water vapor: All 3 states co-exist at the freezing point
of water..
 Solids with high vapor pressures, such as Iodine and Camphor, can pass
directly from the solid to the gaseous state without melting at room
temperature. This process is known as sublimation.
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7. Matter
Pure substances
elements
compounds
Mixture of
substances
Heterogeneous
mixtures
Homogeneous
mixtures
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8. STATE OF MATTER
 A substance is a form of matter that has a constant composition.
 Physicochemical properties of a substance are dependent on the
organizational arrangement of its constituent atoms.
 Example: n-butane and iso-butane (same chemical formula)
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Physical properties n-butane iso-butane
Boiling point 0°C
0°C
Melting point
-138°C -159°C
density 0.622 g/ml 0.604 g/ml

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12. Changes in States of Matter
 Molecular interactions: keep the molecules together while the thermal
energy provides motions to the molecules.
 K.E. based on thermal energy and intermolecular interactions based on
pressure.
 These are responsible for intermolecular forces of attraction and decide
physical state of the substance.
 Intermolecular forces are the forces of attraction between neighbouring
molecules.
 Temperature and pressure decides the physical state of the substance.
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14. STATE OF MATTER
 Changes in the physical state: Changes in the physical state of substance
are reversible in nature
 These are due to rearrangement of the molecules in a substance.
 Changes in the chemical state: Changes in the chemical state are due to
change in specific orientation or arrangement of the atoms and groups of the
substance.
 Changes may be irreversible
 Chemical changes always result in formation of a new compound having
different properties.
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15. Measurable properties of gases
 Characteristics of gases:
1) Mass
2) Volume
3) Temperature
4) Pressure
5) Density
6) Diffusion
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16. Measurable properties of gases
Mass:
 Each gas molecule has characteristic mass
 Mass of single gas molecule is negligibly small,
 Mass of one mole of gas molecule = 6.022*1023
 Mass unit = gm/kg
Volume:
 Gas occupies entire space available to it.
 Volume of gas is the volume of container in which it is stored.
 Unit : cm3/dm3/mL/L
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17. Measurable properties of gases
Pressure:
 It is the force exerted by the gas molecules per unit area on the walls of the
container.
 Pressure measured by using Barometer or Mercury manometers
 Unit: Pascal, N/m2
Density: Mass/Volume
 Unit: Kg/m3
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18. Measurable properties of gases
Diffusion:
 The process of mixing of two or more gases to form homogeneous mixture
is called diffusion.
 The rate at which gases diffuse depends on molar mass of gas
 Lighter gases diffuse faster than heavier gases.
 Unit = cm3/s or dm3/s
 𝑟𝑎𝑡𝑒 𝑜𝑓 𝑑𝑖𝑓𝑓𝑢𝑠𝑖𝑜𝑛 =
𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑔𝑎𝑠 𝑑𝑖𝑓𝑓𝑢𝑠𝑒𝑑
𝑡𝑖𝑚𝑒 𝑟𝑒𝑞𝑢𝑖𝑟𝑒𝑑 𝑓𝑜𝑟 𝑑𝑖𝑓𝑓𝑢𝑠𝑖𝑜𝑛
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19. Measurable properties of gases
Temperature:
℉ =
9
5
℃ + 32
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20. Gas Laws
Boyle’s Law:
 The pressure (P) of a given mass of a gas varies inversely as its volume (V)
at constant temperature.
𝑃 ∝
1
𝑉
PV= K1
Gay- Lussac Law:
Pressure of a given mass of gas varies directly with the temperature at constant
volume.
𝑃 ∝ 𝑇
𝑃
𝑇
= Constant = K2
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21. Gas Laws
Charle’s Law:
Volume of the given mass of the gas is directly proportional to absolute
temperature at constant pressure.
𝑉 ∝ 𝑇
V= K3T
By combining all three equations:
PV=nRT
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