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Answers
Answer:
• Ion-induced Dipolar Interactions. ...
• London Forces or Dispersion Forces. ...
• Boyle's Law (Pressure-Volume Relationship) ...
Charles' law: At constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature.
• Gay Lussac's Law (Pressure-Temperature Relationship) ...
• Ideal Gas Equation.
Explanation:
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Explanation:
Hitherto five states of matter are known, viz, solid, liquid, gas, plasma and Bose-Einstein condensate. Out of these solid, liquid and gas are commonly found while remaining two are found only under specific
conditions.
Interconversion of States of Matter
These stateS are interconvertible.
(i) Melting point This is the temperature at which a matter converts from its solid state to liquid state. It decreases in the presence of impurity.
(ii) Boiling point This is the temperature at which the vapour” pressure of a liquid becomes equal to the atmospheric pressure. It increases in the presence of impurity and with rise in pressure. Boiling point of water is 100°C.
(iii) Freezing point At this temperature, a matter converts from its fluid state into solid state.
Freezing point of water is 0°C.
(iv) Evaporation It is the process of conversion of a liquid into vapours at any temperature.
Due to evaporation,
(a) water droplets appear on the outer surface of a glass containing ice-cold water.
(b) water kept in earthen pot becomes cool during summer.
(c) desert cooler cool better on a hot dry day.
In short,
The temperature and pressure at which all the three states of a substance can exist together in equilibrium is called triple point, e.g.,
ice, liquid water and water vapours can coexist
(i. e., ice ⇔ water ⇔ vapour) at 0.0098°C and 4.58 mm.
Plasma
It is a state of matter similar to gas in which a certain portion of the gaseous particles are ionised. Because of the average strength of the electrical forces, the plasma is neutral. It is commonly found in the universe.
On earth, plasma is naturally occurring in flames, lightnings and the auroras.
Bose-Einstein Condensate
A Bose-Einstein condensate is a gaseous superfluid phase formed by atoms cooled to temperature very near to absolute zero.
This state was first predicted by Satyendra Nath Bose and Albert Einstein in 1924-25. Such first condensate was produced by Eric Cornell and Carl Wieman in 1995. It can be thought of as the opposite of a plasma.
Factors Deciding Physical State of a Substance
For gaseous state,
Forces of attraction << thermal energy For liquid state, Forces of attraction > Thermal energy
For solid state,
Forces of attraction >> Thermal energy
Intermolecular Forces
The forces of attraction existing among the molecules of a substance (gaseous, liquid or solid) are called intermolecular forces
[Greater the intermolecular forces, higher is the melting and boiling point.
Attractive intermolecular forces are known as van der Waals’ forces.]
The different types of intermolecular forces are briefly explained below
(i) Dipole-dipole interactions Dipole-dipole forces act between the molecules possessing permanent dipoles.
The interaction is stronger than London forces and weaker than ion-ion interaction.
(ii) Dipole-induced dipole forces Dipole-induced dipole forces act between the polar molecules having permanent dipole and the molecules lacking permanent dipole
(iii) Dispersion forces or London forces Dispersion forces or London forces are present among non-polar atoms and molecules, e.g., among the atoms or chlorine molecules. These are the weakest intermolecular forces. These forces increases with
(i) increase in number of electrons in molecules,
(ii) increase in molecular size
The Gaseous State
This is the simplest state of matter. Characteristics of this ‘state of matter are
In gases, the intermolecular forces are weakest.
Gases are highly compressible.
Gases exert pressure equally in all directions.
Gases have much lower density than the solids and liquids.
The volume and the shape of gases are not fixed.
Gases mix evenly and completely in all proportions without any mechanical aid.
Measurable Properties of Gases
(i) Mass It is expressed in gram or kg.
(ii) Volume It is equal to the volume of the container and is expressed in terms of litre (L), millilitre (mL), cubic centimetre (cm3), cubic metre (m3) or cubic decimetre (dm3).
1 L = 1000 mL = 1000 cm3 = 1 dm3
1 m3 = 103 dm3 = 106 cm3 = 106 mL = 103L
(iii) Pressure Gas pressure is measured with manometer and atmospheric pressure is measured by barometer.
1 atm = 76 em of Hg = 760 mm of Hg = 760 torr
1 atm = 101.325 kPa = 101325 Pa = 101.325 Nm-2 = 1.01325 bar
1 bar = 105 Pa.
Measurement of pressure of gas
(i) Open end manometer, pgas = patom – h
(ii) Closed end manometer, pgas = h
where h is difference in the mercury levels in the two columns of density (d) (of a gas).
(iv) Temperature It is measured in celsius scale (OC) or in Kelvin scale (K). SI unit of temperature is kelvin (K), T (K) = t°C+ 273