RBSE Class 11 Chemistry Notes Chapter 5 States of Matter

These comprehensive RBSE Class 11 Chemistry Notes Chapter 5 States of Matter will give a brief overview of all the concepts.

RBSE Class 11 Chemistry Chapter 5 Notes States of Matter

→ Intermolecular Force: Intermolecular forces are those which mediate interaction between molecules, including force of attraction or repulsion which act between molecules and other type of neighbouring particles e.g., atoms or ions. 

→ Keesom Force: Dipole-dipole force is known as Keesom force. It occurs between polar molecules.

→ London Force: It is instantaneous induced dipole- induced dipole interaction and exists between non¬polar molecules.

→ Debye Force: It is dipole induced interaction and produced between polar and non-polar molecules.

→ Thermal Energy: It is the energy of a body arising from motion of its atoms or molecules.

→ Atmospheric Pressure: Due to gravitational force, the gases present in atmosphere are pulled towards earth and exert pressure on the surface of earth. This amount of exerted pressure is called atmospheric pressure.

→ Temperature: It is measurement of hotness or coldness of any substance.

→ Boyle’s law: It states that under isothermal condition, pressure of fixed amount of a gas is inversely proportional to its volume.

→ Charles’ law: It states that at constant pressure, the volume of a fixed mass of a gas is directly proportional to its absolute temperature.

→ Critical Temperature: 273°C (or - 273.15°C) is an imaginary temperature at which volume of gas becomes zero.

→ Gay Lussac’s law: It states that at constant volume, pressure of a fixed amount of gas varies directly with temperature.

→ Avogadro’s law: It states that equal volume of all gases under the same condition of temperature and pressure contain equal number of molecules.

→ Standard Temperature and Pressure (STP):
273.15 K, temperature and 1 bar, pressure is known as ST.

→ Ideal gas: Gas which obeys Boyle’s law, Charles’ law and Avogadro’s law at all temperatures and pressures, is called ideal gas.

→ Dalton’s law of partial pressure: It states that the total pressure exerted by the mixture of non reactive gases is equal to the sum of the partial pressure of individual gases.

→ Aqueous tension: Pressure of water vapour is called aqueous tension.

→ Diffusion: Gases have tendency to spread out evenly in available space. This property of gases is known as diffusion.

→ Effusion: It is the process of escaping out gas molecule through a tiny pore.

→ Graham’s law of Diffusion: According to this, the rate of effusion or diffusion of a gas is inversely proportional to square root of its molecular weight or at fixed temperature and pressure, the rate of diffusion of any gas is inversely proportional to its vapour density.

→ Maxwell’s Generalisation: The kinetic energy of 1 mol of ideal gas is directly proportional to its absolute temperature i.e., kinetic energy is independent of nature of gas. .

→ Average Speed: In a model of gas, the average speed of all molecules present in it is called average speed.

→ Most probable Speed: It is a speed obtained by maximum number of molecules present in a model of gas.

→ Boyle’s temperature: The temperature at which real gas obeys ideal gas law over an appreciable range of pressure.

→ Root Mean Square Speed: It is the average of square of speed of all molecules present in a sample of gas.

→ Critical Temperature: The maximum temperature at which any gas can be converted to liquid .state. Above this temperature, liquification of gas is not possible even pressure is increased to maximum extent.

→ Critical Pressure: It is minimum amount of pressure to liquify any gas at its critical temperature.