PowerPoint Presentation

[image] of School Adda. Today's Agenda We will explore the following topics: Van der Waals Equation Dalton's Law of Partial Pressures Graham's Law of Diffusion and Effusion Applications of the Kinetic Molecular Theory of Gases.

Van der Waals Equation. The Van der Waals equation introduces corrections to the Ideal Gas Law to account for the non-ideal behavior of real gases. It modifies the equation to include corrections for intermolecular forces and the finite volume of gas particles..

Dalton's Law of Partial Pressures. States that in a mixture of non-reacting gases, the total pressure exerted by the mixture is equal to the sum of the partial pressures of each individual gas in the mixture..

Graham's Law of Diffusion and Effusion. Graham's Law Statement: The rate of diffusion or rate of effusion of a gas is inversely proportional to the square root of its molar mass (M)..

Applications of Kinetic Molecular Theory of Gases.

Graham’s Law of Diffusion of Gases. [image] Divide the above equation by 'ma' Divide the above equation by 'Vb2' Taking square root of equation (4.39) mpN moN.

4.9 LIQUEFACTION OF GAS The process in which the gases are converted to their liquid state by lowering temperature and increasing pressure is called liquefaction of gases. It is impossible to liquefy a gas by pressure alone if the required temperature is not obtained. Critical Conditions: A gas can only be liquefied if it is at or below its critical temperature. Above this temperature, no amount of pressure can liquefy the gas. For carbon dioxide (CO₂):Critical temperature: 31.1°C (87.8°F), Critical pressure: 73.8 atm..

4.9.1 Joule – Thomson Effect When a compressed gas is allowed to enter from a region of high pressure into a region of low pressure, it expands. This sudden expansion causes cooling. This phenomenon is known as Joule – Thomson effect..

Fourth State of Matter; Plasma It is a state in which a gas becomes ionized, meaning that a significant portion of its atoms or molecules are broken apart into charged particles: ions (positively charged) and electrons (negatively charged). Example: Stars: In stars like the Sun, hydrogen gas is ionized into plasma by the extreme heat and pressure in the core. Nuclear fusion occurs within this plasma, which releases energy and sustains the star’s brightness. Lightning: When lightning strikes, the electric discharge heats the air so much that it ionizes, forming plasma. The ionized air allows the electrical current to pass through, creating the visible light and heat associated with a lightning strike..

Micro-Plasma Welding: Micro-plasma welding is a method used for joining paper-thin sheets of metal. It is commonly used in the manufacture of stainless steel, water storage tanks, and kitchen equipment. Plasma Spray: Plasma spray is used to coat various materials, enabling the coating of any material onto any surface. Some common applications include: Metal onto metal: For example, titanium onto steel to prevent corrosion. Metal onto non-metal: Copper onto porcelain (used in capacitors). Non-metal onto metal: Alumina onto stainless steel (to reduce wear and corrosion). Non-metal onto non-metal: Teflon onto ceramics (to prevent corrosion from acids)..

[image] of School Adda. Today's Agenda We will explore the following topics: Kinetic molecular interpretations of Liquids Simple properties of Liquids Intermolecular forces 3.1. Hydrogen bonding.

STATE OF MATTER – II LIQUID. [image]. The state of matter, which has definite volume but no definite shape is called Liquid..

Molecular Forces. Intramolecular Forces The attractive forces within a molecule of a liquid are called intramolecular forces. e.g. Covalent bond, Co-ordinate covalent bond etc. Intermolecular forces The attractive forces among the molecules of a substance are called intermolecular forces. e.g. Hydrogen bonding , dipole-dipole interactions and London dispersion forces..

Dipole-Dipole Interaction. The attractive forces between the positive pole of one polar molecule and negative pole of other polar molecule are called diploe-dipole forces..

Hydrogen Bonding Force of attraction between partially positive charged hydrogen atom which is covalently bonded to a small size, high electronegative (F, O, N) and active lone pair of another electronegative atom (F, O, N) is called Hydrogen bonding..

[image] 150 100 50 ? —50 -100 —150 —200 H20 H2Se HBr SiH, Period Fig. 5.2: A graph between period number and the boiling points of hydrides.

APPLICATIONS OF HYDROGEN BONDING. Acidic Strength: H-F, H-Cl, H-Br, H-I Solubility: Ethyl alcohol is soluble in water DNA Structure: Role of Hydrogen Bonds: Hydrogen bonding between nitrogenous bases holds the two strands of the DNA double helix together. Base Pairing: Adenine (A) forms two hydrogen bonds with Thymine (T) in DNA. Guanine (G) forms three hydrogen bonds with Cytosine (C).These hydrogen bonds are specific and ensure complementary base pairing, which is critical for accurate DNA replication and transcription. Protein Structure: Secondary Structure: In proteins, hydrogen bonds stabilize the alpha-helix and beta-sheet structures. Tertiary and Quaternary Structures: Hydrogen bonds between side chains of amino acids contribute to the folding and stability of the three-dimensional structure of proteins. Significance of Ice's Structure: The ability of ice to float is crucial for the survival of aquatic ecosystems. Ice insulates the water below, preventing complete freezing in cold climates and allowing organisms to survive..

London Dispersion Forces. London dispersion forces (also known as dispersion forces or van der Waals forces) are weak intermolecular forces that arise due to temporary dipoles in atoms or molecules. Origin of London Dispersion Forces: Electrons in motion Induced dipoles Attractive force.

Vapours Pressure. The pressure exerted by the vapours of the liquid when the rate of evaporation becomes equal to rate of condensation. In the beginning, rate of evaporation is greater than rate of condensation, but after sometime both the rates become equal and a dynamic equilibrium is establishes as shown in the below figure The magnitude of vapour pressure does not depend upon the amount of liquid in container, It depend upon the surface area of liquid..

Boiling Point. The temperature at which the vapour pressure of a liquid becomes equal to atmospheric pressure or some other external pressure is called boiling point..

Surface Tension. Surface tension is the force per unit length acting along the surface of a liquid at rest, due to the imbalance of intermolecular forces at the interface between the liquid and another phase (e.g., air or another liquid). It is measured in units of Nm-1 Surface tension of liquid depends on: Intermolecular forces Temperature.