First Law OF Thermodynamics || Calculation OF ΔH ΔU q and w for Different -2 Process || Case 1 Change OF State - (a) ideal Gas (i) Isothermal Process || Reversible and irreversible || Solved Numerical Class illustration

Enthalpy|| Calculation OF deltaH||deltaE||W||q for different Processes||Case OF Ideal gas undergoing change OF state||Isothermal Process||Reversible and Irreversible Process|| Class Illustrations with Short Tricks

Idea OF Entropy || Second Statement OF SLOT || Calculation OF ΔS System ΔS Surroundings and ΔS Universe for Different -2 Process || Case I :-Change OF State OF IG (ideal Gas)

Calculation OF ΔH ΔU q and w for Chemical Reaction and Phase Change || Isothermal and Adiabatic free Expansion

Thermodynamics Process (Types OF Changes) 1)Physical 2)Chemical 3) Change OF State || Thermodynamics Graph Reversible and Irreversible Process

Molar Heat Capacity OF Polytropic Process || Conversion OF Polytropic Process || into other Process || Case II :-Solid/Liquid || Case III :-Real Gas || Solved Numerical Class illustration

Thermodynamic Quantity - Work || Sign Convention || Work for Isobaric || Isochoric || Adiabatic || Isothermal (Reversible and Irreversible) || Phase Charge || Chemical Reaction|| Unit OF Work || Solved Numerical Class illustration

Let Q and W denote the amount of heat given to an ideal gas the work done by it in an isothermal process.

Calculate Delta U , q and w when 2.0 mol of an ideal gas at 25^(@)C are compressed isothermally and reversibly from 1.0 bar to 10.0 bar.

State first law of thermodynamics and state the relation between the change in internal energy (DeltaU) , work done (W) and heat (Q).