Thermodynamics Chemistry class 11 | Chapter 6

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Timestamps:-
0:00 Introduction
0:42 Thermodynamics
2:42 Macroscopic Vs Microscopic
4:30 Limitations:Thermodynamics
6:30 System & Surroundings
7:57 System:Types
9:47 Thermodynamic Process
11:48 State of System
12:57 State Vs. Path Func
15:36 Internal Energy
19:38 Internal Energy:By Work
23:09 Adiabatic Work
24:26 Internal Energy:By Heat
27:05 Internal Energy:Heat & Work
29:09 Internal Energy: P,V& W
37:29 Single Vs Gradual
39:20 Reversible vs. Irreversible process
40:55 P,V&T:Reversible
44:57 Reversible & Irrever.Exp.
47:07 Reversible Vs. Irreversible
48:08 Free Exp. Gas
50:45 Ist law Equ.
52:07 Ex 1
55:58 Enthalpy
59:33 ∆H & ∆U
1:00:28 ∆H:Gases
1:02:57 Ex 2
1:06:05 Extensive & Intensive
1:07:59 Heat Vs.Specific

Thermodynamics is a branch of physics that deals with heat, work, and temperature, and their relation to energy, radiation, and physical properties of matter.In chemistry and physics, internal energy (U) is defined as the total energy of a closed system.In thermodynamics, an adiabatic process is a type of thermodynamic process which occurs without transferring heat or mass between the system and its surroundings. Unlike an isothermal process, an adiabatic process transfers energy to the surroundings only as work.The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic processes, distinguishing two kinds of transfer of energy, as heat and as thermodynamic work, and relating them to a function of a body's state, called Internal energy.

The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed.

In this video we will cover -
1.Why to study Thermodynamics?
2.Macroscopic Vs. Microscopic
3.Scope & Limitation:Thermodynamics
4.What is system abd surroundings?
5.Types of System.
6.What is thermodynamic Process?
7.What is state of system?
8.State Function Vs. Path Function
9.What is Internal energy(U)?
10.Internal energy change by work
11.What is adiabatic work?
12.Internal energy change by heat
13.Change in internal energy by heat and work.
14.Change in internal energy by Pressure,Volume and Work
15.Single step vs. Gradual Change
16.Reversible & Irreversible expansion.
17.Difference between irreversible and reversible process.
18.Work done in Free Expansion of Gas.
19.Points to remember.
20.ist Law equation for Isothermal Reversible & Irreversible changes
21.Two litres of an ideal gas at a pressure of 10 atm expands isothermally in vacuum until its total volume is 10 litres. How much heat is absorbed in the expansion?
22.Why Enthalpy?
23.∆U and ∆H.
24.Enthalpy:Formula for Gasses.
25.If water vapour is assumed to be a perfect gas, molar enthalpy change for vapourisation of 1 mol of water at 1bar and 100°C is 41kJ mol-1. Calculate the internal energy change, when (i) 1 mol of water is vaporised at 1 bar pressure and 100°C.
(ii) 1 mol of water is converted into ice.
26.Extensive & Intensive Properties.
27.Heat Capacity vs. Specific Heat

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