Thermodynamics
- Zeroth Law of Thermodynamics: If two systems are in thermal equilibrium with a third system, then they are in thermal equilibrium with
each other. - First Law of Thermodynamics: The change in internal energy of a system is equal to the heat added to the system minus the work done by
the system. - ΔU = Q - W
- Second Law of Thermodynamics:
It is impossible to construct a heat engine that operates with 100% efficiency. - Kelvin-Planck Statement: No heat engine can convert all the heat absorbed from a reservoir into work.
- Clausius Statement: Heat cannot be transferred from a colder body to a hotter body without work being done.
- Third Law of Thermodynamics: It is impossible to reach absolute zero temperature.
- Thermodynamic Processes:
- Isothermal: Temperature remains constant.
- Adiabatic: No heat exchange with surroundings.
- Isobaric: Pressure remains constant.
- Isochoric: Volume remains constant.
- Carnot Cycle: A theoretical cycle that represents the maximum possible efficiency for a heat engine.
- Efficiency = 1 - (T₁/T₂)
Kinetic Theory of Gases
- Ideal Gas Law: PV = nRT
- P: Pressure
- V: Volume
- n: Number of moles
- R: Gas constant
- T: Temperature
- Kinetic Energy of a Gas Molecule: KE = (3/2)kT
- k: Boltzmann constant
- Root Mean Square (RMS) Speed of Gas Molecules: v_rms = √(3RT/M)
- M: Molar mass
- Mean Free Path: Average distance traveled by a gas molecule between collisions.
- λ = (1/√2) * (Ï€d²/n)
- d: Diameter of gas molecule
- Maxwell-Boltzmann Distribution: Describes the distribution of molecular speeds in a gas.
- Specific Heat Capacity: Amount of heat required to raise the temperature of a unit mass of a substance by 1 degree Celsius.
- Cv: Specific heat capacity at constant volume
- Cp: Specific heat capacity at constant pressure
- Cp - Cv = R
Important Formulas:
- Work done by a gas: W = ∫PdV
- Heat added to a gas: Q = ΔU + W
- Internal energy of a gas: U = (3/2)nRT
Remember:
- Practice solving numerical problems.
- Understand the concepts and their applications.
- Review key formulas and their derivations.