Thermodynamics (Physics) — AI Study Guide
Master temperature, heat transfer, ideal gases, and thermodynamic laws from your physics course notes.
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Thermodynamics is the branch of physics dealing with heat, temperature, and their relation to energy and work. Temperature measures the average kinetic energy of particles in a substance. Heat (Q) is energy transferred due to a temperature difference; work (W) is energy transferred by force through displacement. The distinction between heat and temperature is fundamental: two objects at thermal equilibrium have the same temperature but can contain different amounts of internal energy.
The ideal gas law (PV = nRT) relates pressure, volume, amount of gas, and temperature for ideal gases — those whose molecules occupy negligible volume and have no intermolecular attractions. Real gases approximate ideal behavior at high temperature and low pressure. The kinetic theory of gases derives the ideal gas law from molecular motion, connecting macroscopic properties to microscopic behavior. RMS speed (v_rms = √(3RT/M)) gives the characteristic molecular speed.
The laws of thermodynamics: Zeroth law: if A and B are each in thermal equilibrium with C, then A and B are in thermal equilibrium with each other — defining temperature. First law: energy is conserved (ΔU = Q - W). Second law: the entropy of an isolated system cannot decrease (natural processes move toward greater disorder). Third law: the entropy of a perfect crystal at absolute zero is zero — setting the absolute reference for entropy.
Heat engines convert heat into work with efficiency limited by the Carnot efficiency (η_Carnot = 1 - T_cold/T_hot). No real engine can exceed Carnot efficiency for the same temperature reservoirs. Refrigerators and heat pumps run heat engines in reverse. Understanding heat engine cycles (Carnot, Otto for gasoline engines, Diesel) connects thermodynamics to engineering applications.
Frequently Asked Questions: Thermodynamics (Physics)
What is the first law of thermodynamics?
The first law of thermodynamics states that energy is conserved: ΔU = Q - W. The change in internal energy (ΔU) of a system equals the heat added to the system (Q) minus the work done by the system (W). Heat added to a system increases its internal energy; work done by a system decreases its internal energy. This is the energy conservation law applied to thermodynamic systems.
What is entropy?
Entropy (S) is a measure of the disorder or dispersal of energy in a system — quantifying how many microstates (arrangements of particles and energy) are consistent with a macrostate. The second law states that entropy of an isolated system always increases in spontaneous processes (ΔS_universe > 0). Entropy increases with: temperature, volume, number of particles, and transitions from ordered to disordered states. It explains the directionality of natural processes (heat flows from hot to cold, not the reverse).
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