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What is 1st law of thermodynamics?
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What is 1st law of thermodynamics?
1st Law of Thermodynamics
The First Law of Thermodynamics, also known as the Law of Energy Conservation, is a fundamental principle in physics and chemistry. It asserts that energy cannot be created or destroyed, only transformed from one form to another.
Key Concepts
  • Energy Conservation: The total energy of an isolated system remains constant. When energy is added to a system, it can be transformed into work or heat.
  • Internal Energy: The internal energy of a system is the total energy contained within it, arising from its molecules' kinetic and potential energies.
  • Heat Transfer: Heat (Q) is energy transferred due to temperature differences. It can enter or leave a system, affecting its internal energy.
  • Work Done: Work (W) is energy transferred when a force is applied over a distance. In thermodynamics, work done on or by a system also contributes to changes in internal energy.

Mathematical Representation
The First Law can be mathematically expressed as:
  • ΔU = Q - W
  • Where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system.

Applications
  • Heat Engines: The First Law is fundamental in understanding how heat engines convert thermal energy into mechanical work.
  • Chemical Reactions: It helps in calculating the energy changes during chemical reactions.
  • Refrigeration: The principles of energy conservation are applied in cooling and heating systems.

This law is crucial for analyzing energy systems in various scientific and engineering fields, making it a cornerstone of thermodynamics.
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