According to the First Law of Thermodynamics, what is the relationship between internal energy (U), heat (Q), and work (W)?

According to the First Law of Thermodynamics, energy can only be moved or transformed; it cannot be created or destroyed. This can be stated mathematically as:

Δ𝑈 = 𝑄 − 𝑊

  • ΔU represents the change in the internal energy of the system.
  • Q is the heat added to the system.
  • W is the work done by the system on its surroundings.

This law links changes in internal energy to heat and work, emphasizing energy conservation.

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