First Law of Thermodynamics

The First Law of Thermodynamics, also known as the law of energy conservation, states that the change in internal energy of a system (ΔU) is equal to the heat added to the system (Q) minus the work done by the system (W). It's a statement about the conservation of energy, which suggests that energy can neither be created nor destroyed, but it can be transferred from one form to another.

In this formula, ΔU is the change in internal energy of the system, Q is the amount of heat added to the system, and W is the amount of work done by the system. The result is expressed in Joules or any other unit of energy. Practical applications of this formula include a wide range of engineering problems, chemical reactions, and physical processes where energy conservation plays a crucial role.