state and explain first law of thermodynamics?
Answers
Answer:
The First Law of Thermodynamics states that heat is a form of energy, and thermodynamic processes are therefore subject to the principle of conservation of energy. This means that heat energy cannot be created or destroyed.
Explanation:
The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic systems. The law of conservation of energy states that the total energy of an isolated system is constant; energy can be transformed from one form to another, but can be neither created nor destroyed. The first law is often formulated[1][nb 1]
{\displaystyle \Delta U=Q-W.} {\displaystyle \Delta U=Q-W.}
It states that the change in the internal energy ΔU of a closed system is equal to the amount of heat Q supplied to the system, minus the amount of work W done by the system on its surroundings. An equivalent statement is that perpetual motion machines of the first kind are impossible.
Answer:
The net heat supplied to a system is equal to the net workdone by the system on its surroundings
Explanation:
ΔU = Q− W