first law of thermodynamics
Answers
Explanation:
First law of Thermodynamics :-
→ According to this La energy can neither be created nor be destroyed. So you in any physical or chemical process Total energy of universe is constant .
°•° ∆U = q + W.
Answer:
The first law, also known as Law of Conservation of Energy, states that energy cannot be created or destroyed in an isolated system.
Explanation:
Formula
Δ U = Q - W
Δ U = change in internal energy
Q = heat added
W = work done by the system
For example, turning on a light would seem to produce energy; however, it is electrical energy that is converted.
A way of expressing the first law of thermodynamics is that any change in the internal energy (∆E) of a system is given by the sum of the heat (q) that flows across its boundaries and the work (w) done on the system by the surroundings:
This law says that there are two kinds of processes, heat and work, that can lead to a change in the internal energy of a system. Since both heat and work can be measured and quantified, this is the same as saying that any change in the energy of a system must result in a corresponding change in the energy of the surroundings outside the system. In other words, energy cannot be created or destroyed. If heat flows into a system or the surroundings do work on it, the internal energy increases and the sign of q and w are positive. Conversely, heat flow out of the system or work done by the system (on the surroundings) will be at the expense of the internal energy, and q and w will therefore be negative.