Is this statement for the First Law of Thermodynamics correct? My Biochemistry book states the First law of Thermodynamics like this:
"The First Law of Thermodynamics states that in a closed system, energy is conserved".
My book defines Closed System as a system which can exchange energy with its surroundings but not matter.
My doubt is how can energy be remain conserved(constant) if the system can exchange energy with its surroundings.
Please clarify.
You can think of the first law of thermodynamics as an energy accounting method. It says that all inputs and outputs of energy should add up to the total change in the energy of a system. The exchanged energy is generally classified as work or heat. By "energy can neither be created nor destroyed," it is meant that nuclear reactions, in which the structure of nuclei changes with accompanying transformation of matter into energy and vice-versa, will not be considered. The reactions considered are ordinary chemical reactions involving making and breaking of chemical bonds resulting from interactions between electrons and nuclei.