The change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and work done.
Work done is the energy needed or supplied to perform any task.
The first law of thermodynamics gives the relation between the heat and work done.
The heat added to a system is divide into two. One portion adds up heat to increase the internal energy and the left heat is used to do work.
ΔQ = ΔU + W
ΔU = ΔQ -W
Thus, the first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and work done.
Learn more about work done.
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