The first law of thermodynamics states that ΔE = Q - W. Is this also a statement of the principle of conservation of energy? Yes, the heat added and the change in internal energy of the gas equal the work done by the piston. No, the change in internal energy is the energy lost in the system. Yes, the heat that flows into the system is used to change the internal energy of the gas and becomes work done by the piston. No, the heat that is added to the system is only used to do work.

Yes, the heat that flows into the system is used to change the internal energy of the gas and becomes work done by the piston.

Explanation:

First law of thermodynamics known as Law of Conservation of Energy, states that energy can neither be created nor destroyed; energy can only be transferred or changed from one form to another.

The first law of thermodynamics states that the change in internal energy of a system equals the net heat transfer into the system minus the net work done by the system. In equation form, the first law of thermodynamics.

This is the first law of thermodynamics

ΔE = Q - W

ΔE = change internal energy of the system.

Q = heat transfer into the system

And

W = work done by the system.

Rewriting the equation

ΔE = Q - W

Q=ΔE + W

Show that the heat flowing l into the system is transferred to the internal energy of the system and the work done by the piston

So the third option is correct