Answer :
Answer:
B. adding heat to the system and having the system do work on the surroundings
Explanation:
The internal energy of a system is the energy contained within the system. From first law of thermodynamics we have the equation : dq=du+dw
and we know that energy can neither be created nor destroyed; energy can only be transferred or changed from one form to another therefore du is zero. dq = dw this means that the entire heat supplied is converted into work (on the surroundings)
However, some of the heat supplied is also used to increase the internal energy of the system
The internal energy of a system is always increased by adding heat to the system.
According to the first law of thermodynamics, energy can neither be created nor destroyed but can be converted from one form to another. From the statement of the first law of thermodynamics; E = q + w
E = internal energy of the system
q = heat absorbed/released by the system
w = work done by/on the system
If heat is added to the system q is positive, if heat is removed from the system, q is negative. If the system does work, w is negative, if work is done on the system, w is positive.
From the foregoing, we can agree that the internal energy is increased when heat is added to the system.
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