Answer :
Final answer:
The change in internal energy of the system is -76.8 Joules, meaning the internal energy of the system decreased by this amount.
Explanation:
We will use the first law of thermodynamics. This law states that the change in internal energy (ΔU) of a system equals the heat added to the system (Q) minus the work done by the system (W).
So, ΔU = Q - W.
By the provided problem, the work is equal to 41.0 J (meaning the system has done work and thus exerted energy), and the heat is -35.8 J, representing energy that exited the system.
Using these values in the formula, the change in internal energy (ΔU) is
ΔU = (-35.8 J) - (41.0 J) = -76.8 J.
Thus, the change in the system's internal energy is -76.8 Joules, which means the system's internal energy has decreased by 76.8 Joules.
Learn more about First Law of Thermodynamics here:
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