Final answer:
The change in the internal energy of the system is 150 J.
Step-by-step explanation:
The change in the internal energy (ΔE) of a system can be calculated using the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system:
ΔE = Q - W
In this case, the system receives 575 J of heat (Q = 575 J) and delivers 425 J of work (W = 425 J). Plugging these values into the equation, we get:
ΔE = 575 J - 425 J = 150 J
Therefore, the change in the internal energy of the system is 150 J (option c).
The change in the internal energy (ΔE) of a system is determined by the first law of thermodynamics, which is given by the formula ΔE = Q - W, where Q is the heat added to the system and W is the work done by the system.
In the given scenario, the system receives 575 J of heat and delivers 425 J of work. Applying the formula: ΔE = 575 J - 425 J, we get ΔE = 150 J.