54 kJ of heat was absorbed by a system, whilst also having 33 kJ of work done by it. What is the change in the internal energy of this system after these processes?

Question

BlackTom AI · Accepted Answer

The problem describes a thermodynamics scenario where a system absorbs heat and does work on its surroundings. According to the first law of thermodynamics, the change in internal energy is given by ΔU = Q − W, where Q is the heat added to the system and W is the work done by the system (positive when the system does work). Here, Q = 54 kJ (heat absorbed) and W = 33 kJ (work done by the system). Substituting these values: ΔU = 54 kJ − 33 kJ = 21 kJ.

Thus, the internal energy increases by 21 kJ. Since the answer options are not provided in the question data, there is no selectable choice to map this result to within the given options. The key idea is applying ΔU = Q − W with the given sign conventions to obtain the net change in internal energy.

MUF0121 Physics Unit 1 - Semester 2, 2025

54 kJ of heat was absorbed by a system, whilst also having 33 kJ of work done by it. What is the change in the internal energy of this system after these processes?

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