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Answer :
Final answer:
The change in internal energy for the system that absorbs 196 kJ of heat and has 117 kJ of work done on it by the surroundings is 313 kJ.
Explanation:
the change in internal energy of a system based on the first law of thermodynamics, which states that the change in internal energy (ΔU) of a system is equal to the heat (Q) added to the system minus the work (W) done by the system on its surroundings.
Given that the system absorbs 196 kJ of heat and the surroundings do 117 kJ of work on the system, we calculate ΔU as:
ΔU = Q - W
ΔU = 196 kJ - (-117 kJ) (Note: Work done on the system is considered negative as per sign convention)
ΔU = 196 kJ + 117 kJ
ΔU = 313 kJ
Thus, the change in internal energy of the system is 313 kJ.
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Rewritten by : Brahmana