The value of ΔE for a system that performs 168 kJ of work on its surroundings and loses 79 kJ of heat is __________ kJ.

Question

Quizplus · Accepted Answer

According to the first law of thermodynamics, the change in internal energy (ΔE) of a system is equal to the heat (q) absorbed by the system minus the work (w) done by the system: ΔE = q - w.
Substitute the given values: ΔE = -79 kJ - 168 kJ = -247 kJ.
The negative sign indicates that the system has lost energy (exothermic process), and the absolute value of 247 represents the magnitude of that energy loss. Therefore, the answer is B.

The Value of ΔE for a System That Performs 168