Final answer:
The change in internal energy (ΔE) for the surroundings is 156.0 kJ, which is obtained by summing the heat produced by the system (111.0 kJ) and the work done by the system on the surroundings (45.0 kJ).
Step-by-step explanation:
To calculate the change in internal energy (ΔE) for the surroundings, we need to consider the first law of thermodynamics which states that the change in internal energy of a system is equal to the heat transferred to the system (q) minus the work done by the system (w). However, we are asked about the surroundings, so we must take the opposite signs of heat and work since the system's loss is the surroundings' gain and vice versa.
In this case, the system produces 111.0 kJ of heat and does 45.0 kJ of work on the surroundings. Therefore, the surroundings absorb 111.0 kJ of heat and have work done on them by the system equivalent to 45.0 kJ. To calculate the change in internal energy (ΔE) for the surroundings, we add the heat absorbed by the surroundings to the work done on the surroundings:
ΔE = q + w
ΔE = 111.0 kJ + 45.0 kJ
ΔE = 156.0 kJ
Thus, the change in internal energy (ΔE) for the surroundings is 156.0 kJ.