Final answer:
The system lost 105.15 kJ of energy as heat, calculated using the first law of thermodynamics with a given internal energy increase and the work done on the system.
Step-by-step explanation:
To find the amount of energy lost as heat in the system, we can use the first law of thermodynamics, which is expressed as ΔU = Q - W, where ΔU is the change in internal energy of the system, Q is the heat transfer into or out of the system, and W is the work done on or by the system. In this case, the internal energy increased by 57.12 kJ, which means ΔU is +57.12 kJ, and 162.27 kJ of work was done on the system, so W is -162.27 kJ (negative because work is done on the system). Solving for Q gives us Q = ΔU + W = 57.12 kJ + (-162.27 kJ) = -105.15 kJ. Therefore, the system lost 105.15 kJ of energy as heat.