Question

If a system absorbs 155.0 kJ of heat from its surroundings and the system does 55.0 kJ of work on its surroundings, what is the change in the internal energy of the system, in kJ?

Answer 1

The change in internal energy of the system is 100.0 kJ, which is the result of the system absorbing 155.0 kJ of heat and performing 55.0 kJ of work on its surroundings.

Step-by-step explanation:

To calculate the change in internal energy of the system, we can use the first law of thermodynamics. This law 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:

ΔU = Q - W

In this scenario, the system absorbs 155.0 kJ of heat from its surroundings (Q = 155.0 kJ) and does 55.0 kJ of work on its surroundings (W = 55.0 kJ). Therefore, the change in internal energy (ΔU) of the system can be calculated as follows:

ΔU = 155.0 kJ - 55.0 kJ = 100.0 kJ

So, the change in the internal energy of the system is 100.0 kJ. This means the system has an increase in internal energy of 100.0 kJ after the interaction with its surroundings.