Question

suppose there is heat transfer of 60.00 j to a system, while the system does 12.00 j of work. later, there is heat transfer of 25.00 j out of the system while 4.00 j of work is done on the system. what is the net change in internal energy of the system?

Answer 1

The net change in internal energy of the system is calculated using the first law of thermodynamics and amounts to 27.00 J after accounting for heat transfer and work done during two separate processes.

Step-by-step explanation:

To calculate the net change in internal energy of the system, we use 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. This is expressed as ΔU = Q - W. In this scenario, we have two separate processes:

• First, there is a heat transfer of 60.00 J to the system, and the system does 12.00 J of work. So for this process, ΔU = 60.00 J - 12.00 J = 48.00 J.
• Second, there is a heat transfer of 25.00 J out of the system (which is negative since it is leaving the system), and 4.00 J of work is done on the system. For this process, ΔU = -25.00 J + 4.00 J = -21.00 J.

To find the total change in internal energy, we add up the changes from both processes: Total ΔU = 48.00 J + (-21.00 J) = 27.00 J.

Therefore, the net change in internal energy of the system is 27.00 J.