If a system does 150 J of work on the surroundings and absorbs 100 J of heat, wh

If a system does 150 J of work on the surroundings and absorbs 100 J of heat, what is the change in internal energy?

If a system does 150 J of work on the surroundings and absorbs 100 J of heat, what is the change in internal energy?

Step 1: Identify the work done by the system on the surroundings. In this case, it is 150 J.
Step 2: Identify the heat absorbed by the system. Here, it is 100 J.
Step 3: Recall the formula for the change in internal energy (ΔU) which is ΔU = Q - W.
Step 4: Substitute the values into the formula. Q (heat absorbed) is 100 J and W (work done) is 150 J.
Step 5: Calculate ΔU: ΔU = 100 J - 150 J.
Step 6: Perform the subtraction: 100 J - 150 J = -50 J.
Step 7: Conclude that the change in internal energy (ΔU) is -50 J.

First Law of Thermodynamics – The first law states that the change in internal energy (ΔU) of a system is equal to the heat added to the system (Q) minus the work done by the system on the surroundings (W).