If a system absorbs 200 J of heat and does 50 J of work, what is the change in i

If a system absorbs 200 J of heat and does 50 J of work, what is the change in internal energy?

If a system absorbs 200 J of heat and does 50 J of work, what is the change in internal energy?

Step 1: Identify the heat absorbed by the system, which is given as 200 J. This is represented as Q.
Step 2: Identify the work done by the system, which is given as 50 J. This is represented as W.
Step 3: Use the formula from the First Law of Thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat absorbed (Q) minus the work done (W).
Step 4: Substitute the values into the formula: ΔU = Q - W = 200 J - 50 J.
Step 5: Calculate the result: 200 J - 50 J = 150 J.
Step 6: Conclude that the change in internal energy (ΔU) is 150 J.

First Law of Thermodynamics – The principle 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 (W).