To solve this problem, we need to use the First Law of Thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system:
ΔU = Q - W
Where: ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system.
Given: Q = 35 J (heat absorbed) W = 11 J (work done) Initial internal energy (U) = 205 J
Substituting the given values into the equation:
ΔU = Q - W ΔU = 35 J - 11 J ΔU = 24 J
The change in internal energy is 24 J. To find the final internal energy, we add this change to the initial internal energy:
Final internal energy = Initial internal energy + ΔU Final internal energy = 205 J + 24 J Final internal energy = 229 J
Therefore, the final internal energy of the system is 229 J.