Heat is added to a system, and the system does 35.0 J of work. If the internal energy increases by 17.0 J, how much heat was added to the system?
18
To determine the amount of heat added to the system, we need to apply the First Law of Thermodynamics, which states that the change in internal energy (ΔU) is equal to the heat added to the system (Q) minus the work done by the system (W).
The equation can be written as:
ΔU = Q - W
Given that the work done by the system (W) is 35.0 J, and the change in internal energy (ΔU) is 17.0 J, we can use the equation to find the heat added to the system (Q).
ΔU = Q - W
17.0 J = Q - 35.0 J
To solve for Q, we can rearrange the equation by adding 35.0 J to both sides:
17.0 J + 35.0 J = Q - 35.0 J + 35.0 J
This simplifies to:
52.0 J = Q
Therefore, the heat added to the system is 52.0 J.