A closed 2.0-L container holds 3.0 mol of an ideal gas. If 200 J of heat is added, what is the change in internal energy of the system?
A. 300 J
B. 150 J
C. zero
D. 100 J
E. 200 J
-Since there is no mention of work being done I thing the answer is 200J but I want to make sure?
closed 2.0-L container
Yes, 200J
To find the change in internal energy of the system, we can use the equation:
ΔU = Q - W
Where:
ΔU = change in internal energy of the system
Q = heat added to the system
W = work done by or on the system
In this case, the container is closed, which means no work is being done. Therefore, W = 0.
Substituting the values, we have:
ΔU = Q - W
ΔU = 200 J - 0 J
ΔU = 200 J
So, the change in internal energy of the system is 200 J.
Therefore, the correct answer is E. 200 J.
To determine the change in internal energy of the system, we can 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:
ΔU = Q - W
In this case, the container is closed, which means no work is done (W = 0), so the equation simplifies to:
ΔU = Q
Given that 200 J of heat (Q) is added to the system, the change in internal energy (ΔU) of the system is also 200 J.
Therefore, the correct answer is E. 200 J.