A system performs 349 J of work on its surroundings while losing 133 J of internal energy. Determine the heat transferred to the system during this process.
Delta U = Q - W
Delta U = -133 J
W = 349 J
Solve for Q.
To determine the heat transferred to the system, we can use the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat transferred to the system minus the work done by the system:
ΔU = Q - W
Where:
ΔU = change in internal energy
Q = heat transferred to the system
W = work done by the system
In this case, we are given that the system loses 133 J of internal energy (ΔU = -133 J) and performs 349 J of work on its surroundings (W = 349 J). We need to find the heat transferred to the system (Q).
Substituting the given values into the equation, we have:
-133 J = Q - 349 J
To isolate Q, we can rearrange the equation:
Q = -133 J + 349 J
Q = 216 J
Therefore, the heat transferred to the system during this process is 216 J.