Answer:
ΔU = -4.904 × 10^(5) J
Explanation:
We are given;
Heat transfer into the system;Q1 = 3.88 × 10^(6) J
Heat transfer out of the system;Q2 = 7.92 × 10^(6) J
Work done; W = 4.5 × 10^(5) J
Now, the net heat transfer is the heat transfer into the system minus the heat transfer out of the system. Thus;. Q = Q1 - Q2
Q = (3.88 × 10^(6)) - (7.92 × 10^(6))
Q = -4.04 × 10^(6) J
The formula for change in internal energy is given by the first law of thermodynamics:
ΔU = Q - W
ΔU = (-4.04 × 10^(6)) - 4.5 × 10^(5)
ΔU = -4.904 × 10^(5) J
The negative sign means loss of internal energy
