Question

If a system has 375 kcal of work done to it, and releases 5.00×102 kJ of heat into its surroundings, what is the change in internal energy (Δ or Δ) of the system?

Δ= kJ

Answer 1

Step-by-step explanation:

We need to 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

First, we need to convert the units of work from kcal to kJ:

375 kcal × 4.184 J/kcal = 1570.5 J = 1.5705 kJ

Now we can plug in the values we have:

ΔU = (5.00×10² kJ) - (1.5705 kJ)

ΔU = 498.4295 kJ

Therefore, the change in internal energy of the system is ΔU = 498.4295 kJ.