What is the change in internal energy (in J) of a system that absorbs 0.677 kJ of heat from its surroundings and has 0.438 kcal of work done on it?
To find the change in internal energy (ΔU) of a system, you need to consider the heat (q) absorbed and the work (w) done on the system.
The given heat transfer is 0.677 kJ or 677 J (since 1 kJ = 1000 J). The work done on the system is 0.438 kcal or 1832.392 J (since 1 kcal = 4.184 J). Note that it is important to convert all quantities to the same unit before performing any calculations.
The change in internal energy can be calculated using the First Law of Thermodynamics:
ΔU = q + w
Substituting the values, we get:
ΔU = 677 J + 1832.392 J
Adding the two values, we find:
ΔU = 2509.392 J
Therefore, the change in internal energy of the system is 2509.392 J.