This is an incomplete question. The complete question is :
Calculate the change in internal energy (ΔE) for a system that is giving off 25.000 kJ of heat and is changing from 18.00 L to 15.00 L in volume at 1.50 atm pressure.
Answer: The change in internal energy for a system is -24544 Joules
Explanation:
According to first law of thermodynamics:
[tex]\Delta E=q+w[/tex]
[tex]\Delta E[/tex]=Change in internal energy
q = heat absorbed or released
w = work done or by the system
w = work done by the system=[tex]-P\Delta V[/tex] {Work done on the system as the final volume is lesser than initial volume and is positive}
w =[tex]-1.50atm\times (15.00-18.00)L=4.50Latm=456Joules[/tex] {1Latm=101.3J}
q = -25.000 kJ =[tex]-25.000\times 10^3J[/tex] {Heat released by the system is negative}
[tex]\Delta E=456J+(-25000)=-24544J[/tex]
Thus change in internal energy for a system is -24544 Joules
