Answer :
Answer: The work done by the system is -506.5 Joules and change in the system's internal energy is -206.5 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 is done by the system as the final volume is greater than initial volume and is negative}
w =[tex]-1atm\times (15.0-10.0)L=-5.00Latm=-506.5Joules[/tex] {1Latm=101.3J}
q = +300J {Heat absorbed by the system is positive}
[tex]\Delta E=+300+(-506.5)=-206.5J[/tex]
Thus the work done by the system is -506.5 Joules and change in the system's internal energy is -206.5 Joules