Nitrogen $($N$\_(2))$ undergoes an internally reversible process from $6$ bar, $247\backslash$deg C during which pv$^(1\mathrm{.}2)=$ constant. The initial volume is $0\mathrm{.}1$m$^(3)$

and the work for the process is $50$ kJ $.$

Assuming ideal gas behavior, and neglecting kinetic and potential energy effects, determine heat transfer, in kJ$,$ and the entropy

change, in k$($J$)/($K$).$

Q$=$

kJ

$\backslash$Delta S$=$

k$($J$)/($K$)$