Calculate the adiabatic change in entropy when $9$ g of ice at $-5\backslash$deg C is

added to $36\mathrm{.}75$ g of hot water at $60\backslash$deg C in an isolated system. Given the

following information:

Heat capacity of ice cp $[$H$2$ O$($s$)]=37\mathrm{.}17$ J K$-1$ mol $-1$

Heat capacity of water cp $[$H$2$O$($l$)]=75\mathrm{.}29$ J $\backslash$deg C$-1$ mol $-1.$

Molar enthalpy of fusion of ice $$HO m $[$H$2$O$($s$)]=+6\mathrm{.}008$ kJ mol $-1$Calculate the adiabatic change in entropy when $9g$ of ice at $-5C$ is

added to $36\mathrm{.}75g$ of hot water at $60C$ in an isolated system. Given the

following information:

Heat capacity of ice $c_p[H_{2}O(s)]=37\mathrm{.}17J{K}^{-1}mo{l}^{-1}$

Heat capacity of water $c_p[H_{2}O(l)]=75\mathrm{.}29J{C}^{-1}mo{l}^{-1}.$

Molar enthalpy of fusion of ice $H^{O}m[H_{2}O(s)]=+6\mathrm{.}008kJmo{l}^{-1}$