A simple fluid flows through a pipe under steady state conditions with no work and negligible kinetic and potantial energy changes. Heat is added to this fluid through steps a$,$ b$,$ c and d as shown in the figure. Dueinf this process, fluid at $44\mathrm{.}4$C and $1,5$ MPa is heated at complety transfrom to superheated vapor at $125$C and $1023$kPa. tHE ENTHALPY OF THE FLU$$D AT PO$$NT B hB $$S G$$VEN AS $35$KJ$/$MOL AND THAT AT PO$$NT C hC $$S G$$VEN $64$kJ$/$MOL AT $72$c AND $4$MPa. The fluid follows the ideal gas equation of state both in the liquid and vapor phases nd has constant specific heat given CPl$/$R$=8\mathrm{.}9$ for the liquid and Cpig$/$R$=4\mathrm{.}4$ for the vapor. Calculate the total change in the entropy of $1$ mole of this fluid between point a and d in J$/$K$.$