A $25-$kg iron block initially at $350$C is quenched in an insulated tank that contains $100$ kg of water at $18$C$.$ Assuming the water that vaporizes during the process condenses back in the tank, determine the total entropy change during this process. Take the specific heats of water and iron to be $4\mathrm{.}18$ kJ$/$kg$-$K and $0\mathrm{.}45$ kJ$/$kg$-$K$,$ respectively. How could the iron block be cooled to $18$C will almost no change in entropy of the universe? $($Ans: $4\mathrm{.}08$ kJ$/$K$)$