A piece of iron with a mass of $72\mathrm{.}4$ g is heated to $363$ K

$(90\backslash$deg C$)$ and then plunged into $100\mathrm{.}0$ g of water that is

initially at $283$ K $(10\backslash$deg C$).$ Calculate the temperature of

thermal equilibrium, assuming that no heat is lost to

the surroundings.

$($From Table $10-1,$ specific heat capacities of water

and iron are $4\mathrm{.}184$ and $0\mathrm{.}449$ J K$-1$ g$-1,$ respectively$).$