Make a graph of the molar enthalpy of water as a function of temperature, from $150K$ to $450$ K$.$ For convenience, you can take $H=0$ for $H_{2}O(cr)$ at $150K.$ Also make a graph of the molar entropy of water over the same temperature range. Here make use of $S=69\mathrm{.}91\frac{J}{m}$olK for $H_{2}O(1)$ at $298K($you can find this value in the back of your book$).$ For both plots, let $P=1$ bar. If you wish, you need only calculate values of $H$ and $S$ for the following temperatures: $150K,273K,298K,373K,$ and $450K.$ Use the information below. Keep track of units $($some quantities below are "specific", i$.$e$.,$ on a per gram basis.$)$

$C_p($water$,$ solid$)=2\mathrm{.}1\frac{J}{g}K$

$C_p($water$,$ liquid$)=4\mathrm{.}18\frac{J}{g}K$

$C_p($water$,$ vapor$)=2\mathrm{.}0\frac{J}{g}K$

water, $273K$

water, $373K$