How much heat is required to convert $20\mathrm{.}4$ g of liquid H$2$O at $83\mathrm{.}8\backslash$deg C into steam at $144\mathrm{.}5\backslash$deg C$?$

For liquid water, C $=4\mathrm{.}185$ J$/$g $\backslash$deg C

For water vapor, C $=1\mathrm{.}996$ J$/$g $\backslash$deg C

$$Hvap $=40\mathrm{.}65$ kJ$/$mol

Energy needed $=\_\_\_$ JRemember that there are three pieces that must be considered:

$q_1=$ heat needed to raise the temperature of the liquid to $100\mathrm{.}0C=mCDT$

$q_2=$ heat needed to vaporize the sample $=(\frac{\text{m}\text{a}\text{s}\text{s}}{MW})H_{\text{v}\text{a}\text{p}}$

$q_3=$ heat needed to raise the temperature of the vapor from $100\mathrm{.}0C$ to the

final temperature $=mCDT$