# Question #b01e8

Sep 22, 2017

$\text{33,360 J}$

#### Explanation:

The idea here is that the enthalpy of fusion, $\Delta {H}_{\text{fus}}$, tells you the amount of energy needed to convert $\text{1 g}$ of a given substance from solid at its melting point to liquid at its melting point.

In your case, the enthalpy of fusion of water

$\Delta {H}_{\text{fus" = color(darkorange)("333.6 J")color(white)(.)color(blue)("g}}^{- 1}$

tells you that in order to turn $\textcolor{b l u e}{\text{1 g}}$ of ice at its normal melting point of ${0}^{\circ} \text{C}$ to liquid water at ${0}^{\circ} \text{C}$, you need to provide $\textcolor{\mathrm{da} r k \mathmr{and} a n \ge}{\text{333.6 J}}$ of heat.

This means that you will need

$100.0 \textcolor{red}{\cancel{\textcolor{b l a c k}{\text{g"))) * color(darkorange)("333.6 J")/(color(blue)(1)color(red)(cancel(color(blue)("g")))) = color(darkgreen)(ul(color(black)("33,360 J}}}}$

The answer is rounded to four sig figs, the number of sig figs you have for the mass of the sample.