# Question #1c02e

Apr 24, 2015

You need 16,700 J to melt that much ice at ${0}^{\circ} \text{C}$.

Since you're dealing with a phase change, the equation you'll need to use is

$q = m \cdot \Delta {H}_{\text{fus}}$, where

$q$ - the heat you need to suplly to the ice;
$m$ - the mass of the ice;
$\Delta {H}_{\text{fus}}$ - the latent heat of fusion, or enthalpy of fusion, which is the change in enthalpy you get when you heat a gram of a substance to change it from solid state to liquid state.

In your case, you need to supply 334 J for every 1 gram of ice at ${0}^{\circ} \text{C}$ to get it to melt it to water at ${0}^{\circ} \text{C}$. Since you've actually got 50.0 g of ice, the energy required to melt the ice will be

$q = m \cdot \Delta {H}_{\text{fus}}$

$q = 50.0 \cancel{\text{g") * "334 J" = color(green)("16,700 J}}$