Sample results:

Initial mass of ice $=150\mathrm{.}89g$

Final mass of ice $=99\mathrm{.}69g$

Initial temperature of water $=42C$

Final temperature of water $=0\mathrm{.}4C$

Analysis

Determine the mass of the ice that has melted.

Determine the variation of the water temperature $(T).$

a$)$ Calculate the energy $($in J$)$ released by $100g(100mL)$ of water when it cooled by $T.$ Recall that the energy lost by the surroundings $($the water$)$ will be the energy gained by the system $($the ice$).$ The specific heat capacity$($c$)$ of water is $4\mathrm{.}18\frac{J}{gC}.$ Use the formula $Q=mcT$ and the mass of water.

b$)$ Convert your answer into kJ$.$

Calculate the energy necessary to melt $1g$ of ice $($in $kJ).$ Recall that the energy you calculated in $3($a$)$ is the amount to melt $51\mathrm{.}2g$ of ice. Use this to find the energy to melt the $1g$ of ice in this question.

Using the results from this experiment, determine how many $kJ$ are required to melt $1$ mole of ice.

Write the chemical equation for the melting of ice. Don't forget to include the value for the energy term in your equation.