# What is the enthalpy of the phase transition ice to water with respect to a 20*g mass of ice?

##### 1 Answer
Jul 8, 2017

We interrogate the reaction............

#### Explanation:

We interrogate the phase transition............

${H}_{2} O \left(s\right) + \Delta \stackrel{{\text{0" }}^{\circ} C}{\rightarrow} {H}_{2} O \left(l\right)$

Since both the $\text{reactant}$ and the $\text{product}$ are conceived to be at the same temperatgure, we only need consider the enthalpy change of the phase transition, and we expect reasonably, that the process gives an $\text{endotherm}$, as we are breaking ice-ice bonds..........

And we gots a $20 \cdot g$ mass of ice.......

${\Delta}_{\text{phase transition}} = 20 \cdot g \times 334 \cdot J \cdot {g}^{-} 1 = + 6680 \cdot J = 6.68 \cdot k J$

And this represents 6680*Jxx1/(4.184*J*"cal"^-1)=??"cal"

And if we have a 2 molar quantity of ice, i.e. a $36 \cdot g$ mass, we simply solve.......

${\Delta}_{\text{phase transition}} = 36 \cdot g \times 334 \cdot J \cdot {g}^{-} 1 = + 12024 \cdot J = 12.0 \cdot k J$

$\cong 2874 \cdot \text{cal}$........