- #1

- 2

- 0

Given Data:

triple point of water (.006 atm, .0075ºC).

density of water = 1 g/cm^3

latent heat of fusion = 6000 J/mol (at normal melting temperature)

Problem:

Calculate the density of ice?

I assumed there is 1 mol of water, thus the volume is .01802 L.

To calculate the density of ice I need to find the accompanying change in volume from liquid to solid. From my textbook, the only equation which relates liquid - sold phase equilibrium as a variation of temp and pressure is:

Pressure = deltaH/deltaV*ln(T) + constant

This seems useful but im still not sure if it's the right equation.

triple point of water (.006 atm, .0075ºC).

density of water = 1 g/cm^3

latent heat of fusion = 6000 J/mol (at normal melting temperature)

Problem:

Calculate the density of ice?

I assumed there is 1 mol of water, thus the volume is .01802 L.

To calculate the density of ice I need to find the accompanying change in volume from liquid to solid. From my textbook, the only equation which relates liquid - sold phase equilibrium as a variation of temp and pressure is:

Pressure = deltaH/deltaV*ln(T) + constant

This seems useful but im still not sure if it's the right equation.

Last edited: