- #1

Ariel Jo

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## Homework Statement

You have 0.50 mol of steam which has been supercooled to 95˚C at 1 atm. Since the steam is below the boiling/condensation point, it proceeds to partially condense into liquid water. This happens in a thermally-insulated vessel at constant pressure.

(a) When the system re-attains equilibrium, what will the final temperature be?

(b) What fraction of the water will condense?

(c) Calculate ΔS for this process.

## Homework Equations

ideal gas equation (the gas is assumed to behave ideally)

deltaS=n*Cp*ln(Tf/Ti)

## The Attempt at a Solution

From PV=nRT, obtained an initial volume of steam of 15.1L but unsure how to proceed... Vf and Tf are both unknowns but should not be equal to Vi and Ti (from common sense - steam at 95degC will both condense and cool spontaneously.) Can easily find change in entropy from knowing final temperature... Would U=3/2RT be useful in this situation?

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