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Consider liquid water (ρ = 0.9999 g/cm3) and ice (ρ = 0.9150 g/cm3) in equilibrium at 0oc and calculate the difference in molar Gibbs energies of liquid water and its vapour when the pressure is increased from 1.0 bar to 100.0 ba
Accepted Answer
The difference in molar Gibbs energies of liquid water and its vapor at a given temperature and pressure can be calculated using the Clausius-Clapeyron equation. This equation relates the vapor pressure of a liquid to its temperature and enthalpy of vaporization. The change in pressure from 1.0 bar to 100.0 bar would significantly affect the vapor pressure and hence the Gibbs free energy difference. However, without knowing the enthalpy of vaporization at 0°C, we cannot provide a numerical answer.
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