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The molar enthalpy of vaporization of water at its normal boiling point of 373.15 K and 1 atm is 40.65 kJ/mol. The density of liquid water is 958.4 g/L and the density of water vapor is 0.6010 g/L . a) Use Clapeyron equation to determine the value of dP/dT for water at its normal boiling point of 373.15 K. Express your answer in atm/K. Use this result to determine the boiling point of water at a pressure of 2 atm. b) use the Clausius Clapeyron equation to estimate the boiling point of water at a pressure of 2 atm.

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