4.8)  Calculate the values of ΔU, ΔH, and ΔS for the following process:1 mole of liquid water at 25 C and 1 atm ➡️ 1 mole of steam at 100 C and 1 atmThe molar heat of vaporization of water at 373 K is 40.79 kJ mol-1, and molar heat capacity of water is 75.3 J K-1 mol-1.  Assume molar heat capacity to be temperature independent and ideal-gas behavior.

Question
Asked Mar 12, 2019

4.8)  Calculate the values of ΔU, ΔH, and ΔS for the following process:

1 mole of liquid water at 25 C and 1 atm ➡️ 1 mole of steam at 100 C and 1 atm

The molar heat of vaporization of water at 373 K is 40.79 kJ mol-1, and molar heat capacity of water is 75.3 J K-1 mol-1.  Assume molar heat capacity to be temperature independent and ideal-gas behavior. 

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Expert Answer

Step 1

In isobaric process, ΔH = q, the given process also an isobaric process so the molar heat of vaporization equal to enthalpy change,

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Step 2

Internal energy change of 1 mole of liquid water to 1 mole of steam is calculated by substituting the values of R and T (373K) give ΔH (40.7 KJ mol-1) and Δn (1) in below equation.

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Step 3

Heat change of given process is equal to molar heat of vaporization of wate...

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