The initial state consists of a closed system containing one mole of super-heated liquid water at 115°C and 1 atmosphere pressure. The immediate surroundings are also at 115°C and 1 atmosphere pressure.
The change in state is described as this one mole of super-heated liquid water vaporizing to water vapor at 115°C, as shown by the following reaction at 1 atmosphere pressure.
1 mole, H2O, liquid, 115°C ---> 1 mole, H2O, vapor, 115°C
a) Calculate the Enthalpy change for the system at 115°C.
b) Calculate the Entropy change for this system at 115°C.
c) Assuming that the surroundings behave as a constant temperature reservoir,
calculate the Enthalpy change for the surroundings
d) Assuming that the surroundings behave as a constant temperature reservoir,
calculate the Entropy change for the surroundings
e) Calculate the Entropy change for the universe.
Given the following:
Cp (liquid) = 75.33 J/mole K,
Cp (vapor) = 37.47 J/mole K,
∆H vaporization (100°C) = 40790 J/mole
I really have no idea what to do or where to start. I know I need to break the problem down into steps but I'm not sure exactly how to split it up.
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