Self-Test 9.15A

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Self-Test 9.15A

Postby Alex_Wagas_3K » Thu Feb 02, 2017 2:04 pm

Calculate the entropy change of the surroundings when 1.00 mol H2O(l) vaporizes at 90°C and 1 bar. Take the enthalpy of vaporization of water as
40.7 kJ*mol-1.

For this problem, you do not need to set the 40.7 kJ*mol-1 negative because it is already given at the vaporization stage correct?

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Re: Self-Test 9.15A

Postby Nikhil_Madan_3C » Thu Feb 02, 2017 3:01 pm

Yes, you are correct. The enthalpy of vaporization is positive because it represents the energy that must be added to the liquid substance to transform a quantity of that substance into gas.

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