Question

Calculate the entropy change of 18.6 g of steam that condenses to liquid water at 373.15 K. (Enter your answer in J/K).

Without doing further calculations, which of the following statements apply to the entropy change of the surroundings for the problem above?


True False  ΔS_surroundings will be negative.
True False  ΔS_surroundings will be positive.
True False  ΔS_surroundings < ΔS_steam
True False  ΔS_surroundings = -ΔS_steam
True False  ΔS_surroundings > -ΔS_steam
True False  ΔS_surroundings will not change.

Answer 1

Enthalpy of vaporization of water = 40.7 kJ/mol

∆S_sys = - n×∆H_vap./T

= - (18.6/18)×40.7×1000/373.15

= -112.7 J/K

A) False

B) True

C) False

D) True

E) false

F) False