Which process has the greatest decrease in entropy and why?

[katrina007]

Hi again,

Need help with one more question if anyone don't mind. Any help is appreciated. Thanks in advance.

Arrange these three processes in order of their decreasing tendencies toward spontaneity.

I. H2O (l) --> H2O (g) at 105 C degrees, 1.00 atm
II. H2O (l) --> H2O (s) at 25 C degrees, 1.00 atm
III. H2O (l) --> H2O (s) at 0 C degrees, 1.00 atm

Select one answer
a) I > III > II
b) II > III > I
c) I > II > III
d) III > II > I
e) II > I > III

I think the answer is (a) because the gas form is more sponteous than the solids. And then its the third one then the second one because the temp. of 3rd one is less than 2nd. ??

 

[hage567]

Which answer do you think it is? You need to show some effort, you know!

 

[katrina007]

Sorry. Ok I've given my opinion for this question. Let me know if I am wrong or right.

 

[Oaksinstructor]

Take a look at the Gibbs Free Energy Equation:
ΔG = ΔH - TΔS(init)
whereas T is the temperature (SI Units: kelvins); S is the entropy (SI Units: joules per kelvin); H is the enthalpy (SI Units: joules)

and remember that when ΔG < 0 the reaction is spontaneous...