Gibbs Free Energy?

Question

Which statement about the hydrations of sulfur trioxide is correct?
SO3(g) + H2O(g) ---> H2SO4

delta(H) = -227 kJ/mol, delta(S )= -309 J/mol-K


A.At 1,000oC, G = 1.98 X 105 J/mol.
B.The reaction would be at equilibrium at about 735 K.
C.The reaction is spontaneous at 1,400 K.
D. deltaG can be negative only at high temperatures.
E. None of the above


Well this little bugger is making me angry. I'll try to show you what I did step by step.

1st scenario: At 1000 C , equation would look like.
deltaG= -227kJ/mol - 1273K * (-.309kJ/mol*K)=166
NO Match

2nd scenario:
deltaG= -227kJ/mol - 735K * (-.309kJ/mol*K)=.115
No Match

3rd scenario.
deltaG= -227kJ/mol - 1400K * (-.309kJ/mol*K)=205.6
Nope

4th scenario
Well according to my notes, deltaG is positive at high temperatures.
Nope

5th scenario: None of the above.
Since all others didn't make sense , I went with this answer:


But guess what??? I was wrong.

What did I do wrong? I went over it

Answer 1

Look at your value for B. Your value of delta G is actually very close to zero, the condition for equilibrium. Now read the exact words of the question!

Answer 2

certain, fee of Gibbs loose power (delta G) and Gibbs loose power lower than established situations (delta G knot) has similarities in the journey that they are both calculated lower than a similar temperature (298K) although this is going to also be observed to maintain a million atm rigidity also.