Entropy and free energy question?

Question

I encountered this problem on the 2004 FRQ AP exam:

(d) The standard free energy of formation, ΔG°f, of Fe2O3(s) is -740. kJ mol-1 at 298 K.

The ΔS°f is -0.28 KJ/mol/K
The ΔH°f is -824 KJ/mol

The question basically is, by how much does the ΔS°f decrease the free energy of the reaction?
And the same question goes for ΔH°f , except in this case it would be by how much does it increase the free energy of the reaction! (KJ/mol of Fe2O3)

thanks!

Answer 1

-.055 and no

Answer 2

The question seems to be "would loose skill opposite entropy?" the only loose skill i comprehend of ios that skill created by skill of a Being. Technologically conversing , there is no such subject as "loose" skill. -- the universe doessnt artwork that way... nothuing is "loose". for each output of skill or remember, and so on.,, there could be an enter of a few sort. Likewise entropy is a elementary regulation of the universe which will not be able to be broken. -- each and every thing decays and degenerates finally. To opposite entropy will require restructuring the function of the completed universe.

Answer 3

delta G = delta H - T*delta S (reference books I have list entropy of formation for Fe2O3 as +0.088 kJ/mol)

If the entropy was zero, then delta G = delta H, so the entropy decreases the free energy produced by the difference between G and H, or 84 kJ/mol.

If enthalpy was zero, then delta G = - T delta S, so the enthalpy increases the free energy produced by 824 kJ/mol.

Answer 4

Delta G = Delta H - Delta S into T

Now plug in values, making sure all quantities are in SI.