How to calculate ∆rGº from entropy and ∆fGº in different temperatures? &quot;The total oxidation of glucose occurs according to the following chemical equation:
C6H12O6 (s) + 6O2 (g) -&gt; 6CO2 (g) + 6H2O (l)
The following table gives us the free energies of standard formation and the standard molar entropies of
compounds involved in the previous reaction.




Compound
∆fGº(298 K) kJ/mol
Smº (298 K) J/K/mol




C6H12O6
-917,2
212,10


O2
0
205,14


CO2
-394,36
213,14


H20
-273,13
69,91




Based on the previous data, determine the ∆rGº
for glucose oxidation at 308 K&quot;
It's a question of a doctoral selection process and I want to figure out if it is formulated wrong or if there is a way to an answer.
For a small temperature change like that, you can make use of dG=-SdT.  Determine $\Delta rG^0$ and $\Delta r S^0$ at 298, multiply the latter by 10 , and subtract it from the former to get $\Delta rG^0$ at 308K.