For reaction $A \rightleftharpoons B$, $\Delta G^{\circ} = 105 - 35 \log T$. Find the transition temperature (in $^{\circ} C$) of the above reaction at 1 bar.
Finding the temperature at which a reaction becomes spontaneous or reaches equilibrium by setting the Gibbs Free Energy change to zero.
CALCULATION: 1. We are given the relation for standard Gibbs energy: $\Delta G^{\circ} = 105 - 35 \log T$. 2. At the transition point, the standard free energy change is zero: $0 = 105 - 35 \log T$. 3. Rearranging: $35 \log T = 105 \Rightarrow \log T = 3$. 4. Taking the antilog: $T = 10^3 = 1000 \text{ Kelvin}$. 5. To convert Kelvin to Celsius: $t(^{\circ} C) = 1000 - 273 = 727^{\circ} C$. The answer is 727.
