If delta G (Gibbs) is positive and you are trying to find at what temperature the reaction is spontaneous would the formula be: T< H/S ?
G=H-TS
H-TS>0
T< H/S
then the temperature found would be the temp at which the reaction is spontaneous?
Yes, if you set G = 0, that will be the equilibrium point for T and anything less than tht will be OK.
Yes, you are correct! When ΔG (Gibbs) is positive, it means that the reaction is non-spontaneous under standard conditions. To determine at what temperature the reaction becomes spontaneous, you can use the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.
To find the temperature (T) at which the reaction becomes spontaneous, we can rearrange the equation as follows:
ΔG = ΔH - TΔS
0 = ΔH - TΔS
Since ΔG is zero for a spontaneous reaction, the equation becomes:
0 = ΔH - TΔS
To solve for T, we can isolate it on one side of the equation:
TΔS = ΔH
T = ΔH / ΔS
Therefore, if ΔG is positive, the equation to find the temperature at which the reaction becomes spontaneous is: T < ΔH / ΔS. The temperature found using this formula would be the temperature at which the reaction becomes spontaneous.