Since std free energy has constant pressure, ΔH = Q and TΔS = T(ΔQ/T) = Q, so ΔG = Q - ΔQ, right? Wouldn't that just essentially mean reaction direction is entirely determined by the energy lost?
If your variables you subsitute for Delta H and Delta G lead you back to the gibbs free energy equation: ΔG = ΔH = TΔS, your equation should be correct! ΔG symbolizes Gibbs energy, when negative the reaction is spontaneous, when positive, the reaction is non-spontaneous ΔH symbolizes change in energy change usually in Joules ΔS symbolizes entropy change or the measure of randomness in a reaction T symbolizes temperature in Kelvins The reaction direction is determined by comparing Q: the reaction quotient, and K the equilibrium constant. When K is greater than Q, the reaction would proceed forward. Hopefully you are given K. I hope this helps! God bless!
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Since std free energy has constant pressure, ΔH = Q and TΔS = T(ΔQ/T) = Q, so ΔG = Q - ΔQ, right? Wouldn't that just essentially mean reaction direction is entirely determined by the energy lost?
If your variables you subsitute for Delta H and Delta G lead you back to the gibbs free energy equation: ΔG = ΔH = TΔS, your equation should be correct!
ΔG symbolizes Gibbs energy, when negative the reaction is spontaneous, when positive, the reaction is non-spontaneous
ΔH symbolizes change in energy change usually in Joules
ΔS symbolizes entropy change or the measure of randomness in a reaction
T symbolizes temperature in Kelvins
The reaction direction is determined by comparing Q: the reaction quotient, and K the equilibrium constant. When K is greater than Q, the reaction would proceed forward. Hopefully you are given K.
I hope this helps! God bless!
Thanks😃