00:01
All right, so we want to consider why if we have a substrate or a reactant turning into a product, and if we have a very large change in delta g, which presumably is a large negative number to make the reaction very spontaneous, why would the reaction not happen quickly? so when you're talking about delta g or delta h or any one of these quantities, those are thermodynamic quantities, meaning that they relate.
00:31
To the equilibrium position.
00:38
And equilibrium has nothing to do with the actual rate of the reaction, which is a kinetic factor.
00:45
So we want to talk about kinetic factors to explain why, regardless of the thermodynamics, a reaction can be slow.
00:54
Exothermic, again, that's a thermodynamic quantity, so that has nothing to do with this.
00:59
Also, if the reaction is exothermic, it's actually favorable because heat is released.
01:04
So we can cross that out.
01:05
Okay.
01:05
The rate of conversion from substature product does not depend on the free energy difference.
01:09
We just said that because the rate is a kinetic factor and delta g is a thermodynamic...