00:01
Talk about equilibrium constants and in relation to gibbs -free energy.
00:05
So here i kind of listed the definitions of each of these.
00:08
So we have equilibrium constant.
00:09
We have delta g, which is the change in gibbs energy, and then q.
00:14
K is the equilibrium constant.
00:16
It is the value of a reaction quotient at equilibrium.
00:19
So you can think about it as the ratio of products to reactants.
00:24
Our delta g, we know it's the change in gibbs -free energy, a negative delta g.
00:31
Indicates its spontaneous process or a spontaneous reaction, whereas a positive delta g indicates a non -spontaneous reaction.
00:39
Remember, spontaneous is one that occurs naturally.
00:43
It's going to go forward towards the products.
00:46
Whereas a positive delta g, it's going to rather, it happens rather slowly.
00:51
It's not spontaneous, so it's not going to go forward as much as a spontaneous reaction.
00:57
It's actually going to prefer the reactants.
00:59
You can think about it.
01:00
There's two ways you can think about our delta g.
01:03
This is just a couple of ways in which you can think about it.
01:06
And lastly, our q is a measurement of the relative amounts of products and reactants present at a given time.
01:12
So those one requires a little bit more calculation.
01:14
May sound a little bit similar to our k or equilibrium constant, but our equilibrium constant is the ratio of products reactions, whereas q measures the relative amounts.
01:25
So if we were curious and if we had, for example, where our k we can put k is much less we can indicate as k is much smaller than one um well what do we know about the sign of our delta g our gips free energy well let's think about this well we know that we said that k is equilibrium constant and it's a ratio right so we're saying here that the ratio of products to reactants is much less than one and if we want to think about our ratio our product should go at the top and our reactants are going to be at the bottom...