00:01
As per the equation, the equation delta g is equal to delta h minus t into delta s.
00:19
So here, the difference between the free energy of the product and the free energy of the reactant.
01:06
A reaction is thermodynamically favorable when its enthalpy means delta h decreases and its entropy increases.
01:24
So here, delta h is less than zero and delta s greater than zero.
01:48
Now here, delta g is equal to negative.
02:01
Let's show in a diagram here, thermodynamically delta g here negative.
02:19
So this is an indication of reactant, free energy of reactant and this line represents the free energy of products.
02:35
Here the graph will be like this.
02:48
This represents activation energy...