00:01
In this problem, we need to explain the differences between the change in gibbs -free energy delta -g at standard conditions and the change in gibbs -free energy delta -g at any set of conditions.
00:14
The main difference between these two in terms of the symbols for these variables is that this zero corresponds to standard conditions.
00:23
And those standard conditions mean that we have one molar of concentration units for all these species involved.
00:31
In the reaction and all of the species have a partial pressure of one atmosphere.
00:39
The equation that we use to find delta g at standard conditions is negative r, which is a constant, times a temperature, times the ln of k, where k is equal to the equilibrium constant of this reaction.
00:56
We can find k by taking the concentration of all the gaseous and aqueous species, of the products of the reaction and multiplying them and then dividing by the product of the concentrations of all of the reactants of that chemical reaction and we could also define this this k value in terms of of partial pressure units so the partial pressure of each product divided by the partial pressure of each reactant.
01:48
And when the system is at equilibrium, we know that that means that delta g is equal to zero.
01:55
So if we set delta g equal to zero to represent equilibrium conditions at a given temperature value, then we can solve for k, which would correspond to the equilibrium concentration, the equilibrium constant value, either kc, if we are using the concentration equation or kp we are using the partial pressure form of the equation for the equation to find delta g at any standard conditions we use the delta g at standard conditions as a component of this equation and we add the product of r and t multiplied by the ln of q and q is similar to k and this is called the the reaction quotient and the the reaction quotient and we use the same formulas to solve for q.
02:52
However, these can be any values for concentrations or pressures of the system...