Now this divided by this gives us negative 4.61. And so if we carry out this calculation, raised ten to the power of negative 4.61, we get about 2.45 times ten to negative five. Now, what this means is when the Q value, when this quantity, when the ratio of the concentration of the product and the reactants is equal to 0.245, the reaction, this reaction here will actually be exergonic, it will be spontaneous and it will be product favored. So what we basically show is even though this reaction is undergodonic under standard conditions, when the concentrations of these are equal, if we change the concentrations around, we can actually transform that endergonic non spontaneous reaction into an exergonic spontaneous reaction, as can be seen in the following example where we use the delta g on negative quantity. So ultimately it's the delta g that determines whether our reaction under those concentration conditions and that temperature value is actually spontaneous or not. This doesn't necessarily have to be negative or positive.