Now, because the energy, the free energy of the products is higher than the free energy of the reactants, that means this reaction is andergonic. And so we need to input 21.3 kilojoules of energy to actually drive this reaction in the forward direction. So this reaction, as described here understanding conditions, is andergonic it's non spontaneous, it's reactant favorite. And this is in accordance with the fact that formic acid is a weak acid and will not associate to a very large extent. Now, just because the Delta G degree symbol the Delta G under standard state conditions is positive for these conditions, does not mean the Delta G will be positive under some other conditions. In fact, by changing the Q value, by changing the concentrations of the reactants and products, we can ultimately transform this endergonic reaction into an exergonic reaction.