So when this is the case, we see that when 1 mol of formic acid at a concentration of one molar transforms into 1 mol of conjugate base and 1 mol of H plus ion. Which are also at a concentration of one molar. Then we see the Delta G between the product and the reactants is given by 21.3 kilojoules or 21,300 Joules of energy. 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.