The negative free energy change comes instead from the fact that the bonds formed after hydrolysis-or the phosphorylation of a residue by ATP-are lower in energy than the bonds present before hydrolysis . ( This includes " all " of the bonds involved in the reaction, not just the phosphate bonds themselves ).
42.
Where k _ { et } is the rate constant for electron transfer, | H _ { AB } | is the electronic coupling between the initial and final states, \ lambda is the reorganization energy ( both inner and outer-sphere ), and \ Delta G ^ \ circ is the total Gibbs free energy change for the electron transfer reaction ( k _ b is the Boltzmann constant and T is the absolute temperature ).
43.
Constant pressure, constant temperature reactions are exergonic if and only if the Gibbs free energy change is negative ( " " G " < 0 ) . " Exergonic " ( from the prefix exo-, derived for the Greek word ?? " exM ", " outside " and the suffix-ergonic, derived from the Greek word ???? " ergon ", " work " ) means " releasing energy in the form of work ".
44.
Δ G is the Gibbs free energy change ( kJ & middot; mol " 1 ) during transfer of 1 mol of cations X m + from the phase A to B down the electrical potential, & Delta; & psi; is the electrical potential difference ( mV ) between phases P and N ( A and B ), [ X m + ] A and [ X m + ] B are our cation concentrations on opposite sides of the membrane, F is the Faraday constant, R gas constant.
45.
:Unfortunately, we don't seem to have an article on the van't Hoff isotherm, but Googling it turns up several sites ( ( page 269 in the last ) ) From these I surmise that the van't Hoff reaction isotherm refers to the equation giving the free energy change for a reaction system which is not in equilibrium : \ Delta G =-RT \, ln \, K _ { eq } + RT \, ln \, Q, where Q has the same form as the equilibrium constant but uses the current, non-equilibrium talk ) 19 : 26, 14 June 2009 ( UTC)
