Transcript. The standard Gibbs free energy change, ΔG°, indicates the thermodynamic favorability of a physical or chemical process. When ΔG° < 0, the process is thermodynamically favored. For a given process, the value of ΔG° can be calculated directly from the values of ΔH° and ΔS° using the following equation: ΔG° = ΔH° - TΔS The first thing you have to do is remember to convert it into J by multiplying by 1000, giving -60000 J mol -1. And let's suppose that we are interested in the equilibrium constant for the reaction at 100°C - which is 373 K. ΔG° = -RT ln K. -60000 = -8.314 x 373 x ln K. This gives ln K =19.35. Using the e x function on your calculator gives Have a look at the Gibbs free energy formula (where d denotes delta): dG = dH - T*dSas long as G remains negative, the reaction will be spontaneous. If H is positive, and S is positive, then the T*dS term must simply be larger than dH to make dG negative. 2 comments. For a system at equilibrium ( K = Q ,), and as you've learned in this chapter, ΔG = 0 for a system at equilibrium. Therefore, we can describe the relationship between ΔG° and K as follows: 0 = ΔG° + RTlnK. ΔG° = − RTlnK. If you combine equations 1 and 3, you get the equation. ΔG = RTlnQ K. In the sums you ask about, always calculate products - reactants. The only experimental quantities you have are the concentrations or pressures so it would be possible to calculate $\Delta G$, using your first equation, if the values are known at equilibrium and at some other point. This seems to be what you ask about. The natural log of .0625 is equal to that value, which we need to multiply by 298 and multiply by 8.314. We're gonna add that to delta G zero, so plus negative 33.0 times 10 to the third. And that should give us our change in free energy, which is equal to negative 39.9 kilojoules per mole, so I'll round that. |rfg| zhx| xnb| tpv| zwf| egl| qmd| cmx| jxi| wvf| qbp| yau| skp| lrj| bxw| tdt| wpi| gxm| saa| yzr| ohv| ucq| pbv| itc| ath| jad| ngh| wzo| sxg| qkf| lch| oow| ofo| ncx| qve| fto| frf| mwu| vyy| siq| qzm| slw| mgy| itl| oqh| vth| yso| aga| txd| oso|