A reversible reaction proceeds in the direction that decreases the free energy of the system. There is an important relationship between the equilibrium constant and the standard free energy of the system given bylog K=−ΔG02.303 RTThis equation is applicable to all reversible processes and allows us to estimate the equilibrium constant from the standard free energy and the enthalpy change of the reaction.Take R=253J/molK,112L atm/molk,ln 2=0.7,ln3=1.1,ln5=1.6,log2=0.3,log 3=0.5,log5=0.7 The equilibrium constant for the dissociation of N2O4 into NO2 is 0.125 at 27∘C. What is the standard free energy change for this reaction?

A reversible reaction proceeds in the direction that decreases the fre

1.	A reversible reaction proceeds in the direction that decreases the free energy of the system. There is an important relationship between the equilibrium constant and the standard free energy of the system given bylog K=−ΔG02.303 RTThis equation is applicable to all reversible processes and allows us to estimate the equilibrium constant from the standard free energy and the enthalpy change of the reaction.Take R=253J/molK,112L atm/molk,ln 2=0.7,ln3=1.1,ln5=1.6,log2=0.3,log 3=0.5,log5=0.7 The equilibrium constant for the dissociation of N2O4 into NO2 is 0.125 at 27∘C. What is the standard free energy change for this reaction?
Answer» A reversible reaction proceeds in the direction that decreases the free energy of the system. There is an important relationship between the equilibrium constant and the standard free energy of the system given by $log K = \frac{- Δ G^{0}}{2.303} RT$ This equation is applicable to all reversible processes and allows us to estimate the equilibrium constant from the standard free energy and the enthalpy change of the reaction. Take $R = \frac{25}{3} J/molK, \frac{1}{12} L atm/molk, ln 2 = 0.7, ln 3 = 1.1, ln 5 = 1.6, log 2 = 0.3, log 3 = 0.5, l o g 5 = 0.7$ The equilibrium constant for the dissociation of $N_{2} O_{4}$ into $N O_{2}$ is 0.125 at $27^{\circ}$ C. What is the standard free energy change for this reaction?