Chemistry 433 Lecture 14 Gibbs Free Energy and Chemical Potential NC State University The internal energy expressed in terms of its natural variables We can use the combination of the first and second laws to derive an expression for the internal energy in terms of its natural variables. If we consider a reversible process: dU = δq + δw δw = -PdV (definition of work) δq = TdS S (second ( law rearranged)) Therefore, dU = TdS - PdV This expression expresses the fact that the internal energy U has a T when the entropy changes and a slope -P when the volume changes. changes We will use this expression to derive the P and T dependence of the free energy functions. The Gibbs energy expressed in terms of its natural variables To find the natural variables for the Gibbs energy we begin with the internal energy: dU = TdS - PdV and d substitute b i iinto: dH = dU + PdV + VdP to find: dH = TdS + VdP (S and P are natural variables of enthalpy) and using: dG = dH - TdS - SdT we find: dG = -SdT + VdP (T and P are natural variables of G) O Once again i we see why h G is i so useful. f l It Its natural t l variables i bl are ones that we commonly experience: T and P. The variation of the Gibbs energy with pressure We shown that dG = VdP - SdT. This differential can be used to determine both the pressure and temperature dependence p of the free energy. gy At constant temperature: p SdT = 0 and dG = VdP. The integrated form of this equation is: ΔG = P2 VdP P1 For one mole of an ideal gas we have: ΔGm = RT P2 P1 dP = RT ln P2 P1 P Note that we have expressed G as a molar quantity Gm = G/n. The variation of the Gibbs energy with pressure We can use the above expression p to indicate the free energy at some pressure P relative to the pressure of the standard state P = 1 bar. Gm T = G 0 T + RT ln P 1 bar G0(T) is the standard molar Gibb’s free energy for a gas. As discussed above the standard molar Gibb’s G ’ ffree energy is the free energy of one mole of the gas at 1 bar of pressure. The Gibb’s free energy gy increases logarithmically g y with p pressure. This is entirely an entropic effect. Note that the 1 bar can be omitted since we can write: RT ln P = RT ln P – RT ln 1 = RT ln P 1 bar The pressure dependence of G for liquids and solids If we are dealing g with a liquid q or a solid the molar volume is more or less a constant as a function of pressure. Actually, it depends on the isothermal compressibility, κ = -1/V(∂V/∂P) 1/V(∂V/∂P)T, but κ is very small small. It is a number of the order 10-4 atm-1 for liquids and 10-6 atm-1 for solids. We have discussed the fact that the density of liquids is nott strongly t l affected ff t d by b pressure. The Th smallll value l off κ is another way of saying the same thing. For our p purposes p we can treat the volume as a constant and we obtain Gm T = G 0 T + Vm P – 1 Question What is the isothermal compressibility κ = -1/V(∂V/∂P)T for an ideal gas? A. κ = -1/V B. κ = 1/P C. κ = 1/T D. κ = nRT/P Question What is the isothermal compressibility κ = -1/V(∂V/∂P)T for an ideal gas? A. κ = -1/V B. κ = 1/P C. κ = 1/T D. κ = nRT/P Question Compare the following two equations for the pressure dependence of the Gibbs free energy. Which one applies t the to th formation f ti off diamond di d from f graphite? hit ? P 1 bar A. Gm T = G 0 T + RT ln B. Gm T = G 0 T + Vm P – 1 Question Compare the following two equations for the pressure dependence of the Gibbs free energy. Which one applies t the to th formation f ti off diamond di d from f graphite? hit ? P 1 bar A. Gm T = G 0 T + RT ln B. Gm T = G 0 T + Vm P – 1 Systems with more than one component Up p to this p point we have derived state functions for p pure systems. (The one exception is the entropy of mixing). However, in order for a chemical change to occur we must have more than one component present present. We need generalize the methods to account for the presence of more than one type of molecule. In the introduction we stated that we would d thi do this using i a quantity tit called ll d th the chemical h i l potential. t ti l Th The chemical potential is nothing more than the molar Gibbs free energy gy of a p particular component. p Formally y we write it this way: Rate of change of G as number of moles of i changes with all other μ i = ∂G ∂n i T,P, j ≠ i variables held constant. Example: p ag gas p phase reaction Let’s consider a gas phase reaction as an example. We will use a textbook t tb k example: l N2O4 (g) = 2 NO2 (g) We know how to write the equilibrium q constant for this reaction. 2 NO 2 P K= PN 2O4 At constant T and P we will write the total Gibbs energy as: dG = μ NO 2dn NO 2 + μ N 2O 4dn N 2O4 dG = 2μ NO 2dn – μ N 2O 4dn We use the reaction stoichiometry to obtain the factor 2 for NO2. Definition of the Gibbs free energy change for chemical reaction We now define ΔrxnG: Δ rxnG = dG dn T,P This is ΔrxnG but it is not ΔrxnGo! Note that we will use ΔrxnG and ΔG interchangably. If we now apply the pressure dependence for one component component, Gm T = G 0 T + RT ln P 1 bar t a multicomponent to lti t system: t μ i T = μ 0i T + RT ln Pi 1 bar These two expressions are essentially identical. The chemical potential, μi, is nothing more than a molar free energy. Question How should one think of the chemical potential, μ of component j? A. It is the potential energy of that component B It is B. i a molar l free f energy off that th t componentt C. It is potential entropy of that component D. It is a molar entropy of that component Question How should one think of the chemical potential, μ of component j? A. It is the potential energy of that component B It is B. i a molar l free f energy off that th t componentt C. It is potential entropy of that component D. It is a molar entropy of that component Single component: Gm T = G 0 T + RT ln P 1 bar Multiple components each have a μj: μ i T = μ 0i T + RT ln Pi 1 bar Application of definitions to the chemical reaction We can write the Gibbs energy as: ΔG = 2μ NO 2 – μ N 2O4 and use the chemical p potentials: μ NO 2= μ 0NO 2 + RT ln PNO 2 μ N 2O4= μ 0N 2O4 + RT ln PN 2O4 to obtain the following: ΔG = 2μ 0NO 2 – μ 0N 2O4 + 2RT ln PNO 2 – RT ln PN 2O4 2 P NO 2 ΔG = ΔG 0 + RT ln PN 2O4 , ΔG 0 = 2μ 2 0NO 2 – μ 0N 2O4 Note the significance g of ΔG and ΔGo The change ΔG is the change in the Gibbs energy function. It h has th three possible ibl ranges off value: l ΔG < 0 (process is spontaneous) ΔG = 0 ((system y is at equilibrium) q ) ΔG > 0 (reverse process is spontaneous) On the other hand ΔGo is the standard molar Gibbs energy change for the reaction. It is a constant for a given chemical reaction. We will develop these ideas for a general reaction l t iin th later the course. F For now, let’s l t’ consider id th the system t att equilibrium. Equilibrium means ΔG = 0 so: 2 P NO 2 0 0 0 = ΔG + RT ln K , ΔG = –RT ln K , K = PN 2O4 Question Which statement is true at equilibrium if K = 2? A. ΔG = -RT A RT ln(2), l (2) ΔGo = 0 B. ΔG = 0, ΔGo = -RT ln(2) C. ΔG = ΔGo = -RT ln(2) B. ΔG = 0, ΔGo = 0 Question Which statement is true at equilibrium if K = 2? A. ΔG = -RT A RT ln(2), l (2) ΔGo = 0 B. ΔG = 0, ΔGo = -RT ln(2) C. ΔG = ΔGo = -RT ln(2) B. ΔG = 0, ΔGo = 0 Temperature dependence of ΔGo The van van’tt Hoff equation We use two facts that we have derived to determine the t temperature t dependence d d off the th free f energy. Here H are we are skipping some derivations that are not often used and deriving a very useful expression in biology. ΔG 0 = –RT ln(K) ΔG 0 = ΔH 0 – TΔS 0 0 0 ΔH ΔS ln(K) = – + RT R 0 ΔH 1 – 1 ln(K 2) – ln(K 1) = R T1 T2 If we plot ln(K) vs 1/T the slope is -ΔHo/R. This is a useful expression for determining the standard enthalpy change. Example: p the formation of diamond Graphite and diamond are two forms of carbon. Given that th ffree energy off fformation the ti off diamond di d is: i C(s, graphite) C(s, diamond) ΔrGo = + 2.90 kJ/mol and the densities are: ρ(graphite) = 2.26 and ρ(diamond) = 3.51 calculate the pressure required to transform carbon into diamond. diamond Solution: Graphite will be in equilibrium with diamond when: 0 = ΔG + ΔVm P – 1 0 P = 1 – ΔG = 1 – ΔG M –M ΔVm ρ d ρ gr 0 0 Example: p the formation of diamond Plugging the values we find: 0 = ΔG 0 + ΔVm P – 1 0 0 ΔG ΔG P=1– =1– M –M ΔVm ρ d ρ gr 2900 J/mol J/ l =1– 0.012 kg/mol 1 – 1 3510 2260 9 = 1.5 x 10 Pa = 15000 bar Protein folding example: T Two state t t model d l kf U F ku Unfolded Folded K = [F]/[U] K = ff/(1-ff) ( ) Fraction folded ff Fraction unfolded 1-ff Thermodynamic y model ff = 1/(1+K) o/RT -ΔG ΔG K=e o/RT -ΔG ff = 1/(1 + e ) o/RT ΔSo/R -ΔH ff = 1/(1 + e e ) The temperature at which the protein is 50% folded can be defined as Tm the melt temperature. o o o At Tm , ΔG = 0 or Tm = ΔH /ΔS . Equilibrium q melt curves o Mostly folded o Mostly unfolded Tm In this case: Tm = 300 K = ΔH /ΔS o o Van’t Hoff plots p Slope = -ΔH /R o The standard method for obtaining the reaction enthalpy is a plot of ln K vs. 1/T Question What determines the steepness of the equilibrium melt curve? A. The melt temperature B. The equilibrium constant C. The ratio of the enthalpy to the entropy D. The magnitude of the enthalpy and entropy Question What determines the steepness of the equilibrium melt curve? A. The melt temperature B. The equilibrium constant C. The ratio of the enthalpy to the entropy D. The magnitude of the enthalpy and entropy Question What can you say about the enthalpy of reaction for the process shown in the figure p g below? A. The reaction is exothermic. B. The reaction is endothermic. C. The reaction is spontaneous. D. None of the above. Question What can you say about the enthalpy of reaction for the process shown in the figure p g below? A. The reaction is exothermic. B. The reaction is endothermic. C. The reaction is spontaneous. D. None of the above.