L3 - Spontaneous processes? Gibbs free energy G = H -...

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1 Spontaneous processes? Gibbs free energy G = H - TS Δ G < 0 exergonic (reaction is spontaneous) Δ G > 0 endergonic (reaction is non-spontaneous) Δ G = 0 equilibrium Δ G = Δ H - T Δ S
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2 Reactions can be driven by enthalpy or entropy
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3 nA + oB pC + qD Δ G = Δ G° + RT ln ([C] p [D] q /[A] n [B] o ) Δ G varies with the concentration of reactants and products R = Gas constant (8.31 J K -1 mol -1 )
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4 At equilibrium the rate of the forward reaction is equal to the rate of the reverse reaction Equilibrium is established at a speciFc ratio of reactants and products K eq = [C] p [D] q /[A] n [B] o eq eq eq eq Δ G = 0 nA + oB π C + qD
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5 Δ G = Δ G° + RT ln ([C] p [D] q /[A] n [B] o ) Δ G° = -RT ln K eq K eq = e - Δ G°/RT The equilibrium constant depends on the standard state free energy ( Δ G°)
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6 Standard state conventions for biochemists Temperature = 25°C (298°K) Pressure = 1 atm activity of solutes = 1 activity of pure water is assigned 1 H + activity at pH 7.0 = 1
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This note was uploaded on 05/07/2011 for the course CHEM 365 taught by Professor Huxford during the Spring '08 term at San Diego State.

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L3 - Spontaneous processes? Gibbs free energy G = H -...

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