Tuesday, April 1, 2014
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To remember the sign and direction of Gibbs free energy change (ΔG), focus on the relationship between spontaneity, enthalpy, and entropy. A negative ΔG always indicates a spontaneous process under given conditions, while a positive ΔG means the reaction is non-spontaneous. You can remember this by thinking of Goldrolling downhill—systems naturally move toward lower free energy, just like objects move toward lower potential energy. If ΔG equals zero, the system is at equilibrium and no net change occurs. Also recall the equation ΔG = ΔH − TΔS, which links heat change and disorder to spontaneity. Favorable reactions usually have negative ΔH, positive ΔS, or both. Higher temperature makes entropy more important in determining ΔG. Overall, the sign of ΔG tells you the direction in which a reaction will naturally proceed.
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