CHEM 1E03 Lecture Notes - Lecture 31: Gibbs Free Energy, Spontaneous Process
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Dilute solute higher entropy per mole than concentrated solute. Dilute solute lower gibbs energy than concentrated solute. Lower pressure gas higher entropy per mol than high-pressure gas. Lower pressure gas lower gibbs energy than high-pressure gas. K = e^(- g / rt: make sure you convert kj to j, very input sensitive, make sure everything is correct when you calculate it. Q < k forward reaction, reaction shifts right. Q > k reverse reaction, reaction shifts left. Solution: exothermic reaction, which is driven by enthalpy: g = h = t s . G = -104. 9kj 298. 2k(-290. 2/1000) divide so convert the unit. Therefore the reaction is spontaneous because g is negative: k = e^ (- g / rt) K = 1. 66 *103 (remember all units will cancel, k is unitless: q = 1/p2h2o. G = -18. 3 + ((8. 314*298)/1000) * ln (9. 7*102) G = -1. 3 kj/mol: g = g + rt ln q = 0 (set =0 because you are at equilibrium)