handout_L07_FreeEnergy&amp;Equilib

# handout_L07_FreeEnergy&amp;Equilib - Useful Information...

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Useful Information E = q + w E = nC v T H = nC p T w =− P ext V w rev nRT ln V final V initial S = dq rev T S = k ln () Ω= A ! a i ! i S = nR ln V final V initial S = nC P ln T final T initial S = nC v ln T final T initial G =∆ G °+ RT ln( Q ) and K = Q (at equilibrium) aA + bB  → ←  cC + dD K = C [] c D d A a B b H ° rxn = c H ° f products c H ° f reac tan ts S ° rxn = cS ° products cS ° reac tan ts G ° rxn = c G ° f products c G ° f reac tan ts ln( K ) = −∆ H ° R 1 T  + S ° R ln K 2 K 1  = H ° R 1 T 2 1 T 1 Lecture 7A: G, Q, and K • Reading: Zumdahl 10.10, 10.11 • Outline – Relating G to Q – Relating G to K Relating G to Q • Recall from Lecture 6: S = R ln ( final / initial ) • For the expansion of a gas final Volume Relating G to Q (cont.) • Given this relationship S = R ln (V final /V initial ) S = R ln nRT P final nRT P initial = R ln P initial P final  =− R ln P final P initial Relating G to Q (cont.) • This equation tells us what the change in entropy will be for a change in concentration away from standard state. S fi S fi °− R ln P final P initial Entropy change for process occurring under standard conditions Additional term for change in concentration.

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handout_L07_FreeEnergy&amp;Equilib - Useful Information...

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