lecture3 - General Chemistry II - X19B Week 3 Lecture...

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General Chemistry II - X19B Week 3 Lecture Principles of Reactivity: Chemical Equilibria
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Fe 2 0 3 + 2Al Al 2 O 3 + 2Fe Irreversible Reaction ice
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N 2 O 4 2NO 2
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Reversible Reaction More Products? More Reactants? N 2 O 4 2NO 2 Rate = k f [N 2 O 4 ] Rate = k r [NO 2 ] 2
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Dynamic Equilibrium can be reached with any mixture of reactants or products. N 2 O 4 2NO 2 Rate = k f [N 2 O 4 ] = k r [NO 2 ] 2 Equilibria
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Equilibrium Constant N 2 O 4 2NO 2 Rate = k f [N 2 O 4 ] Rate = k r [NO 2 ] 2 k f [N 2 O 4 ] = k r [NO 2 ] 2 k f / k r = [NO 2 ] 2 / [N 2 O 4 ] K c = [NO 2 ] eq 2 / [N 2 O 4 ] eq
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Equilibrium Constant N 2 O 4 2NO 2 K c = [NO 2 ] eq 2 / [N 2 O 4 ] eq Concentrations are at equilibrium Products over reactants Concentration raised to stoich power K depends on reaction and temp no units in K In general, aA + bB cC+ dD, K = [C] c [D] d / [A] a [B] b
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Equilibrium Constant N 2 O 4 (g) 2NO 2 (g), K c K c = [NO 2 ] eq 2 / [N 2 O 4 ] eq H 2 (g) + I 2 (g) 2HI(g), K p
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This note was uploaded on 02/09/2012 for the course CHEMISTRY 101 taught by Professor Endy during the Spring '11 term at Harvard.

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lecture3 - General Chemistry II - X19B Week 3 Lecture...

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