CH302 Chapter 6 Notes part 2

CH302 Chapter 6 - Q = K Reaction IS already at equilibrium no shift Q> K Product concentration is too high Reaction must shift to the left to

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CH302 Chapter 6 notes part 2 K and Reaction Extent K > 1 Equilibrium lies to the right : System will contain more product than reactant. (K >>> 1: reaction goes to completion) K < 1 Equilibrium lies to the left : System will contain more reactant than product. (K <<< 1: very little reaction occurs) Reaction Quotient Looks very similar to the expression for K, BUT the concentrations are those of the INITIAL setup. .. For a simple reversible reaction: j A + k B « l C + m D The reaction quotient is: Q = [C] l [D] m [X] = INITIAL concentration of X [A] j [B] k Q vs. K: Shift in System
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Unformatted text preview: Q = K Reaction IS already at equilibrium: no shift. Q > K Product concentration is too high: Reaction must shift to the left to reach equilibrium Q < K Product concentration is too low: Reaction must shift to the right to reach equilibrium Example K = 49 at 450 o C for this reaction: H 2(g) + I 2(g) ↔ 2HI (g) If 0.22 mole of I 2 , 0.22 mole of H 2 , and 0.66 mole of HI were put into an evacuated 1.00-liter container, would the system be at equilibrium? If not, what must occur to establish equilibrium?...
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This note was uploaded on 06/13/2011 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.

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