Lecture_Notes_091109b

# Lecture_Notes_091109b - Lecture Note

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Reaction Quotient y Reaction Quotient – (Q) determines which way a reaction needs to proceed in order to reach equilibrium. Calculated the same way as K, just with initial, not equilibrium concentrations.

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Reaction Quotient y Q = K at equilibrium y Q > K needs to proceed to reactants y Q < K needs to proceed to products
Under a particular set of conditions Q was found to be 56 for the following reaction with a K of 9.8, what will happen to the concentration of D in order to reach equilibrium? i ncrease decrease we n e d to k no w th . .. we n ow te m 22% 0% 7% 71% 1. increase 2. decrease 3. we need to know the initial concentration 4. we need to know temperature a A (g) +b B (g) c C (g) + d D (g)

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Reaction Quotient y At 2000 K the equilibrium constant for the formation of NO gas is 4.0 x 10 -4 . In a certain container the concentration of N 2 is 0.50 M, that of O 2 is 0.25 M, and that of NO is 4.2 x 10 -3 M. Is the system at equilibrium? If not, predict which way the reaction will proceed to achieve equilibrium.
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Lecture_Notes_091109b - Lecture Note

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