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Equilibrium shift

Discussion in 'DAT Discussions' started by pandalove89, Jul 30, 2011.

  1. pandalove89

    7+ Year Member

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    say we have this reaction:


    2 NOBr (g) <--- ---> 2NO (g) + Br2 (g) and delta H = -30 KJ


    So at this state the reaction is exothermic.


    However if we increase the temperature of this reaction which way would the equilibrium shift.

    On the other hand, if we decrease the temperature which way would the equilibrium shift?
     
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  3. LetsGo2DSchool

    Removed 2+ Year Member

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    The best fool proof way to attack these problems is to think of the heat as either a reactant (endothermic) or product (exothermic).

    Thus in the above exothermic rxn, if you increase the temp (add heat), then the system will shift to the left to use up some of this excess heat.

    Similarly, if you decrease the temp (remove heat), then the system will shift to the right to generate more heat.

    Pretty simple, right? Now you should get every one of these questions correct.
     

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