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    The equilibrium constant for the following reaction is equal to 0.447 at 100°C:
    ½N2O4(g) <-> NO2(g)

    What is the value for K for the following reaction: 2NO2(g) <-> N2O4(g)?
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    (Original post by anonymous50594)
    The equilibrium constant for the following reaction is equal to 0.447 at 100°C:
    ½N2O4(g) <-> NO2(g)

    What is the value for K for the following reaction: 2NO2(g) <-> N2O4(g)?
    Do you know how to write the equilibrium law expression from the equation?
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    And your thoughts are?
 
 
 
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