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  (a)    2 NO2(g) à 2 NO(g) + O2(g) The rate law for this reaction is 2nd...

  1.   (a)    2 NO2(g) à 2 NO(g) + O2(g)

The rate law for this reaction is 2nd order.

The rate constant is k = 0.775 M¯¹s¯¹.

How much time would it require for [NO2] to go from 0.06M to 0.05M?

     (b) A 1st order reaction has a rate constant of k = 1.0 X 10¯³ s¯¹ at 25ᴼC. If the reaction rate doubles (2X faster) at 35ᴼC, what is the activation energy (Ea) for this reaction?

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