The decomposition of hydrogen peroxide as represented by the equation below follows the first-order rate law.                   2H2O2(aq)  -->  2H2O(l)  + O2(g)          Rate = -D[H2O2]/Dt = k[H2O2], where k = 3.2 x 10-5 s–1 at room temperature.

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The decomposition of hydrogen peroxide as represented by the equation below follows the first-order rate law.

                  2H2O2(aq)  -->  2H2O(l)  + O2(g)

         Rate = -D[H2O2]/Dt = k[H2O2], where k = 3.2 x 10-5 s–1 at room temperature.

      Which of the following represents an approximate half-life for this reaction?  

         (A) 87 hrs

          (B) 8.7 hrs

          (C) 6.0 hrs

          (D) 17 hrs

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