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The value of ΔH° for the reaction below is -126 kJ. The amount of heat that...

The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 45.0 g of Na2O2 with water is ________ kJ.

2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)

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Answer #1

           2Na2O2 (s) + 2H2O (l) → 4NaOH (s) + O2 (g)     ΔH   = -126Kj

      2 moles of Na2O2 react with H2O to release energy is -126Kj

      2*78g of Na2O2 react with H2O to release energy is -126Kj

       45g of Na2O2 react with H2O to release energy is = -126*45/2*78    = -36.35Kj >>>>answer

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