Asked by Karla
Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:
2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure?
2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide decomposes at constant pressure?
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