Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂O₂(l) → 2 H₂O(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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The Answer of Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂O₂(l)→ 2 H₂O(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. A) -26.5 kJ B) -13.3 kJ C) -0.0189 kJ D) 1.25 kJ E) -2.65 × 10⁴ kJ

Hydrogen Peroxide Decomposes to Water and Oxygen at Constant Pressure