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 3.00 g of hydrogen peroxide decomposes at constant pressure? 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 3.00 g of hydrogen peroxide decomposes at constant pressure? - 1.73 * 104 kJ 1.92 kJ - 8.65 kJ - 17.3 kJ - 0.0289 kJ

Question

Chemistry

Davis Hodge

8 February, 18:03

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 3.00 g of hydrogen peroxide decomposes at constant pressure? 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 3.00 g of hydrogen peroxide decomposes at constant pressure? - 1.73 * 104 kJ 1.92 kJ - 8.65 kJ - 17.3 kJ - 0.0289 kJ

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Answers (1)

Know the Answer?

Keira Kaiser · Answer 1

-8.64kJ

Explanation:

Based on the reaction:

2 H₂O₂ (l) → 2 H₂O (l) + O₂ (g) ΔH = - 196 kJ

When 2 moles of hydrogen peroxide (H₂O₂) descomposed, there are released - 196kJ of energy.

Now, if 3,00g of hydrogen peroxide react, moles are:

3.00g * (1mol / 34.01g) = 0.0882moles H₂O₂

Releasing:

0.0882moles H₂O₂ * (-196kJ / 2mol H₂O₂) = - 8.64kJ