Question

-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

Answer 1

Answer:

-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