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

-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

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.