Question

Ozone, o3(g) , is a form of elemental oxygen that is important in the absorption of ultraviolet radiation in the stratosphere. it decomposes to o2(g) at room temperature and pressure according to the following reaction: 2o3(g)→3o2(g)δh=−284.6kj,what is the enthalpy change for this reaction per mole of o3(g) ?

Answer 1

The enthalpy change for the decomposition of ozone (O3) into oxygen (O2) per mole of ozone is -142.3 kJ/mole, obtained by dividing the total enthalpy change (-284.6 kJ) by the number of moles of ozone (2 mol).

Step-by-step explanation:

The student is looking to find the enthalpy change of the reaction where ozone (O3) decomposes into oxygen (O2) per mole of O3. The reaction provided is:

2 O3(g) → 3 O2(g) ΔH = -284.6 kJ

This means that -284.6 kJ of heat is released when 2 moles of ozone decompose into 3 moles of oxygen. To find the enthalpy change per mole of O3, we divide the total enthalpy change by the number of moles of O3 reacting.

ΔH per mole of O3 = Total ΔH / number of moles of O3

ΔH per mole of O3 = -284.6 kJ / 2 moles of O3

ΔH per mole of O3 = -142.3 kJ/mole

Thus, the enthalpy change for the reaction per mole of ozone is -142.3 kJ/mole.