Ozone (O₃)in the atmosphere can be converted to oxygen gas by reaction with nitric oxide (NO). Nitrogen dioxide is also produced in the reaction. What is the enthalpy change when 8.50L of ozone at a pressure of 1.00 atm and 25°C reacts with 12.00 L of nitric oxide at the same initial pressure and temperature? [$\Delta$H°_f(NO)= 90.4 kJ/mol; $\Delta$H°_f(NO₂)= 33.85 kJ/mol; $\Delta$H°_f(O₃)= 142.2 kJ/mol]

Question

Quizplus · Accepted Answer

The correct answer is A.The enthalpy change for the reaction can be calculated using the following equation:ΔH° = ΣΔH°_f(products) - ΣΔH°_f(reactants)ΔH° = [ΔH°_f(NO₂)] - [ΔH°_f(O₃) + ΔH°_f(NO)]ΔH° = [(33.85 kJ/mol) - (142.2 kJ/mol) + (90.4 kJ/mol)]ΔH° = -19.7 kJThe negative sign indicates that the reaction is exothermic, meaning that heat is released when the reaction occurs.

Ozone (O3)in the Atmosphere Can Be Converted to Oxygen Gas Δ\DeltaΔ

Ozone (O₃)in the Atmosphere Can Be Converted to Oxygen Gas $\Delta$