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^$\circ$C reacts with 12.00 L of nitric oxide at the same initial pressure and temperature [$\Delta$H^$\circ$_f(NO) = 90.4 kJ/mol; $\Delta$H^$\circ$_f(NO₂) = 33.85 kJ/mol; $\Delta$H^$\circ$_f(O₃) = 142.2 kJ/mol] A) -1690 kJ B) -167 kJ C) -97.6 kJ D) -69.2 kJ E) -19.7 kJ

Question

Quizplus · Accepted Answer

The enthalpy change for the reaction can be calculated using the given standard enthalpies of formation and the stoichiometry of the reaction. Given the volumes of gases involved and assuming ideal gas behavior, the reaction involves equal moles of ozone and nitric oxide reacting. The enthalpy change can be calculated using the formula ΔH = ΣΔHf(products) - ΣΔHf(reactants). The calculation leads to an enthalpy change of -69.2 kJ, indicating that option D is correct.

Ozone (O3) in the Atmosphere Can Be Converted to Oxygen ∘\circ∘

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