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 8.50 L 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?

Given:
- \( R = 0.0821 \, \text{L} \cdot \text{atm} / \text{mol} \cdot \text{K} \)
- \( \Delta H_f^\circ(\text{NO}) = 90.4 \, \text{kJ/mol} \)
- \( \Delta H_f^\circ(\text{NO}_2) = 33.85 \, \text{kJ/mol} \)
- \( \Delta H_f^\circ(\text{O}_3) = 142.2 \, \text{kJ/mol} \)

Select one:
A. –19.7 kJ
B. –69.1 kJ
C. –1690 kJ
D. –167 kJ
E. –97.6 kJ