One key reaction used in making nitric acid is the catalytic oxidation of ammonia. $4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g)$ For each mole of $\text{O}_2$ that undergoes this reaction, 181.8 kJ of energy is released. A factory produces $2.50 \times 10^5$ mol of NO per day. What quantity of energy, in kJ, is released each day?
- A$3.64 \times 10^7$
- B$4.55 \times 10^7$
- C$5.68 \times 10^7$
- D$2.27 \times 10^8$