A key reaction used in the production of 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 $\text{O}_2$ consumed in this reaction, $181.8\,\text{kJ}$ of energy are given out. A factory produces $2.50 \times 10^5\,\text{mol}$ of NO each day. What amount of energy, in kJ, is released in one day?
- A$3.64 \times 10^7$
- B$4.55 \times 10^7$
- C$5.68 \times 10^7$
- D$2.27 \times 10^8$