The following reaction occurs in a…

The accurate description states that the oxidation state of nitrogen in NO changes from +2 to 0, while the oxidation state of carbon in CO changes from +2 to +4 during the reaction. Explanation: An oxidizing agent is a substance that facilitates the oxidation of another while being reduced itself; this involves gaining electrons and a decrease in its oxidation state. Conversely, a reducing agent is one that reduces another substance and is oxidized in the process, leading to a loss of electrons and an increase in its oxidation state. For the provided chemical reaction: [tex]2NO(g)+2CO(g)rightarrow N_2(g)+2CO_2(g)[/tex] On the reactant side: Nitrogen’s oxidation state = +2, Carbon’s oxidation state = +2, Oxygen’s oxidation state = -2. On the product side: Nitrogen’s oxidation state = 0, Carbon’s oxidation state = +4, Oxygen’s oxidation state = -2. The oxidation state of carbon increases from +2 to +4, indicating it loses electrons and is oxidized, thus CO acts as a reducing agent. On the other hand, the oxidation state of nitrogen decreases from +2 to 0, showing it gains electrons and is reduced, making it an oxidizing agent. Therefore, the correct statement is that the oxidation state of nitrogen in NO changes from +2 to 0, and the oxidation state of carbon in CO changes from +2 to +4 during the reaction.