Question

question 2 (1 point)
identify the oxidizing agent in the reaction:
$ce{al(s) + o_{2}(g) -> al_{2}o_{3}(s)}$
$\bigcirc$ $ce{al(s)}$
$\bigcirc$ $ce{o_{2}(g)}$
$\bigcirc$ $ce{al_{2}o_{3}(s)}$
$\bigcirc$ $ce{al(s)}$ and $ce{o_{2}(g)}$
$\bigcirc$ there is no oxidizing agent

Explanation:

To identify the oxidizing agent, we analyze the oxidation states. In \( \text{Al}(s) \), the oxidation state of Al is 0. In \( \text{O}_2(g) \), the oxidation state of O is 0. In \( \text{Al}_2\text{O}_3(s) \), Al has an oxidation state of +3 (so it is oxidized, losing electrons) and O has an oxidation state of -2 (so it is reduced, gaining electrons). The oxidizing agent is the species that gets reduced (causes oxidation of another species). Since \( \text{O}_2(g) \) is reduced (O goes from 0 to -2), it is the oxidizing agent.

Answer:

B. \( \text{O}_2(\text{g}) \)