Question

question 2 (1 point)
identify the oxidizing agent in the reaction:
$ce{al}(s) + ce{o_2}(g) \
ightarrow ce{al_2o_3}(s)$
$\bigcirc$ $ce{al}(s)$
$\bigcirc$ $ce{o_2}(g)$
$\bigcirc$ $ce{al_2o_3}(s)$
$\bigcirc$ $ce{al}(s)$ and $ce{o_2}(g)$
$\bigcirc$ there is no oxidizing agent

Explanation:

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

Answer:

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