determine whether each reaction is a redox reaction. for each redox reaction, identify the oxidizing agent…

determine whether each reaction is a redox reaction. for each redox reaction, identify the oxidizing agent and the reducing agent. for each redox reaction, identify the oxidizing agent and the reducing agent.\na. 4 li(s) + o₂(g) → 2 li₂o(s)

determine whether each reaction is a redox reaction. for each redox reaction, identify the oxidizing agent and the reducing agent. for each redox reaction, identify the oxidizing agent and the reducing agent.\na. 4 li(s) + o₂(g) → 2 li₂o(s)

Answer

Explanation:

Step1: Determine oxidation states

In $Li(s)$, the oxidation state of $Li$ is $0$. In $O_2(g)$, the oxidation state of $O$ is $0$. In $Li_2O(s)$, the oxidation state of $Li$ is $+ 1$ and of $O$ is $-2$.

Step2: Check for redox reaction

$Li$ changes from $0$ to $+1$ (oxidation, loss of electrons), and $O$ changes from $0$ to $-2$ (reduction, gain of electrons). So this is a redox reaction.

Step3: Identify oxidizing and reducing agents

The substance that is reduced is the oxidizing agent. Here, $O_2$ is reduced, so $O_2$ is the oxidizing agent. The substance that is oxidized is the reducing agent. Here, $Li$ is oxidized, so $Li$ is the reducing agent.

Answer:

This is a redox reaction. The oxidizing agent is $O_2$, and the reducing agent is $Li$.