Question

oxygen is acting as an oxidizing agent in all of the following reactions except
a. 2 c(s) + o₂(g) → 2 co(g)
b. s(s) + o₂(g) → so₂(g)
c. 2 f₂(g) + o₂(g) → 2 of₂(g)
d. 2 na(s) + o₂(g) → na₂o₂(s)
e. 2 mg(s) + o₂(g) → 2 mgo(s)

Explanation:

Step1: Determine the oxidation state of oxygen in each reaction

• In reaction A: In \(O_2\), the oxidation state of oxygen is \(0\). In \(CO\), oxygen has an oxidation state of \(- 2\). Oxygen is reduced (oxidation state decreases), so it acts as an oxidizing agent.
• In reaction B: In \(O_2\), oxidation state of oxygen is \(0\). In \(SO_2\), oxygen has an oxidation state of \(-2\). Oxygen is reduced, so it acts as an oxidizing agent.
• In reaction C: In \(O_2\), oxidation state of oxygen is \(0\). In \(OF_2\), oxygen has an oxidation state of \(+2\). Oxygen is oxidized (oxidation state increases), so it does not act as an oxidizing agent.
• In reaction D: In \(O_2\), oxidation state of oxygen is \(0\). In \(Na_2O_2\), oxygen has an oxidation state of \(-1\). Oxygen is reduced, so it acts as an oxidizing agent.
• In reaction E: In \(O_2\), oxidation state of oxygen is \(0\). In \(MgO\), oxygen has an oxidation state of \(-2\). Oxygen is reduced, so it acts as an oxidizing agent.

Answer:

C. \(2F_{2}(g)+O_{2}(g)\to2OF_{2}(g)\)