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:

To determine when oxygen is not an oxidizing agent, we check the oxidation state of O in each reaction. An oxidizing agent is reduced (decrease in oxidation state).

• In A, B, D, E: O in \(O_2\) (oxidation state 0) becomes -2 (in CO, \(SO_2\), \(Na_2O_2\) (O is -1, still reduced from 0), MgO), so O is reduced (oxidizing agent).
• In C: O in \(O_2\) (0) becomes +2 in \(OF_2\) (since F is -1, 2*(-1) + x = 0 → x=+2 for O). Oxidation state of O increases (oxidized), so \(O_2\) is a reducing agent here, not an oxidizing agent.

Answer:

C. \(2 F_2(g) + O_2(g)
ightarrow 2 OF_2(g)\)