oxygen is acting as an oxidizing agent in all of the following reactions except\n\na. $2\\text{ c(s)} +…
oxygen is acting as an oxidizing agent in all of the following reactions except\n\na. $2\\text{ c(s)} + \\text{o}_2\\text{(g)} \\rightarrow 2\\text{ co(g)}$\nb. $\\text{s(s)} + \\text{o}_2\\text{(g)} \\rightarrow \\text{so}_2\\text{(g)}$\nc. $2\\text{ f}_2\\text{(g)} + \\text{o}_2\\text{(g)} \\rightarrow 2\\text{ of}_2\\text{(g)}$\nd. $2\\text{ na(s)} + \\text{o}_2\\text{(g)} \\rightarrow \\text{na}_2\\text{o}_2\\text{(s)}$\ne. $2\\text{ mg(s)} + \\text{o}_2\\text{(g)} \\rightarrow 2\\text{ mgo(s)}$
Answer
Explanation:
Step1: Define oxidizing agent
An oxidizing agent gains electrons and its oxidation state decreases.
Step2: Analyze reaction A
Carbon state increases from $0$ to $+2$; Oxygen decreases from $0$ to $-2$. $$2\text{C}(s) + \text{O}_2(g) \rightarrow 2\text{CO}(g)$$
Step3: Analyze reaction B
Sulfur state increases from $0$ to $+4$; Oxygen decreases from $0$ to $-2$. $$\text{S}(s) + \text{O}_2(g) \rightarrow \text{SO}_2(g)$$
Step4: Analyze reaction C
Fluorine is more electronegative than oxygen. Oxygen state increases from $0$ to $+2$. $$2\text{F}_2(g) + \text{O}_2(g) \rightarrow 2\text{OF}_2(g)$$
Step5: Analyze reaction D
Sodium state increases from $0$ to $+1$; Oxygen decreases from $0$ to $-1$. $$2\text{Na}(s) + \text{O}_2(g) \rightarrow \text{Na}_2\text{O}_2(s)$$
Step6: Analyze reaction E
Magnesium state increases from $0$ to $+2$; Oxygen decreases from $0$ to $-2$. $$2\text{Mg}(s) + \text{O}_2(g) \rightarrow 2\text{MgO}(s)$$
Answer:
C. $2\text{F}_2(g) + \text{O}_2(g) \rightarrow 2\text{OF}_2(g)$