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)

Question

Accepted Answer

# Explanation:
To determine in which reaction oxygen is not acting as an oxidizing agent, we analyze the oxidation states of oxygen in each reaction. An oxidizing agent is a substance that gets reduced (its oxidation state decreases).

## Step 1: Analyze Reaction A
In $2C(s) + O_2(g)
ightarrow 2CO(g)$:
- Oxidation state of $O$ in $O_2$ is $0$.
- In $CO$, oxidation state of $O$ is $-2$.
- Oxidation state of $O$ decreases (from $0$ to $-2$), so $O_2$ is an oxidizing agent.

## Step 2: Analyze Reaction B
In $S(s) + O_2(g)
ightarrow SO_2(g)$:
- Oxidation state of $O$ in $O_2$ is $0$.
- In $SO_2$, oxidation state of $O$ is $-2$.
- Oxidation state of $O$ decreases (from $0$ to $-2$), so $O_2$ is an oxidizing agent.

## Step 3: Analyze Reaction C
In $2F_2(g) + O_2(g)
ightarrow 2OF_2(g)$:
- Oxidation state of $O$ in $O_2$ is $0$.
- In $OF_2$, oxidation state of $O$ is $+2$ (since $F$ has an oxidation state of $-1$, and for $OF_2$, let oxidation state of $O$ be $x$, then $x + 2(-1) = 0 \implies x = +2$).
- Oxidation state of $O$ increases (from $0$ to $+2$), so $O_2$ is being oxidized (acting as a reducing agent), not an oxidizing agent.

## Step 4: Analyze Reaction D
In $2Na(s) + O_2(g)
ightarrow Na_2O_2(s)$:
- Oxidation state of $O$ in $O_2$ is $0$.
- In $Na_2O_2$ (peroxide), oxidation state of $O$ is $-1$.
- Oxidation state of $O$ decreases (from $0$ to $-1$), so $O_2$ is an oxidizing agent.

## Step 5: Analyze Reaction E
In $2Mg(s) + O_2(g)
ightarrow 2MgO(s)$:
- Oxidation state of $O$ in $O_2$ is $0$.
- In $MgO$, oxidation state of $O$ is $-2$.
- Oxidation state of $O$ decreases (from $0$ to $-2$), so $O_2$ is an oxidizing agent.

# Answer:
C. $2 F_2(g) + O_2(g)
ightarrow 2 OF_2(g)$

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QUESTION IMAGE

Question

Explanation:

Step 1: Analyze Reaction A

Step 2: Analyze Reaction B

Step 3: Analyze Reaction C

Step 4: Analyze Reaction D

Step 5: Analyze Reaction E

Answer: