oxygen is acting as an oxidizing agent in all of the following reactions except
a.
$2 c(s) + o_2(g) \
ightarrow 2 co(g)$
b.
$s(s) + o_2(g) \
ightarrow so_2(g)$
c.
$2 f_2(g) + o_2(g) \
ightarrow 2 of_2(g)$
d.
$2 na(s) + o_2(g) \
ightarrow na_2o_2(s)$
e.
$2 mg(s) + o_2(g) \
ightarrow 2 mgo(s)$

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:

## Step 1: Recall the definition of an oxidizing agent
An oxidizing agent is a substance that gets reduced (its oxidation state decreases) during a reaction.

## Step 2: Analyze Reaction A
In $2C(s)+O_2(g)
ightarrow2CO(g)$:
- 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 reduced (oxidizing agent).

## Step 3: 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 reduced (oxidizing agent).

## Step 4: Analyze Reaction C
In $2F_2(g)+O_2(g)
ightarrow2OF_2(g)$:
- 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 $OF_2$: $x + 2(-1)=0\Rightarrow x = + 2$).
- Oxidation state of $O$ increases from $0$ to $+2$, so $O_2$ is oxidized (not an oxidizing agent).

## Step 5: 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 reduced (oxidizing agent).

## Step 6: Analyze Reaction E
In $2Mg(s)+O_2(g)
ightarrow2MgO(s)$:
- 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 reduced (oxidizing agent).

# Answer:
C. $2F_2(g)+O_2(g)
ightarrow2OF_2(g)$

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QUESTION IMAGE

Question

Explanation:

Step 1: Recall the definition of an oxidizing agent

Step 2: Analyze Reaction A

Step 3: Analyze Reaction B

Step 4: Analyze Reaction C

Step 5: Analyze Reaction D

Step 6: Analyze Reaction E

Answer: