88 MULTIPLE CHOICE Question 10 The chemical equation below shows the reaction that takes place when rust forms. How many moles of oxygen are required to make 2 moles of iron (III) ox- ide (Fe_(2)O_(3)) 4Fe_((s))+3O_(2(g))arrow 2Fe_(2)O_((s)) A 1 mole B 2 moles C 4 moles D 3 moles

## Step 1
The given chemical equation is:
$$4Fe_{(s)}+3O_{2(g)}\rightarrow 2Fe_{2}O_{3(s)}$$
This equation tells us that 4 moles of iron (Fe) react with 3 moles of oxygen (O2) to produce 2 moles of iron (III) oxide (Fe2O3).

## Step 2
We are asked to find out how many moles of oxygen are required to produce 2 moles of iron (III) oxide.

## Step 3
We can set up a proportion to solve this:
$$\frac{3 \text{ moles of } O_{2}}{2 \text{ moles of } Fe_{2}O_{3}} = \frac{x \text{ moles of } O_{2}}{2 \text{ moles of } Fe_{2}O_{3}}$$

## Step 4
Solving for x gives us:
$$x = \frac{3}{2} \times 2 = 3$$