Calculate the number of moles of chlorine needed to form 14 moles of iron (III) chloride. 2Fe + 3Cl2 --> 2FeCl3.

Answer 1

To find the number of moles of chlorine needed to form 14 moles of iron (III) chloride (FeCl₃), we can use the balanced chemical equation:

$$2\text{Fe}+3{\text{Cl}}_2\to 2{\text{FeCl}}_3$$

From the equation, we can see the stoichiometry between FeCl₃ and Cl₂:

• 2 moles of FeCl₃ are formed from 3 moles of Cl₂.

This means that for every 2 moles of FeCl₃, we need 3 moles of Cl₂. We can set up a ratio to find the number of moles of Cl₂ needed for 14 moles of FeCl₃:

$$\frac{3{\text{ moles Cl}}_2}{2{\text{ moles FeCl}}_3}=\frac{x{\text{ moles Cl}}_2}{14{\text{ moles FeCl}}_3}$$

Now, we can solve for $x$:

$$x=14{\text{ moles FeCl}}_3\times \frac{3{\text{ moles Cl}}_2}{2{\text{ moles FeCl}}_3}$$

Calculating this gives:

$$x=14\times \frac{3}{2}=14\times 1.5=21$$

Thus, 21 moles of chlorine (Cl₂) are needed to form 14 moles of iron (III) chloride (FeCl₃).