Question

According to the following reaction, how many grams of chlorine gas are required for the complete reaction of 25.5 grams of iron?
iron (s) + chlorine (g) iron(III) chloride (s)
_____grams chlorine gas

Answer 1

Answer: 48.4 g of $Cl_2$ will be produced from 25.5 g of iron

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$    

$\text{Moles of} Fe=\frac{25.5 g}{56g/mol}=0.455moles$

The balanced chemical reaction is:

$2Fe(s)+3Cl_2(g)\rightarrow 2FeCl_3(s)$  

According to stoichiometry :

2 moles of $Fe$ require  = 3 moles of $Cl_2$

Thus 0.455 moles of $Fe$ will require=$\frac{3}{2}\times 0.455=0.682moles$  of $Cl_2$

Mass of $Cl_2=moles\times {\text {Molar mass}}=0.682moles\times 71g/mol=48.4g$

Thus 48.4 g of $Cl_2$ will be produced from 25.5 g of iron