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

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} Fe=(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=
`(3)/(2)* 0.455=0.682moles` of
`Cl_2`

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

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