When 125 grams of feo react with 25.0 grams of al, how many grams of fe can be produced? feo + al → fe + al2o3 25.9 g fe 38.7 g fe 50.9 g fe 77.6 g fe

The mass of iron produced will be 77.6 grams

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of FeO = 125 g

Molar mass of FeO = 71.8 g/mol

Putting values in equation 1, we get:

Given mass of aluminium = 25.0 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

The given chemical reaction follows:

By Stoichiometry of the reaction:

2 moles of aluminium metal reacts with 3 mole of FeO

So, 0.93 moles of aluminium metal will react with = of FeO

As, given amount of FeO is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium metal is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of aluminium metal produces 3 mole of iron metal

So, 0.93 moles of aluminium metal will produce = of iron metal

Molar mass of iron = 55.85 g/mol

Moles of iron = 1.395 moles

Putting values in equation 1, we get:

Hence, the mass of iron produced will be 77.6 grams

passing a magnet thought the

mixture , because iron gets attracted to magnet .