Al + Fe3O4 → Al2O3 + Fe. 13. How many grams of iron are produced by the reaction of 225.0 grams of Al and 225.0 grams of Fe3O4? 14. How many grams of Al2O3 are also produced in the reaction of (23)?

Explanation:

Hello,

In this case, by the following balanced reaction:

The first step is to identify the limiting reactant, for which we compute the available moles of aluminium in 225.0 g by using its atomic mass:

Next. we compute the consumed moles of aluminium by 225.0 g of iron (II,III) oxide by using its molar mass and the 8:3 molar ratio between them:

In such a way, since more Al is available, we conclude it is in excess and iron (II,III) oxide is the limiting reactant, therefore, we can compute the produced grams of both iron and aluminium oxide as shown below:

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the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .