Find the mass of AlCl3 that is produced when 10.0 grams of Al2O3 react with 10.0 g of HCl according to the following equation. Al2O3(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2O(aq)

The mass of aluminium chloride produced is 12.17 grams

Explanation:

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

    .....(1)

Given mass of aluminium oxide = 10.0 g

Molar mass of aluminium oxide = 102 g/mol

Putting values in equation 1, we get:

Given mass of HCl = 10 g

Molar mass of HCl = 36.5 g/mol

Putting values in equation 1, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

6 moles of HCl reacts with 1 mole of aluminium oxide

So, 0.274 moles of HCl will react with = of aluminium oxide

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

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

By Stoichiometry of the reaction:

6 moles of HCl produces 2 moles of aluminium chloride

So, 0.274 moles of HCl will produce = of aluminium chloride

Now, calculating the mass of aluminium chloride from equation 1, we get:

Molar mass of aluminium chloride = 133.34 g/mol

Moles of aluminium chloride = 0.0913 moles

Putting values in equation 1, we get:

Hence, the mass of aluminium chloride produced is 12.17 grams

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.