Respuesta :
0.5 mol
The chemical formula give shows that for every 2 mols of Al, 2 mols of AlCl3 is produced. That is a one to one ratio. Since 0.5 mols of aluminum is provided .5 mols of AlCl3 results.
The theoretical yield of aluminium chloride [tex]\left( {{\text{AlC}}{{\text{l}}_{\text{3}}}} \right)[/tex] in moles is [tex]\boxed{{\text{0}}{\text{.50 mol}}}[/tex].
Further Explanation:
Limiting reagent:
It is completely consumed in a chemical reaction. It decides the amount of product formed in any chemical reaction. The amount of product depends on the amount of limiting reagent since the product formation is not possible in the absence of it.
Stoichiometry:
It is used to determine the amount of species present in the reaction by the relationship between reactants and products. It is used to determine the moles of a chemical species when moles of other chemical species present in the reaction is given.
Consider the general reaction,
[tex]{\text{A}} + 2{\text{B}} \to 3{\text{C}}[/tex]
Here,
A is the reactant.
B is the reactant.
C is the product.
One mole of A reacts with two moles of B to produce three moles of C. The stoichiometric ratio between A and B is 1:2, the stoichiometric ratio between A and C is 1:3 and the stoichiometric ratio between B and C is 2:3.
The given reaction occurs as follows:
[tex]2{\text{Al}}\left(s\right)+3{\text{C}}{{\text{l}}_2}\left(g\right)\to2{\text{AlC}}{{\text{l}}_3}\left(s\right)[/tex]
According to the stoichiometry of the reaction, two moles of Al reacts with three moles of [tex]{\text{C}}{{\text{l}}_2}[/tex] to form three moles of [tex]{\text{AlC}}{{\text{l}}_{\text{3}}}[/tex].
Since aluminium is the limiting reagent, the formation of [tex]{\text{AlC}}{{\text{l}}_{\text{3}}}[/tex] will occur according to the amount of Al.
According to the balanced chemical reaction, the stoichiometric ratio between Al and [tex]{\text{AlC}}{{\text{l}}_{\text{3}}}[/tex] is 2:2 or 1:1. So the number of moles of [tex]{\text{AlC}}{{\text{l}}_{\text{3}}}[/tex] produced by 0.50 mol of Al will also be 0.50 mol.
Therefore the theoretical yield of aluminium chloride (in moles) is 0.50 mol.
Learn more:
1. Calculate the moles of chlorine in 8 moles of carbon tetrachloride: https://brainly.com/question/3064603
2. Calculate the moles of ions in the solution: https://brainly.com/question/5950133
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Mole concept
Keywords: Al, AlCl3, Cl2, 3Cl2, 2Al, 0.50 mol, stoichiometry, limiting reagent, A, B, C, two moles, three moles.
