Mx2, X2, MX3 how is it limiting reactant
The limiting reactant is the reactant that is completely consumed during a chemical reaction, thereby limiting the amount of product that can be formed.
In order to determine the limiting reactant, one must compare the stoichiometric ratios of the reactants to the balanced equation for the reaction.
For example, let's consider the reaction:
2Mx + X2 → 2MX3
The stoichiometry of the reaction tells us that 2 moles of Mx react with 1 mole of X2 to form 2 moles of MX3.
If we have 1 mole of Mx and 1 mole of X2, we can see that according to the stoichiometry, only half of the X2 can react to form the product, as there is not enough Mx present.
Therefore, in this case, X2 is the limiting reactant, as it limits the formation of the product MX3.