Answer:
The limiting reactant (or limiting reagent) in a chemical reaction is the reactant that is completely consumed before the other reactants are used up. The amount of product that can be formed in a chemical reaction is limited by the amount of the limiting reactant. The percent yield of a reaction is the ratio of the amount of product that is actually formed to the maximum amount of product that could be formed, expressed as a percentage.
For example, suppose we have a reaction that converts reactant A into product B, and we have a certain amount of reactant A and a certain amount of reactant B. If the reactant A is completely used up before reactant B, then reactant A is the limiting reactant. The maximum amount of product B that can be formed in the reaction is equal to the amount of limiting reactant (in this case, reactant A) that is consumed. If the actual yield of product B is less than this maximum amount, then the percent yield of the reaction will be less than 100%.
To calculate the percent yield of a reaction, we use the following formula:
% yield = (actual yield / theoretical yield) x 100
where the theoretical yield is the m