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Can somone make the subject of limiting reagents easier for me?


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So I just recently started properly reading and studying into the science subjects, and up now is Chemistry. I am using Zumdahl's book as my crutch. I am somewhat confused on the issue of limiting reagents (under Stoichiometry) and was wondering if anyone could make it clearer. I googled it, and sites like Wikipedia made me somehow more confused.




In the first example, why does it feel to me like a given was missing? And in the second example, where did we get the 157.9g from? Much thanks for the help.

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In the first example they fail to give you the original balanced equation, or the fact that you start with 1.5 mol of benzene and 7 mol of oxygen. It seems to me like they just left out the question itself. And as for the 157.9 g/mol, that's the molecular weight of Iron (3) oxide (found from a periodic table).


As for the first part, do you not understand what a limiting reagant is, or just how to find one?

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Thanks for your reply. I don't understand how to find one. What I do know is that the limiting reagent is the reactant that's consumed first and thus it signals the end of the product sum that can be formed. Much thanks again.

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The simplest way is to calculate how many moles of product will be formed for each reactant - so if you have x moles of H2O, calculate how much product will be formed, and if the other reactant is HCl, and you have y moles, do the calculation again with that number.


The reactant that produces the lowest number is the limiting reactant.


Borek, please stop advertising (what I presume is) your site.

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