Solved: FeCl3 Limiting Reagent; Excess O2 Remains Unused

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Discussion Overview

The discussion revolves around a stoichiometry problem involving the reaction of iron(III) chloride (FeCl3) with oxygen (O2) to determine the limiting reagent and the amount of excess reagent remaining after the reaction. The context is primarily homework-related, focusing on the calculation of moles and theoretical yields.

Discussion Character

  • Homework-related
  • Mathematical reasoning

Main Points Raised

  • Participants discuss identifying the limiting reagent in the reaction between FeCl3 and O2, with some suggesting that O2 is the limiting reagent based on the stoichiometric ratios.
  • There is a debate on whether to use moles or grams for calculations, with one participant asserting that either unit can be used.
  • One participant describes their method of calculating the limiting reagent by relating the moles of O2 to the moles of FeCl3 using the stoichiometric coefficients from the balanced equation.
  • Another participant works backwards from the theoretical yield of Cl2 to determine how much FeCl3 is required, leading to a calculation of the excess reagent.
  • Participants express uncertainty about the calculations and seek confirmation on whether their reasoning makes sense.

Areas of Agreement / Disagreement

There is no explicit consensus on the calculations, as participants express uncertainty and seek clarification on their methods. Multiple approaches to determining the limiting reagent and the excess remain present in the discussion.

Contextual Notes

Some calculations involve assumptions about the stoichiometric relationships and the use of moles versus grams, which may not be fully resolved within the discussion.

Who May Find This Useful

This discussion may be useful for students working on stoichiometry problems in chemistry, particularly those involving limiting reagents and theoretical yields in chemical reactions.

UWMpanther
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[SOLVED] Last Stoich I swear

Homework Statement


When FeCl3 is ignited in an atmosphere of pure oxygen, this reaction takes place
4FeCl3 + 3O2 -> 2Fe2O3 + 6Cl2

If 3.00 mol of FeCl3 are ignited in the presence of 2.00 mol of O2 gas, how much of which reagent is present in excess and therefore remains unused?


Now I don't know where to go from here. Obviously solve for the limiting reagent. Then I need some type of ratio to solve for how many mol are used
 
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So which one is the limiting reagent? Or do you need help on that part as well? We can start from there if you'd like.
 
I think the limiting reagent is the O2 but I don't know how to caculate it since it is given in mol not g.
 
UWMpanther said:
I think the limiting reagent is the O2 but I don't know how to caculate it since it is given in mol not g.
It doesn't matter at all. You can use either moles or grams.

Anyways, you're correct about O2 being the LR. It produces only 4.00 mol of Cl2 (Theoretical Yield), while FeCl3 produces 4.50 mol of Cl2.
 
Ok cool I got that far then when I was just guessing. So I basically went something like this:

since in the equation their relationship is 4FeCl2 to 3O2, I just took the 2O2 x 1.5 so it was equal to the 3.0 mol given. So that put 4FeCl2 to 4.5 mol. But I guess that's all I solved for the LR.

So next step would be, I'm assuming a relationship between the two. Maybe:

4.0 mol O2 x 4mol FeCl3/3mol O2 = 5.33mol FeCl3?
 
Ok since we only produce 4.00 mol Cl2 with O2, we use this same number and find how much FeCl3 is needed to produce 4.00 mol of Cl2.

So working backwards:

\mbox{4.00 mol} Cl_2 \times \frac{\mbox{2.00 mol}}{\mbox{3.00 mol}} \frac{FeCl_{2}}{Cl_{2}} = \frac{8}{3}\mbox{mol} FeCl_{3}

We started out with 3.00 mol FeCl3, so it's just the difference.

3.00 mol FeCl3 - 8/3 mol FeCl3 = ?

Does the answer make sense?
 
Last edited:
Ok yeah that makes sense so the difference is .33

Thank you so very much!
 

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