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A different way

Posted: Thu Nov 14, 2019 7:34 pm
by 905174774
The only way I know to find the limiting reagent is to do the picket fences and see how much of the product is produced from each separate reactant. However, it does get kind of confusing. Is there any other way to find the limiting reagent that is more straight forward/ easier?

Re: A different way

Posted: Thu Nov 14, 2019 9:53 pm
by Tiffany_Chen 2K
I would say that's the most efficient and clearest way to do limiting reactant problems for this class.

Re: A different way

Posted: Sat Nov 16, 2019 12:24 am
by Melvin Reputana 1L
I also believe that is the most straight forward way. I think a good way to help you process limiting reagent problems is to list what you're given and what you're trying to find. Then compare to see which reactant produces the least amount of product which means that specific reactant is what's limiting the reaction from going into completion.

Re: A different way

Posted: Sat Nov 16, 2019 12:38 am
by Tiffany Vo 3G
If given the grams of reactants, you can technically convert each reactant to moles and then convert one of the reactants to moles of the other reactant and use the coefficients in the chemical equation to determine the limiting reactant. So for instance, if you have 2H2 + O2 --> 2H2O and you find that you have 3 moles of H2 and 1 mole of O2, you'd use the equation and determine that the O2 was the limiting reagent because the molar ratio in the chemical equation is 2 mole of H2 to 1 mole of O2. I don't know if that's easier necessarily, but it is technically another way that you could calculate limiting reagents.

Re: A different way

Posted: Sat Nov 16, 2019 12:50 am
by Amanda Lin 2I
That is probably the most efficient way because limiting reactant problems often ask for the theoretical yield of the product.

Re: A different way

Posted: Sun Dec 08, 2019 9:14 pm
by Anokhi Patel 2B
This method is very efficient, but you can also compare the moles of the reactant and then use the ratio to compare limiting reactants.

Re: A different way

Posted: Sun Dec 08, 2019 9:33 pm
by Claire Grover 3G
I consider that to be the best way to do it, but I'm not sure.

Re: A different way

Posted: Sun Dec 08, 2019 10:26 pm
by Hussain Chharawalla 1G
Also remember to always look at molar ratios when looking for the limiting reactant. This is a common mistake.

Re: A different way

Posted: Sun Dec 08, 2019 10:39 pm
by Amanda Mei 1B
I think this is the best way to do it since many problems ask you how much product will be formed anyway, so you're essentially answering that question while you determine the limiting reactant. Just convert moles of each reactant to moles of the product you'll be looking for.