STOICHIOMETRY - Limiting Reactant & Excess Reactant Stoichiometry & Moles
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- เผยแพร่เมื่อ 15 มี.ค. 2012
- STOICHIOMETRY - Limiting Reactant & Excess Reactant Stoichiometry & Moles - A video showing two examples of how to solve Limiting Reactant stoichiometry problems. This video also explains how to determine the excess reactant too. Stoichiometry can be a difficult concept, tune in to see how easy it can be.
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Hey bro, thanks for the keen eye. In the first example, oxygen was given in liters so I used 22.4L per mole. Hope that helps.
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Picture this, when you are given a length in feet, such as 6 feet, and are asked to convert to inches, what do you do? You would use a conversion factor such as 12 in = 1 ft. The key is that you need a conversion factor! When you are given the volume of a gas in liters, such as 20 L as the video shows, you need to convert that out of Liters and into moles. In order to convert it, you need a conversion factor.
wait don't u have to convert liters to grams on the second stochiometry problem
there is a stoichometry formula used to convert L to grams
@Alexis Rivera that would only work if it was in grams, but its 20L. The conversion factor between moles and litres is 22.4L/mol at STP. however, the question did not specify that the O2 was gaseous, or that it was at STP, thus the question is done incorrectly. Just little things, but watch out for things like that on a test.
when converting from liters to moles (which you had to do to solve the first problem), 22.4 is a standard conversion factor.
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Wow, this helped so much! Thank you!
how did you get the 22.4l as the bottom half of the second reaction shown.. a bit confused to how you get 22.4l
how did you know what numbers to put in for the balancing
So to get the 130g for the max amount of CaO made from 37.1g of oxygen... Did you multiply 64.96 (Moles of O2 x formula mass of CaO) by 2, since we are looking for the amount of O, rather than O2?
To find the amount of ER, try using stoich to go from reactant to reactant. Then you'll find how much reactant is needed to see the reaction through. Subtract that from the amount o reactant given in the problem.
Just like 12 in = 1 ft, 22.4 liters = 1 mole of O2. This means that in 1 mole of O2 gas, there is a mole of molecules! So, 22.4 L is just a conversion factor, the same way 12 in & 1 ft are conversion factors. I really hope this explanation was helpful.
but how did u get 22.4??
1) Take the limiting reactant amount, then use stoichiometry to convert it into the excess reactant. (Make sure you convert it to the same unit of measurement that the givens were originally expressed in). 2) You should now be in either grams, liters or molecules.... for the excess reactant, this is how much you need to use up all of your limiting reactant. 3) Subtract this amount from the given of the excess reactant. This gives you the amount of excess reactant left over.
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Hey Rain! Thanks for tuning in. Best wishes on your exam! Be awesome!
Nice
umm, quick question. O2 started in Liters, how did it end up in grams?
and is 22.4L converted from 16g?
What do you add together get the ending number
excellent explanation
Thank You!
@TheDaniel7310, 24.33 & 22.4 are the molar masses of magnesium & oxygen.
I love your videos, you definitely explain it 10 times better than my chem teacher. Just one suggestion: You seem to always say "cancel" when it comes to units, but the correct mathematical term is "divide out". Because if they just "canceled", where would they go??
Matthew Troutman Love the feedback. Thanks for the recommendation bro!
where did u get 22.4 liters of o2 6:30
I guess 22.4 L is a conversion factor. It's the volume of a gas at STP? I suppose? I don't know. Do we have enough info to make those assumptions?
Emily Kight That is correct, its the "STP" (or standard temperature and pressure) of O2. "At STP, the molar volume of an ideal gas is 22.4 L. In other words, the volume of 1 mol of a gas like oxygen is 22.4 L. (mol/22.4L) or (22.4L/mol)" Source: (www.wyzant.com/resources/answers/2247/how_many_oxygen_molecules_are_present_in_113_97_liters_of_oxygen_gas_at_stp)
if i were to find the difference between the E.R. and the L.R. then reverse the molar conversion step would that give me the amount of E.R.?