Limiting Reagent and Stoichiometry CR video

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Limiting Reagent and Stoichiometry CR video

Postby cassie » Thu Nov 30, 2017 11:17 am

Slide 7 quiz: stoichiometry question 2/4
True or False: Given this reaction, 80g of oxygen is enough to produce 4 moles of product.

how do we know that only 2.5 moles of O2 is the form of oxygen used in this reaction? also the explanation says 5 moles of O2 would be necessary to produce 4 moles of HNO3 is it supposed to be 7 O2 since there is a total of 7 O2 molecules on the reactant side?
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Re: Limiting Reagent and Stoichiometry CR video

Postby NS_Tutor_Andrew » Fri Dec 01, 2017 3:11 pm

Hi Cassie,

Thanks for the question! In general, when you hear references to oxygen as a product or reactant in a chemical reaction, it's pretty safe to assume that it's O2, because that's the form in which oxygen occurs in nature. This is also true for hydrogen, nitrogen, fluorine, chlorine, bromine, and iodine. Additionally, the reaction given specifies that O2 is used.

We need to distinguish the reactant oxygen (O2) from other molecules that might contain an oxygen atom. When we balance the equation, we do need to account for all atoms of oxygen, regardless of what molecule they're in -- so we will see in this equation 12 oxygen atoms on each side -- but when you read something like "80 g of oxygen is enough to produce 4 moles of product", you don't have to worry about the fact that water contains an oxygen atom too.

Hope this clarifies things, and keep up the great questions!
Andrew D.
Content Manager, Next Step Test Prep.

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