Interpret the following equation using moles, molecules, volumes (assume STP). How would the mass of the reactants compare to the mass of the product? #2N_2(g) + 3O_2(g) -> 2N_2O_3(g)#?

1 Answer
anor277
Aug 3, 2017

Well, conservation of mass applies ABSOLUTELY in every chemical reaction.

Explanation:

And thus #10*g# of reactants, gives #10*g# products. And in the event of LESS than 100% yield, the TOTAL MASS of PRODUCTS AND REACTANTS is STILL CONSTANT AT #10*g#.

You have got........

#2N_2(g) + 3O_2(g)rarr2N_2O_3(g)#

#N_2O_3# is formally a mixed valence compound of #stackrel(+II)N# and #stackrel(+IV)N#, i.e the average oxidation state is #N(+III)#. We would assume a pressure drop in the reaction......why? I also have an idea that #N_2O_3# is relatively high boiling.

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