Question

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)`?

Answer 1

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.