# 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)?

Aug 3, 2017

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

#### Explanation:

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

You have got........

$2 {N}_{2} \left(g\right) + 3 {O}_{2} \left(g\right) \rightarrow 2 {N}_{2} {O}_{3} \left(g\right)$

${N}_{2} {O}_{3}$ is formally a mixed valence compound of $\stackrel{+ I I}{N}$ and $\stackrel{+ I V}{N}$, i.e the average oxidation state is $N \left(+ I I I\right)$. We would assume a pressure drop in the reaction......why? I also have an idea that ${N}_{2} {O}_{3}$ is relatively high boiling.