Chapter 9.2, Problem 16PP

Interpretation Introduction

Interpretation:

The given chemical equation for the reaction of nitrogen dioxide gas with oxygen to produce dinitrogen pentoxide gas needs to be written and classified.

Concept introduction:

In a chemical reaction, the reactants are written on the left side of the equation and the product is written on the right side. The product and the reactants contain an arrow between them showing the proceeding of the reaction from the reactants to the products.

A chemical equation is balanced by balancing the number of moles of each element on the reactants and on the products.

Answer to Problem 16PP

The chemical equation for the reaction is as follows:

$4{\text{NO}}_{\text{2}}\left(\text{g}\right)\text{+}{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{2N}}_2{\text{O}}_5\left(\text{g}\right)$

This reaction is a synthesis as well as combustion type reaction.

Explanation of Solution

The chemical equation for the reaction is,

$4{\text{NO}}_{\text{2}}\left(\text{g}\right)\text{+}{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{2N}}_2{\text{O}}_5\left(\text{g}\right)$

It is a combustion reaction because, in this reaction nitrogen dioxide combines with oxygen to form ${\text{N}}_2{\text{O}}_5$.

It is also a synthesis reaction because, in this reaction, two reactants combined to give one larger product.

Therefore, this reaction is a synthesis as well as combustion type reaction.

Conclusion

The chemical equation for the given reaction is,

$4{\text{NO}}_{\text{2}}\left(\text{g}\right)\text{+}{\text{O}}_{\text{2}}\left(\text{g}\right)\to {\text{2N}}_2{\text{O}}_5\left(\text{g}\right)$

This reaction can be classified as both synthesis as well as combustion type reaction.