Question

a)Nitrous oxide gas (systematic name: dinitrogen monoxide) is used by some dental practitioners as an anesthetic. Nitrous oxide (and water vapor as byproduct) can be produced in small quantities in the laboratory by careful heating of ammonium nitrate. Write the unbalanced chemical equation for this reaction. (Omit states-of-matter from your answer.)

Answer 1

Explanation:

Nitrous oxide or dinitrogen monoxide can be simple be prepared by the decomposition of ammonium nitrate in the following way -

The reaction is as follows -

NH₄NO₃  ---------------->  N₂O + H₂O

This is the unbalanced reaction as was asked in the question , without mentioning the states of matter .

The reaction is carried out in an anhydrous condition ,since , ammonium nitrate can explode on heating .

Answer 2

Answer: The unbalanced chemical equation is written below.

Explanation:

An unbalanced chemical equation is defined as the equation in which total number of individual atoms on the reactant side is not equal to the total number of individual atoms on the product side. These equations does not follow law of conservation of mass.

The chemical equation for the heating of ammonium nitrate follows:

$NH_4NO_3\rightarrow N_2O+H_2O$

The products formed are dinitrogen oxide and water vapor

Hence, the unbalanced chemical equation is written above.