Question

Consider the given chemical reaction

$2Pb(N{O}_3{)}_2\to X_{\left(s\right)}+Y_{\left(g\right)}+Z_{\left(g\right)}$

The ratio of atoms of constituent elements (by number), present in the brown coloured gas produced in the reaction is

• A.
  3 : 2
• B.
  3 : 1
• C.
  2 : 3
• D.
  1 : 2

Answer 1

The correct option is D

1 : 2
On heating, lead nitrate decomposes to produce lead oxide, brown coloured nitrogen dioxide gas, and oxygen gas. The chemical equation involved in the reaction is:

$2Pb(N{O}_3{)}_2\to 2Pb{O}_{\left(s\right)}+4N{O}_{2\left(g\right)}+O\left(2g\right)$


The ratio of atoms of N and O present in the brown coloured NO2 gas is 1 : 2.

Hence, the correct answer is option (d).