Question

In the decomposition of lead $(II)$ nitrate to give lead $(II)$ oxide, nitrogen dioxide and oxygen gas, the coefficient of nitrogen dioxide in the balanced equation is
$(1)$ $1$,
(2)$$$$2,
$(3)$ $3$,
$(4)$ $4$.

Answer 1

A chemical equation is the symbolic representation of a chemical reaction. In a balanced chemical equation, the number of atoms of each element are the same on both sides of the reaction. Decomposition reactions are defined as those reactions in which a single reactant is degraded into two or more products.

Complete answer:
The chemical equation for the decomposition of lead $(II)$nitrate to give lead $(II)$oxide, nitrogen dioxide and oxygen is given as follows:
$Pb{{(N{{O}_{3}})}_{2}}\to PbO+N{{O}_{2}}+{{O}_{2}}$
In order to get the balance chemical equation, we have to multiply $PbO$and $Pb{{(N{{O}_{3}})}_{2}}$ by the factor of $2$and $N{{O}_{2}}$by the factor of $4$. Incorporating these factors into account, the above equation becomes
$2Pb{{(N{{O}_{3}})}_{2}}\to 2PbO+4N{{O}_{2}}+{{O}_{2}}$
From the above balanced chemical equation, we conclude that the coefficient of nitrogen dioxide in the decomposition of lead $(II)$nitrate is 4.

Additional information: In this decomposition reaction of lead $(II)$nitrate, we get a yellow colour solution with simultaneous evolution of brown colour gas. Yellow colour is due to the formation of $PbO$while brown colour gas occurs due to the formation of $N{{O}_{2}}$ gas

Note:
It is important to note that the coefficient of nitrogen dioxide in the balanced decomposition equation is 4. Decomposition reactions are those in which a single reactant is degraded into two or more products. In the decomposition reaction of lead $(II)$ nitrate, a yellow colour solution with simultaneous evolution of brown colour gas occurs.