Explain the whole process to balance the following eqution in detail :-
Pb (NO₃)₂ ----- PbO + NO₂ + O₂

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Solution

Reaction
Pb(NO₃)_{2 $\to$} PbO + NO₂ + O₂
is not balanced since atoms on both side are not equal.

Generally element other than oxygen and hydrogen are balanced first. Then it will be easier for you to balance the equation.

In this equation, Pb is equal on both side. so no need to balance it.
Then check for N. Left hand side has 2 N while there is only 1 N on right hand side. Thus multiply NO₂ by 2. This will balance N.
So the reaction will be :
Pb(NO₃)₂ $\to$ PbO + 2NO₂ + O₂

Now Check for O. There are 6 O on left hand side while 7 on right hand side.
thus we can multiply O₂ by1/2 to balance it.
Therefore the balanced reaction will be:

Pb(NO₃)₂ $\to$ PbO + 2NO₂ +1/2O₂

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Similar questions

Q. Balance the following equation.

P b S + O_{2} ⟶ P b O + S O_{2}

Q. Balance the following equations:

M n O_{2} + H C l \to M n C l_{2} + C l_{2} + H_{2} O

N H_{4} C l + C a (O H)_{2} \to N H_{3} + C a C l_{2} + H_{2} O

B a C l_{2} + A l_{2} (S O_{4})_{3} \to B a S O_{4} + A l C l_{3}

N a A l O_{2} + H_{2} O + C O_{2} \to A l H_{3} + N a_{2} C O_{3}

N H_{3} + O_{2} \to N O + H_{2} O

Z n + H N O_{3} \to Z n (N O_{3})_{2} + N O_{2} + H_{2} O

H_{2} S + O_{2} \to H_{2} O + S O_{2}

P b O + C \to P b + C O_{2}

B a C l_{2} + H_{2} S O_{4} \to B a S O_{4} + H C l

C H_{4} + O_{2} \to C O_{2} + H_{2} O

Balance the following equation by short-cut method and write the coefficient for $O_{2}$
$C_{5} H_{11} N H_{2} + O_{2} \to C O_{2} + H_{2} O + N O_{2}$ ___

Which of the following set of equation represent correct mode of obtaining

P b

from

P b S

by self-reduction process?

(A)

P b S A i r ⟶ Δ P b O + {S O}_{2}

(B)

P b S A i r ⟶ Δ P b O + {S O}

Q. Explain in detail, the steps to balance an equation?

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Explain the whole process to balance the following eqution in detail :-Pb (NO3)2 ----- PbO + NO2 + O2

Explain the whole process to balance the following eqution in detail :-
Pb (NO₃)₂ ----- PbO + NO₂ + O₂