We know that, in a chemical reaction, the atoms of each element remain conserved. If atoms are conserved, moles of atoms will also be conserved. This is known as the principle of atom conservation.
Total number of moles of an atoms of an element on reactant side = Total number of moles of atoms of an on product side.
Illustration
of POAC: Take a chemical
reaction as example.
(A)
According to the principle of atom conservation (POAC) for K atoms:
Total moles of K atoms in
reactant = total mole of K atoms in products
or
Moles
of K atoms in KClO3 = moles of K atoms in KCl.
Now, since 1 molecule of KClO3 contains 1 atom of K, 1mole of KClO3 contains 1 mole of K similarly, 1mole of KCl contains 1mole of K.
Thus, mole of K atoms in
KClO3 = 1 × moles of KClO3
And mole of
K atoms in KCl = 1 × moles of KCl
Hence
1 × moles of KClO3 =
1 × moles of KCl
(B) Similarly applying the principle of atom conservation for O atoms:
Mole of O in KClO3 = 3 ×moles of KClO3
And
moles of O in O2 = 2 × moles of O2
3
× moles of KClO3 = 2 × moles of O2
Illustrative
example (1): Write the POAC equations for all the atoms in the following reaction.
Illustrative solution:
Applying
POAC on (P) atoms:
P à H3PO4
Numbers of
moles of (P) atoms in P4 = Numbers of moles of (P) atoms in H3PO4
4x nP4= 1x nH3PO4
Applying
POAC on (H) atoms:
1x nHNO3
= 3 x nH3PO4 + 2 x nH2O
Applying
POAC on (N) atoms:
1 x nHNO3
= 1 x nNO2
Applying
POAC on (O) atoms:
3 x nHNO3
= 4 x nH3PO4 +2 x nNO2 + 1nH2O
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