Mole Concept & Principle of Atomic Conservation (POAC)

Stoichiometry

Introduction

Stoichiometry deals with the calculation of the quantities of various reactants and products involved in a chemical reaction. The numerals used to balance a chemical equation are known as stoichiometric coefficients. These numerals are essential for solving problems based on chemical equation, hence called stoichiometric calculation.

In stoichiometric calculations, the mole relationship between different reactants and products are required as from them the mass-mass, mass-volume and volume-volume relationship between different reactants and products can be obtained.

Stoichiometric calculations can be carried out by two methods; Gravimetric Analysis and Volumetric Analysis. In the first method the amount of chemical species is determined by measurement of mass, whereas, in second method it is determined by measurement of volume.
Stoichiometric calculation can be carried in terms of two important concept:

(i) Mole Concept;

(ii) Equivalent concept

Mole Concept

A mole (symbol mol) is defined as the amount of substance that contains as many atoms, molecules, ions electrons or any other elementary entities as there are carbon atoms in exactly 12 gm of 12C.

The number of atoms in 12 gm of 12C is called Avogadro’s number (N0)

N0 = 6.023 × 1023

One atomic mass unit (amu) $\large = \frac{1}{N_o}= \frac{1}{6.023 \times 10^{23}}$

1 a.m.u  = 1.66 × 10–24 gm = 1.66 × 10–27 kg

The number of moles of a substance can be calculated by various means depending on data available, as follows.

$\large (a) Number\; of \;moles\; of\; molecules = \frac{Weight\; in \; gram}{Molecular \; mass}$

$\large (b) Number\; of \;moles\; of\; atoms = \frac{Weight\; in \; gram}{Atomic \; mass}$

$\large (c) Number\; of \;moles\; of\; gases = \frac{Volume\; at \; S T P}{Standard \; molar \; volume}$

(Standard molar volume at STP = 22.4 lit)

$\large (d) Number\; of \;moles\; of\; Particles = \frac{Number \; of \; particles}{Avogadro \; number }$

(e) Number of moles of Solute = Molarity × Volume of Solution in litre

$\large Number \; of \;moles \;of \;Solute= \frac{Molarity \times Volume\; in \; ml}{1000}$

(f) for a compound Ax By ,

y moles of A = x  moles of B

(g) Mole fraction = fraction of the substance in the mixture expressed in terms of mol is called its mol fraction (X) .  e.g. for a mixture of substance A & B

$\large X_A = \frac{n_A}{n_A + n_B}$

$\large X_B = \frac{n_B}{n_A + n_B}$

XA + XB = 1

⇒ XA= (1 − XB)

Principle of Atomic Conservation (POAC)

In chemical reaction atoms are conserved , so moles of atoms shall also be conserved. This is known as principle of atomic conservation.  This principle is helpful in solving problems of nearly all stoichiometric calculations e.g.

KClO3(s) → KCl(s) + O2(g)

Applying POAC for K atoms

Moles of K atoms in KClO3 = Moles of K atoms in KCl

Since one mole of KClO3 contains 1 mol of K atom. Similarly 1 mol of KCl contains one mole of K atoms.

$\large 1 \times n_{KClO_3} = 1 \times n_{KCl}$

$\large 1 \times \frac{W_{KClO_3}}{M_{KClO_3}} = 1 \times \frac{W_{KCl}}{M_{KCl}}$

(Mass-mass relationship)

Applying POAC for ‘ O ‘ atoms

Moles of O atom in KClO3 = Moles of O atom in O2

3 × nKClO3 = 2 × nO2

$\large 3 \times \frac{W_{KClO_3}}{M_{KClO_3}} = 2 \times \frac{Volume \;of\; O_2\; at \;STP}{Standard \; Molar \;Volume}$

(Mass volume relationship of reactant and product)

In this way applying POAC we can break the chemical equation into a number arithmetic equations without balancing the chemical equation.

Moreover number of reactions and their sequence from reactants to products are not required. It is important to note that POAC can be applied for the atoms which remain conserved in chemical reaction.

Concept of Limiting Reagent

In reactions involving more than one reactant, one has to identify first, of all the reactant, which is completely consumed (limiting reagent), one can identify the limiting reagent as follow

N2 + 3H2 → 2NH3

Initial mole    5      12      —

If N2 is the limiting reactant moles of NH3 produced = 10

If H2 is the limiting reactant moles of NHproduced

= (3/2) ×12 = 18

The reactant producing the least number of mole of the product is the limiting reactant, hence H2 is the limiting reactant.

The limiting reactant can also be ascertained by knowing the initial number of equivalents or milli equivalents of each reactant.

The reactant with least number of equivalents or milli equivalent is the limiting reactant.

The equivalent methods to identify the limiting reactant used not require balancing of chemical equation.

Also Read :

→ Gravimetric Analysis
→Oxidation and Reduction
→ Balancing Redox Equations
→ Volumetric Analysis
→ Law of Equivalence
→‘ n ‘ Factor
→ Applications of the Law of Equivalence : Simple titration , Back titration
→ Double titration
→ Volume of Strength of H2O2

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