# Mole and Avogadro’s Number | Important Questions

## What is Mole ?

Mole(n) is defined as the amount of substance that contains 6.022 x 1023 particles ( atoms ,molecules or ion)

Or:

Mole can also be defined as ” the atomic mass , molecular mass or formula mass expressed in grams is equal to i mole of a substance”.

(1)   A mole is a  counting unit which contain 6.022 x 1023 particles

As!!

12 things = dozen

2 things = Pair

144 things = gross

1 Kg    =   1000 g

similarly:

1 mole =  6.022 x 1023 particles

## “One mole of a substance contains Avogadro’s number (6.02 x 1023) of things or particles”.

e.g. (i)  6.02 x 1023 atoms of Hydrogen are called one mole or one gram-atom of Hydrogen.

e.g. (ii) 6.02 x 1023 molecules of Hydrogen are called one mole or one gram-molecule of Hydrogen.

e.g. (iii) 6.02 x 1023 electrons are called one mole of electrons.

# Avogadro’s number (NA) :

### Avogadro’s number is defined as “the number of particles that are present in one mole of a substance “.

Avogadro’s number (NA) value is 6.022 x 1023 .

It’s unit is mol-1

## How do you calculate moles in chemistry?

Formulae to calculate moles of a substance are as follow:

## Number of moles = Number of particles /   6.02 x 1023

(2)        “Atomic mass in grams is also called a mole or gram atom.”

Number of moles = Mass In grams / Atomic mass in gram or Molar mass

(3)        “Molecular mass in grams is also called a mole or gram molecule.”

Number of moles =      Mass In grams / Molecular mass in gram or Molar mass

(4)        Volume of one mole of a gas at STP is 22.4 dm3 or litre.

No of moles = Volume (in dm3) at STP  / 22.4

(5)        Volume of one mole of a gas at RTP is 24 dm3 or litre.

Volume (in dm3) at RTP

No of moles = Volume (in dm3) at RTP   / 24

Standard temperature = 0oC or 32oF or 273K               and      Standard pressure = 1atm or 760 mmHg(Torr) or 1.01×105 N/m2 (Pa) or 14.7 PSI(Ib/in2)

Room temperature = 25oC or 77oF or 298K                 and      Room pressure = 1atm or 760 mmHg(Torr) or 1.01×105 N/m2 (Pa) or 14.7 PSI(Ib/in2)

(6)        Moles of solute in the solution = MV

where M = molarity of solution

V = volume of solution indm3

• A molecular formula shows Number of atoms of different elements in a molecule of a compound, as well as it shows number of moles of atoms of elements in a mole of compound.

e.g. One molecule of Ethyl alcohol (C2H5OH) contains two atoms of Carbon, six atoms of Hydrogen and one atom of Oxygen.

OR

One mole of Ethyl alcohol (C2H5OH) contains two moles of Carbon atoms, six moles of Hydrogen atoms and one mole of Oxygen atom.

Related Important Questions !!

Q1.What is the mass of one mole Carbon atom?

Ans. The mass of one mole of carbon atom is 12g.

Q2.How many moles are there in 60g of NaCl  ?

Solution:

Given:

Mass of NaCl= 60g

Moles of NaCl = ?

SOLUTION:

Molar mass of NaCl= 23+35.5= 58.5g/mol

FORMULA:

No of moles= mass / molar mass

No of moles= 60 / 58.5

No of moles(n) =1.02 mol

Q3.What is the mass of 0.5 mole of CaCO3 ?

SOLUTION:

Moles of CaCO3 = 0.5 mol

Mass of CaCO3 =?

SOLUTION:

Molar mass of CaCO3 = 100 g/ mol

FORMULA:

No of moles= mass / molar mass

Mass of CaCO3 = moles. X   molar mass

Mass of CaCO3 =  0.5   X100

= 50g CaCO3

## Also Read !!!

Stoichiometry Important Terms Definitions

What is the difference between Octet Rule and Duplet Rule

Basic Atomic Structure

What is the difference between Shell , Subshell and Orbital

How ions are formed (Cation vs Anion)

Ionic Bond : Definition, Examples & Formation

Covalent Bond :Definition and Examples