# data[].attributes.attachment_link.title
H2O Is Water And H2O2 Is Hydrogen Peroxide. What Is H2O4? | Chemistry Jokes

# data[].attributes.attachment_link.description
Image uploaded by Chemistry Jokes. Find images and videos about jokes, chemistry and chemistry jokes on We Heart It - the app to get lost in what you love.

# data[].attributes.attachment_link.description
Chemistry Cat is breaking the lawz #Cat #Science

# data[].attributes.attachment_link.readable_text
The mole concept is one of the topics with which you kick-off your preparation of physical chemistry in class 11. One of the reasons for it being taught earlier is that the concept of mole will be required in almost every other topic of physical chemistry that you study later, irrespective of the complexity of that topic. Apart from its relevance in chemistry, it must be noted that mole concept is one of the easier topics of chemistry, so, make sure you do study it well and go through each and every point in this topic. To help you in your preparations, here, I have discussed the relevant points and formulae that you must know, related to the concept of mole.

Definition of mole -

To start with, you must be very clear about what exactly does a mole represent.

The mole is the unit of measurement in the International System of Units (SI) for amount of substance. 1 Mole is just a number whose value is equal to the Avagadro's number i.e. 6.022 * 10 ²³. So, when someone claims of a matter to be of 1 mole in quantity, that implies that the matter under consideration contains exactly 6.022 * 10 ²³ number of particles (atoms, molecules, ions, electrons or any other elementary entities). This is very similar to the unit 'dozen', which is a common analogy used to explain the concept of mole, a dozen is always equal to 12 irrespective of the object referred to.

Why was the concept of mole needed?

When dealing with particles of the size of atoms and molecules, it becomes very difficult to do the calculations as they are present in very large numbers. Even in a small sample of an element or chemical compound, generally the number of elementary particles are in the higher order of 10. So to make these calculations simpler, mole was defined. While solving problems, the numbers are expressed in terms of Avogadro number, making the solution to the problems in physical chemistry simpler.

Reference used for defining the Avogadro number:

Since a mole is used to define quantity of matter, it is necessary that we have a reference with respect to which it is being defined. A mole or Avogadro number is defined as the amount of substance that contains as many elementary entities as there are in exactly 12 gm of Carbon-12. The number of atoms in 12 gm of Carbon-12 is called Avogadro's number (N A).

Thus, 1 mole of Cu will contain as many atoms, molecules,etc as there are in 12 gm of Carbon-12, even though mass of both are different.

Applications of Mole Concept:

Though mole is defined as a number but it's not limited to that in calculations. It has various other equivalent definitions with the only difference from each other being that they define mole for different states of matter and at different conditions.

The diagram below indicates various equivalent definitions of 1 mole :

With the use of the above definitions, the mole concept can be used to do various other calculations as shown :
Formulae to calculate the no. of moles -

Number of moles of molecules = wt. in gm / molecular mass

Number of moles of atoms = Wt. in gm / atomic mass

Number of moles of gases = Volume at STP / Standard Molar Volume (Standard molar volume at STP = 22.4 lit)

Number of moles of particles e.g. atoms, molecules ions etc = No. of particles / Avogadro number

Used to express the concentration of the solution in terms of molarity, molality, mass fraction, etc.

Molarity = No. of moles of solute/Volume of solution in litres

Molality = Number of moles of solute/Weight of solvent in kg

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

(n terms of denote number of moles)
The ideal gas equation includes no. of moles as one of the parameters that decides the state of the gas.
PV=nRT -- n: no. of moles of gas in consideration.
Used to find the emperical and molecular formula, used in balancing of redox reactions and to determine the stoichiometry of the reaction.
The aforementioned points are the most relevant that you must be thorough with in the concept of mole. However, understanding the theoretical will be of no good unless you practise a good amount of numericals. So, make sure that you get enough practice in that. Apart from this, you can find detailed explanation of various other concepts related to mole, here.

Now that you are thorough with the theory behind mole concept, you might as well top it off with some practice! Check out our question bank on Mole Concept here!

All the best!

# data[].attributes.attachment_link.title
Mole Concept: The Basics of the Beginning of Chemistry!

# data[].attributes.attachment_link.description
The mole concept is one of the topics with which you kick-off your preparation of physical chemistry in class 11. One of the reasons for it being taught earlier is that the concept of mole will be required in almost every other topic of physical chemistry that you study later, irrespective of the complexity of that topic.

# data[].attributes.attachment_link.description
What do you get when you cut an avocado into 6X10^23 pieces? - - High School Memes

# data[].attributes.attachment_link.description
Anatomy and Physiology AP Biology AP Chemistry AP Environmental Science AP Physics Biology Chemistry Earth Science Educational NGSS - Next Generation Science Standards Physics Statistics & Graphing

# data[].attributes.attachment_link.title
Avogadro's Number, The Mole, Grams, Atoms, Molar Mass Calculations - Introduction

# data[].attributes.attachment_link.description
This general chemistry video tutorial focuses on avogadro's number and how it's used to convert moles to atoms. This video also shows you how to calculate the molar mass of a compound and how to convert from grams to moles. This video contains plenty of examples, notes, and practice problems that you help you complete your next worksheet assignment.

# data[].attributes.attachment_link.title
The mole and Avogadro's number | Atoms, compounds, and ions | Chemistry | Khan Academy

# data[].attributes.attachment_link.description
Don't let these burrowing varmints turn your lawn into their playpen.

# data[].attributes.body
Add Links to videos, descriptions, about the concepts

# data[].attributes.body
Add Links, Pictures Biographical Notes

# data[].attributes.body
https://www.britannica.com/biography/Amedeo-Avogadro