Mole Concept Class 9th, 10th and 11th in Chemistry: Mole and its needs-Definitions, Practice problems

Key Terms You Should Know about mole concept

Welcome, students! If you are in Class 9 to 12, you know that Chemistry can sometimes feel like a puzzle. One of the biggest pieces of that puzzle is the mole concept. Whether you are preparing for your school exams or competitive tests like NEET and JEE, understanding this topic is your first step toward mastering stoichiometry.

To understand the mole concept, let's think about everyday items. If you go to a shop and ask for 12 bananas, you can simply say you want one dozen. If you want 144 pens, you call it one gross. In Chemistry, we deal with atoms and molecules which are so tiny that we cannot count them individually. Instead of dozens, chemists use a unit called a mole. So, what is mole concept exactly? It is a method used to quantify the amount of a substance by linking the microscopic world of atoms to the macroscopic world of grams and litres

These terms are frequently used in the mole concept syllabus:
1. Atomic Mass Unit (amu)
Text shows atomic mass unit definition: one amu equals one-twelfth mass of carbon-12 atom, approximately 1.67 × 10⁻²⁴ grams.

2. Relative Atomic Weight
A unitless number that compares the mass of an atom to Carbon-12.
Example:

3. Gram Atomic Mass
Mass of one mole of atoms expressed in grams.
Example:

4. Gram Molecular Mass
Mass of one mole of molecules.
Example:

Essential Mole Concept Formulas

These formulas are the backbone of mole concept numericals.

1. Number of Moles from Mass

Formula shows number of moles equals given mass in grams divided by molar mass, expressed in grams per mole.

2. Number of Moles from Particles

Formula explains number of moles equals total number of particles divided by Avogadro’s number, 6.022 × 10²³.

3. Number of Moles of a Gas at STP

Text explains one mole of gas occupies 22.4 litres at STP, with formula to calculate moles from volume.

4. Actual Mass of an Atom

If you want a quick one-shot overview of the mole concept, you can also check out this video :

Have you seen a Rs. 100 note? Probably yes. How about Rs. 1000? Probably yes. Most of us have seen the common denominations of Indian currency ranging from Rs 10 to Rs 2000. All of these denominations help in the transaction of money.

Similarly, while dealing with chemical reactions, one has to take the help of numerical denominations to specify quantities of matter getting consumed or produced. Atoms being such a small unit, it's much harder to deal with a number of atoms as a unit of measurement. In order to overcome this problem, Italian scientist Amedeo Avogadro is credited with coming up with the concept of “mole” to identify the number of particles present.

He was the first to realize that the volume of a gas (strictly, of an ideal gas) is proportional to the number of atoms or molecules. (We will study Avagadro’s Law in States of Matter).

To put it into context, what is the value of one mole? Let me give you some (mind-blowing) observations!!! Are you ready?

If you had exactly one mole of sheets of paper, you could make one million equal stacks from sea level on the earth that would pass the sun.
If you had a mole of pennies, you could give out enough money to everyone in the world so that they could spend a million dollars every hour, day and night, for the rest of their lives.
If you wanted to use trial and error to find the combination for an e-mail password, if it contained exactly six alphanumeric characters, it would take you up to 636 different tries, which is approximately 1028, which is over 17,000 moles.

So the natural question would be, “Why should we study mole?”

The mole concept is a convenient method of expressing the amount of a substance. Any measurement can be broken down into two parts – the numerical magnitude and the magnitude’s units. For example, when a ball’s mass is measured to be 2 kilograms, the magnitude is ‘2’ and the unit is ‘kilogram’. When dealing with particles at an atomic (or molecular) level, even one gram of a pure element is known to contain a huge number of atoms. This is where the mole concept is widely used. It primarily focuses on the unit known as a ‘mole’, which is a count of a very large number of particles.

Table of contents

Mole
Mathematical forms of mole
Standard temperature and pressure (STP)
Normal temperature and pressure (NTP)
Practice problems
Frequently asked questions-FAQs

Mole

We know one Dozen=12 entities

Entities can be a pen, pencil, etc, but entities can’t be atoms, ions, molecules, etc)

We know one $M o l e = 6.022 \times 10^{23} e n t i t i e s$

$6.022 \times 10^{23}$ number is known as Avogadro’s number and is represented by NA.

$6.022 \times 10^{23}$ = 1 NA

We can say,

1 mole of H+ion = Collection of $6.022 \times 10^{23} H^{+} i o n$

1 mole of H2 molecules = Collection of $6.022 \times 10^{23} H_{2} m o l e c u l e s$

1 mole of H atoms = Collection of $6.022 \times 10^{23} H a t o m s$

The quantity “mole” can be utilised for either a homogenous or heterogenous mixture. The concept of mole can be utilised to solute or solvent depending upon one’s requirement.

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A mole is defined as the amount of substance comprising the same number of fundamental entities as the number of atoms present in a pure sample of carbon weighing exactly 12 g or A mole is defined as the amount of a substance that contains exactly 6.0221023 elementary entities of the given substance.

Why did we take Avogadro's number to be $6.022 \times 10^{23}$

We know, the mass of one proton = $1.66 \times 10^{- 24} g$

$\Rightarrow \frac{1}{1.66 \times 10^{- 24}} \approx 6.022 \times 10^{23}$

1 amu= $1.66 \times 10^{- 24} g$

Also remember: 1 amuNA1

Mathematical forms of mole

Mole-to-number relation

1 $M o l e = 6.022 \times 10^{23} e n t i t i e s$

We know, number of dozens = $\frac{n u m b e r o f e n t i t i e s}{12}$

Similarly, the number of moles = $\frac{n u m b e r o f e n t i t i e s}{6.022 \times 10^{23}}$

Mole - weight relation

Number of moles = $\frac{w e i g h t o f s u b s t a n c e (g)}{M o l a r m a s s}$

The mass of 6.0221023 particles of any substance is termed the molar mass of the substance.

Mole-volume relationship

Number of moles = volume of gas (L)Molar volume (L) (at same T & P)

At STP,

The number of moles = $\frac{v o l u m e o f g a s (L)}{22.7 L} (a t S T P)$

Standard temperature and pressure (STP)

Temperature = $0^{0} C = 273 K$

Pressure = 1 atm

It was experimentally observed that, at STP conditions, one mole of an ideal gas occupies 22.7 L volume.

Normal temperature and pressure (NTP)

Temperature = $20^{0} C = 293 K$

Pressure = 1 atm

It was experimentally observed that, at NTP conditions, one mole of an ideal gas occupies 24.0 L volume.

Video Link:

Practice problems

Q1. Find the total number of Helium (He) atoms present in 2.5 moles of Helium.

(NA refers to Avagadro’s number)

a. NA
b. 2NA
c. 2.5NA
d. 3NA

Answer: (C)

Solution: we know 1 mole = $6.022 \times 10^{23}$ entities

The total number of He atoms = 2.5 $6.022 \times 10^{23}$ = 2.5NA

Q2. Find the total mass in grams of 3.5 moles of copper.(Molar mass of Cu = 63.5 g mol-1)

a. 222.25 g
b. 250.45 g
c. 234.34 g
d. 342.76 g

Answer: (A)

Solution: number of moles = $\frac{w e i g h t o f s u b s t a n c e (g)}{M o l a r m a s s}$

$W e i g h t o f s u b s t a n c e = n u m b e r o f m o l e s \times M o l a r m a s s$

Weight of substance = (3.5 63.5) g = 222.25 g

Q 3. Find the volume at STP for 64 g SO2 gas.

a. 44.8 L
b. 22.4 L
c. 11.2 L
d. 5.6 L

Answer: (B)

Solution: number of moles of ${S O}_{2} = \frac{w e i g h t o f s u b s t a n c e (g)}{M o l a r m a s s} = \frac{64}{64} = 1 m o l$

number of moles = $\frac{v o l u m e o f g a s (L)}{22.4 L} (a t N T P)$

Volume of SO2 gas = 1 mol 22.4 L=22.4 L

Q4. Find the charge of 54 mg of Al3+ ions.

a. 144.56 C
b. 72.30 C
c. 96.35 C
d. 192.7 C

Answer: (D)

Solution: number of moles of $A l^{3 +} = \frac{w e i g h t o f s u b s t a n c e (g)}{M o l a r m a s s} = \frac{0.054}{27} = 2 \times 10^{- 3} m o l$

The total number of Al3+ ions = $2 \times 10^{- 3} \times 6.022 \times 10^{23} = 12.044 \times 10^{20}$

One ion Al3+ contains three positive charges.

We know the magnitude of charge of one proton equals the magnitude of charge of one electron.

Charge of one proton = $1.6 \times 10^{- 19} C$

Total charge on Al3+= $1.6 \times 10^{- 19} C \times 12.044 \times 10^{20} = 192.7 C$

Frequently asked questions (FAQs)

Q. What is the meaning of gram-atom and gram-molecule?
Answer: According to modern practice, gram-atom and gram-molecule are known as moles.

E.g- 1 gram-atom Na+ = 1 mol of Na+

1 gram-molecule H2O = 1 mol of H2O

Q. When is Mole Day celebrated?
Answer: $1 N_{A} = 6.022 \times 10^{23}$

Mole Day is celebrated on September 23, from 6 AM to 6 PM.

Q. Why do we use mole fraction?
Answer: The mole fraction defines the number of single component molecules (or moles) divided by the total number of molecules (or moles) in the mixture. When two reactive components are mixed together, the mole fraction is useful, as the ratio of the two components is understood if the mole fraction of each is known.

Q. Is mole fraction equal to partial pressure?
Answer: In a mixture, the partial pressure of each gas is proportional to its mole fraction. The pressure exerted by each gas (its partial pressure) in the gas mixture is independent of the pressure exerted by all other gases present in the gas mixture.

Q. What is the importance of the mole concept?
Answer: All chemistry is pervaded by the mole definition. Since most quantitative chemical calculations are focused on the mole, for the study of chemistry, an understanding of the mole is important. Knowledge of how the mole applies to mass, the number of entities, etc.