Study S3 Chemistry The Mole - Geniebook

# The Mole

In this article we are going to learn about the concept of the Mole. We will be covering the following learning outcomes:

• Define relative atomic mass
• Define relative molecular mass & relative formula mass
• Calculate relative molecular mass or relative formula mass of a substance
• Define the term mole
• Convert number of particles into number of moles of particles and vice versa

## Relative Atomic Mass

By definition, the relative atomic mass of an atom (Ar) is the average mass of one atom of that element compared to $$1\over 12$$ of the mass of one carbon-12 atom.

Question:

Why do we use the mass of a carbon-12 and not the actual mass of an atom of that element?

To answer this, let us take a look at the next section.

## Atomic Mass Unit

All the particles in an atom are very light, so light that it is not convenient and practical to express their masses in grams or kilograms in calculations.

It is easier to measure their masses against a standard unit, called the atomic mass unit (amu).

1 amu = 1.67 × 10-27 kg

1 amu is $$1\over 12$$ the mass of a carbon-12 atom. The mass of this carbon was determined accurately by experiment using a modern instrument called mass spectrometer.

$$​ {Relative \; Aatomic \; Mass} = \frac {average \; mass \; of \; one \; atom \; of \; the element} {{\frac {1}{12}} \times \; mass \; of \; an \; atom \; of \; carbon-12} ​$$

For example, one atom of oxygen was found to be 16 times heavier than $$1\over 12$$ of an atom of carbon-12. Thus, oxygen has a relative atomic mass of 16.

As the relative atomic mass is a ratio, it does not have a unit.

## Why Is The ArOf Chlorine A Decimal

Some elements, such as chlorine , occur as mixtures of isotopes. For these elements, their atoms will have different relative masses.

For the ease of calculation, the relative atomic mass will be calculated based on the relative percentage abundance of the isotopes.

Recall that isotopes are atoms of the same element with the same number of protons and electrons, but different numbers of neutrons.

There are two different isotopes of chlorine: 35Cl and  37Cl

Since we cannot account for both of these isotopes individually, hence we take the average of both of these atomic masses.

Worked Example:

Chlorine has two isotopes, 35Cl and  37Cl, with respective abundance of 75% and 25%. Determine the relative atomic mass of chlorine.

Solution:

Relative atomic mass of chlorine = Sum of [relative abundance × isotopic mass]

= $$\frac {75}{100}\; ×\; 35\;+\;\frac {25}{100}\; ×\; 37$$

= 35.5

Question 1:

Chemists discover that the neon element has three isotopes. They are neon-20, neon-21 and neon-22, with respective abundances of 90.92%, 0.26% and 8.82%. Determine the Ar of neon. (* Give your answer correct to 3 s.f.)

1. 21.1
2. 20.2
3. 20.9
4. 21.9

Solution:

(B) 20.2

Explanation:

Ar = Sum of [relative abundance isotopic mass]

= $$\frac {90.92}{100}\; ×\; 20\;+\;\frac {0.26}{100}\; ×\; 21\;+\;\frac {8.82}{100}\; ×\; 22$$

= 20.179

= 20.2 (to 3.s.f.)

Question 2:

The diagram shows the mass spectrum of an unknown sample. Use the data to calculate the relative atomic mass of the sample.

1. 65.00
2. 65.25
3. 65.50
4. 65.66

Solution:

(C) 65.50

Explanation:

A= Sum of [relative abundance isotopic mass]

= $$\frac {40} {100}\; ×\; 64 \;+\; \frac {30} {100}\; ×\; 66 \;+\; \frac {30} {100}\; ×\; 67$$

= 65.50

Question 3:

Potassium has 2 major isotopes. They are 39K and 41K. If the relative atomic mass of naturally occurring potassium is 39.14, What are the relative abundances of 39K and 41K?

1. 7% of  39K      &    93% of  41K
2. 25% of  39K    &    75% of  41K
3. 75% of  39K    &    25% of  41K
4. 93% of  39K & 7% of  41K

Solution:

(D) 93% of  39K & 7% of  41K

Explanation:

We can perform a calculation for each of the options. So when the relative abundance of 39K and 41K are 93% and 7% respectively, the relative atomic mass of potassium is:

Ar = Sum of [relative abundance isotopic mass]

= $$\frac {93} {100}\; ×\; 39 \;+\; \frac {7} {100}\; ×\; 41$$

= 39.14

## Relative Molecular Mass

By definition, the relative molecular mass of a molecular substance (Mr) is the average mass of one molecule of that element or compound compared to $$1\over 12$$ of the mass of one carbon-12 atom.

To compute the relative molecular mass of a substance, we can simply add the relative atomic masses of all the atoms in its chemical formula.

Worked Example:

Calculate the relative molecular mass of sulfuric acid, H2SO4

Solution:

Relative molecular mass of sulfuric acid, H2SO4

= (2 × Ar  of H atom ) + (1 × Aof S atom) + (4 × Aof O atom)

=  (2 × 1 ) + (1 × 32) + (4  × 16)

= 98

## Relative Formula Mass

By definition, the relative formula mass of an ionic compound (Mr) is the average mass of one unit of that ionic compound compared to $$1\over 12$$ of the mass of one carbon-12 atom.

To compute the relative formula mass of a substance, we can simply add the relative atomic masses of all the atoms in its chemical formula.

Worked Example:

Calculate the relative formula mass of magnesium chloride, MgCl2

Solution:

Relative formula mass of magnesium chloride, MgCl2

= (1 × Ar of Mg atom ) + (2 × Ar of Cl atom)

=  (1  ×  24) + (2  ×  35.5)

= 95

Question 4:

Calculate the relative molecular mass of C3H7COOH.

1. 72
2. 76
3. 87
4. 88

Solution:

(D) 88

Explanation:

Relative molecular mass of C3H7COOH

= (4 × Aof C atom ) + (8 × Aof H atom) + (2 × Aof O atom)

= (4 × 12) + (8 × 1) + (2  × 16)

= 88

Question 5:

Calculate the relative formula mass of Fe(NO3)3

1. 166
2. 194
3. 214
4. 242

Solution:

(D) 242

Explanation:

Looking at the chemical formula of iron(III) nitrate, Fe(NO3)3, there are 1 Fe atom, 3 N atoms and 9 O atoms.

Relative formula mass of Fe(NO3)3

= (1 × Aof Fe atom ) + (3 × Aof N atom) + (9 × Aof O atom)

=(1 × 56 ) + (3 × 14) + (9 × 16)

= 242

Question 6:

Calculate the relative formula mass of CuSO4.7H2O.

1. 190
2. 286
3. 2256
4. 20160

Solution:

(B) 286

Explanation:

Looking at the chemical formula of hydrated copper(II) sulfate, CuSO4.7H2O, there are 1 Cu atom, 1 S atom, 4 O atoms and 7 molecules of H2O.

Relative formula mass of CuSO4.7H2O

= (1 × Aof Cu atom ) + (1 × Ar   of S atom) + (4 × Aof O atom) + (7 × Mof H2O)

=(1 × 64 ) + (1 × 32) + (4 × 16) + [7 × (2 × 1 + 16)]

= 286

## Mole

Imagine you are at the supermarket. Many items can be quantified by a unit.

For example:

1 kg of rice

1 litre of oil

1 pair of socks

1 dozen of eggs

However, how do you quantify particles such as atoms which are so small and numerous?

We will use the unit called mole.

One mole of a substance contains the same number of particles as the number of atoms in 12 g of carbon-12.

One mole of particles = 6 × 1023 particles

For Example:

1 mole of Cu atoms = 6 × 1023 Cu atoms

1 mole of H2O molecules = 6 × 1023 H2O molecules

Converting between the number of moles and number of particles, we can apply the following formula:

 $$Number \; Of \; Moles = {\frac {Number \; Of \; Particles} {6 \; × \; 10^{23}}}$$

Worked Example:

One molecule of H2O contains 2 H atoms and 1 O atom. Hence, in one mole of H2O molecules, determine the number of H atoms and O atoms.

Solution:

One mole of H2O molecules = 6 × 1023 H2O molecules

If each molecule of H2O contains 2 H atoms, then number of H atoms = 6 × 1023 × 2

= 1.2 × 1024

If each molecule of H2O contains 1 O atom, then number of O atoms  = 6 × 1023 × 1

= 6 × 1023

Question 7:

Calculate the number of sulfur atoms in 0.25 mole of sulfur.

1. 6 × 1023
2. 3 × 1023
3. 1.5 × 1023
4. 0.25 × 1023

## Explanation:

Number of sulfur atoms = ( Number of moles of sulfur ) × 6 × 1023

## = 1.5 × 1023

Question 8:

Calculate the number of chlorine atoms in 0.04 mole of chlorine gas.

1. 0.24 × 1023
2. 0.48 × 1023
3. 2.4 × 1023
4. 0.48 × 1024

## Explanation:

Number of chlorine gas molecules  = (Number of moles of chlorine molecules) × 6 × 1023

## = 0.24 × 1023

Each chlorine gas molecule contains 2 chlorine atoms.

Number of chlorine atoms = 0.24 × 1023 × 2

= 0.48 × 1023

## Conclusion

In this chapter we have learnt about the concepts of relative atomic mass, relative molecular mass as well as relative formula mass. We also learnt how to calculate the relative molecular mass or relative formula mass by adding the relative atomic masses of all the atoms in the chemical formula of the substance. Lastly, we also learnt about mole as a unit of measurement and Avogadro’s constant, which allows us to convert between the number of moles and the number of particles.

Practice the multiple questions and examples given in the article to understand the concepts better. Keep Learning! Keep Improving!

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Separation and Purification Atomic Structure
Measurement and Experimental Techniques Ionic Bonding
Covalent Bonding Writing Chemical Equations
Oxidation and Reduction Acids And Bases
The Mole Salts
Atmosphere and Environment Periodic Table
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Writing Chemical Equations
Oxidation and Reduction
Acids And Bases
The Mole
Salts
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Periodic Table
Chemical Calculations
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