# What is Mole and Why do we use Moles in Chemistry

If the relative formula mass for a compound is calculated by adding together their relative atomic mass these values for all the atoms in its formula. These moles are units used to measure their substance amount.

## How do you calculate moles in chemistry?

How to find these moles in this solution is to calculate how many more molecules this solution contains. Also, to do this you need to know the volume of this solution and how many more solutes have been dissolved in this solution.

Furthermore, you also need to know the molar mass of this solute. If it refers to a very huge number that we use to measure these atoms.

Moreover, it is more equal to this number for some atoms in 12 grams for carbon-12 which is just about 6.022 × 1023 these atoms. Just like that this way, it is very much easier to measure intergalactic (Space) distance in light-years than to measure it in these inches. Also, it is much easier to calculate these atoms in a mole than in lakhs or crores.

## What is the mole and why do we use moles in chemistry

In this lesson, we will explore these chemical equations or what we can learn about them using these moles. We will learn what a mole is or how moles are used to determine the mass needed for a reaction to occur.

## 1. What Are Moles?

In their chemistry, we frequently use the word these ‘moles’ to refer to the amount of these chemicals used. If this mole is not their little animal that they are digging around in your yard, they instead refer to a set quantity for some of these atoms. If they think of it like this word ‘dozen’. When you say about two dozen these eggs, you mean that these two sets of 12 eggs.

These moles represent a very much bigger number though, 6.023 times ten to this 23rd, which is called ‘Avogadro’s number’. So instead of saying, ‘I have a dozen of these atoms’ we can say that ‘I have an Avogadro’s number of some atoms’ (in chemistry we don’t very typically say it like that, but it’s a good way to think about what a mole their means).

### 2. Moles in Chemical Equations

Right now let’s think about these dozen atoms again concerning this water reaction or some moles.

Now we see that these 2 molecules of hydrogen react with 1 molecule of oxygen to form 2 molecules of water. Now very typically we aren’t only making 1 molecule (remember, that they would be in such a very small quantity that we wouldn’t be able to see it let alone measure it out).

So let’s double it. This would mean that we are using these 4 molecules from hydrogen to react with 2 molecules for the oxygen to form some 4 molecules from the water. How about a dozen times each? There are 2 dozen hydrogen molecules or 1 dozen oxygen.

These molecules are making 2 dozen water molecules. So really, it is 24 hydrogen molecules reacting with these 12 oxygen molecules to make some 24 water molecules, but they are still instead of saying 24, 12, or 24 we can look at it as some multiples for a dozen.

### 3. Moles and the Periodic Table

There sometimes a periodic table will simply have these names or abbreviations for each other element in these blocks. But they are still these. Sometimes we will see your numbers in these blocks. Let’s look at calcium.

If we know that the Ca is simply this abbreviation for their calcium. But they are still what are those numbers? The ’20’ in this top right corner simply refers to the fact that their calcium is element number 20. The 40.08 on the bottom is the most important number right now. This is the atomic weight for their calcium. The atomic weight of each other element is the weight (in grams) of 1 mole for that particular element.

### 4. Using Moles to Determine Mass

The nice thing about us is that they are using these moles to talk about some chemical equations we know the weight of each other element in a mole. If we can this weight for some molecules simply by adding all of these weights for each other atoms.

### 5. Moles of elements

Their one mole for these carbon atoms has a mass of exactly 12 g. However these magnesium atoms each have twice the mass of some carbon atoms (24Mg compared with 12C), one mole for magnesium has a mass of 24 g. One mole of any other element has a mass in these grams that is equal to its relative atomic mass. One mole of iron has a mass of 56 g.

### 6. Moles of compounds

A mole for a molecular compound contains 6 x 1023 molecules. If it has a mass that is equal to its relative formula mass. So a mole of water (H2O) has a mass of 18 g. A mole for carbon dioxide (CO2) has a mass of 44 g. These also work for some ionic compounds, so a mole of sodium chloride (NaCl) has a mass of 58.5 g.

### 7. The Avogadro number

Their one mole of these atoms contains 6 x 1023 atoms, no matter what element it is. This is a very large number: if it is 6 with 23 zeros after it. It is also known as the Avogadro number. This number is also used in chemistry however if you could count out this many more carbon atoms, the total mass for carbon you would have is 12 g. On the other hand, weighing out 12 g of carbon allows you to know how many more atoms you have.

# What is Mole and Why do we use Moles in Chemistry

If the relative formula mass for a compound is calculated by adding together their relative atomic mass these values for all the atoms in its formula. These moles are units used to measure their substance amount.

## How do you calculate moles in chemistry?

How to find these moles in this solution is to calculate how many more molecules this solution contains. Also, to do this you need to know the volume of this solution and how many more solutes have been dissolved in this solution.

Furthermore, you also need to know the molar mass of this solute. If it refers to a very huge number that we use to measure these atoms.

Moreover, it is more equal to this number for some atoms in 12 grams for carbon-12 which is just about 6.022 × 1023 these atoms. Just like that this way, it is very much easier to measure intergalactic (Space) distance in light-years than to measure it in these inches. Also, it is much easier to calculate these atoms in a mole than in lakhs or crores.

## What is the mole and why do we use moles in chemistry

In this lesson, we will explore these chemical equations or what we can learn about them using these moles. We will learn what a mole is or how moles are used to determine the mass needed for a reaction to occur.

## 1. What Are Moles?

In their chemistry, we frequently use the word these ‘moles’ to refer to the amount of these chemicals used. If this mole is not their little animal that they are digging around in your yard, they instead refer to a set quantity for some of these atoms. If they think of it like this word ‘dozen’. When you say about two dozen these eggs, you mean that these two sets of 12 eggs.

These moles represent a very much bigger number though, 6.023 times ten to this 23rd, which is called ‘Avogadro’s number’. So instead of saying, ‘I have a dozen of these atoms’ we can say that ‘I have an Avogadro’s number of some atoms’ (in chemistry we don’t very typically say it like that, but it’s a good way to think about what a mole their means).

### 2. Moles in Chemical Equations

Right now let’s think about these dozen atoms again concerning this water reaction or some moles.

Now we see that these 2 molecules of hydrogen react with 1 molecule of oxygen to form 2 molecules of water. Now very typically we aren’t only making 1 molecule (remember, that they would be in such a very small quantity that we wouldn’t be able to see it let alone measure it out).

So let’s double it. This would mean that we are using these 4 molecules from hydrogen to react with 2 molecules for the oxygen to form some 4 molecules from the water. How about a dozen times each? There are 2 dozen hydrogen molecules or 1 dozen oxygen.

These molecules are making 2 dozen water molecules. So really, it is 24 hydrogen molecules reacting with these 12 oxygen molecules to make some 24 water molecules, but they are still instead of saying 24, 12, or 24 we can look at it as some multiples for a dozen.

### 3. Moles and the Periodic Table

There sometimes a periodic table will simply have these names or abbreviations for each other element in these blocks. But they are still these. Sometimes we will see your numbers in these blocks. Let’s look at calcium.

If we know that the Ca is simply this abbreviation for their calcium. But they are still what are those numbers? The ’20’ in this top right corner simply refers to the fact that their calcium is element number 20. The 40.08 on the bottom is the most important number right now. This is the atomic weight for their calcium. The atomic weight of each other element is the weight (in grams) of 1 mole for that particular element.

### 4. Using Moles to Determine Mass

The nice thing about us is that they are using these moles to talk about some chemical equations we know the weight of each other element in a mole. If we can this weight for some molecules simply by adding all of these weights for each other atoms.

### 5. Moles of elements

Their one mole for these carbon atoms has a mass of exactly 12 g. However these magnesium atoms each have twice the mass of some carbon atoms (24Mg compared with 12C), one mole for magnesium has a mass of 24 g. One mole of any other element has a mass in these grams that is equal to its relative atomic mass. One mole of iron has a mass of 56 g.

### 6. Moles of compounds

A mole for a molecular compound contains 6 x 1023 molecules. If it has a mass that is equal to its relative formula mass. So a mole of water (H2O) has a mass of 18 g. A mole for carbon dioxide (CO2) has a mass of 44 g. These also work for some ionic compounds, so a mole of sodium chloride (NaCl) has a mass of 58.5 g.

### 7. The Avogadro number

Their one mole of these atoms contains 6 x 1023 atoms, no matter what element it is. This is a very large number: if it is 6 with 23 zeros after it. It is also known as the Avogadro number. This number is also used in chemistry however if you could count out this many more carbon atoms, the total mass for carbon you would have is 12 g. On the other hand, weighing out 12 g of carbon allows you to know how many more atoms you have.