# Mole Chemistry Number

**Why do chemists need the Mole Concept?**

But when chemists talk about moles, they’re usually referring to a scientific term. The term ‘mole’ represents a number, in the same way the word ‘dozen’ represents 12 of something. In this case, one mole represents the enormous (and slightly strange) number, 6.02 x 10 23. This is a huge number! The mole is used in chemistry to represent 6.022 × 10 23 of something, but it can be difficult to conceptualize such a large number. Watch this video and then complete the “Think” questions that follow. Explore more about the mole by reviewing the information under “Dig Deeper.”. One mole of atoms contains 6 x 1023 atoms, no matter what element it is. This is a very large number: it is 6 with 23 zeros after it. It is known as the Avogadro number. This number is used in.

Chemists need the mole concept to bridge the gap between the microscopic world of atoms to the macroscopic world of humans. As you know, the molecular level consists of particles that are invisible to us. Because of this, chemists can’t count or weigh these individual particles on a scale.

**So, how do chemists get around this problem?**

To solve this problem, chemists introduced the **mole concept. The mole is the unit for the SI base quantity the Amount of Substance. **And the mole concept connects the macroscopic to the atomic or molecular level. Let use the following model to illustrate:

**What’s the Amount of Substance?**

The **Amount of substance** is a quantity that measures the **size of a pile** (collection) of particles. These particles can be electrons, atoms, molecules, ions, or formula units. The amount of substance is an ** SI**measured quantity that has a symbol

*n*, and a base unit of

*mole*, which is often written in a short way as

*mol*.

**What’s a Mole?**

Teamviewer previous version 10 for macpaperslasopa. A mole is the size of a pile of particles (**amount of substance)** that contains as many particles (electrons, atoms, molecules, ions, or formula units) as there are atoms in 12 grams of carbon-12 **(an isotope of carbon)**. Therefore, a mole or

1 mole of carbon-12 = 12 grams of carbon-12

**What amount of substance can have the same number of particles as in 12g of carbon-12? **The amount of substance that can have the same number of particles include:

### Mole In Chemistry For Kids

- atomic mass of an element expressed in grams
- molecular mass of molecular compounds expressed in grams
- formula mass of ionic compounds expressed in grams

**What do we mean by the atomic mass expressed in grams?**

### Define Mole

It means that we take the relative atomic mass values of all the elements on the periodic table and attach grams to them. Once we do that, we can now weigh 1 mole of any element by simply weighing its exact atomic mass in grams. Similarly, since atoms combine to make molecules, we can find the molecular mass of any molecule by simply finding the sum of all the atomic masses in the chemical formula. The following table shows how to transition from atomic mass (amu) to molar mass (g/mol).

**Why is it that 1 mole of any element has the same number of particles as in 1 mole of carbon-12?**

They do because of **Avogadro’s hypothesis**, and recall that it was his hypothesis that helped scientists determine the relative atomic masses of the elements.

Now, **how many particles (atoms, molecules, or ions) are in 1 mole of a chemical substance?** There are 6.02 x 10^{22 }particles in 1 mole of any chemical substance. As you can see, this number is so huge that it has a special name called the **Avogadro’s number** in honor of Avogadro; The Italian mathematician who contributed to our understanding of the mole concept.

Mathematically, we can write a relationship between 1 mole, Avogadro’s number, and atomic mass in grams. For example, we can write that 1 mole of carbon is equal to 12 g of carbon and in this 12 g there are 6.02 x 10^{22 }atoms of carbon. If we translate that to a mathematical expression, we will get;

- 1 mole = 12 g = 6.02 x 10
^{22 }atoms of carbon.

If we divide through by 1 mole, we will get two ratios:

**12 g**/1mole- 6.02 x 10
^{22 }atoms of carbon/1mole.

The ratio 12 g/1 mole or 12 g/mol (read as grams per mol) has a special name called Molar Mass. So, the molar mass is simply the mass of 1 mol of a substance in grams. As a result, the only number that will keep changing from substance to substance is the mass of 1 mole of substance (see text in bold). Now, if you need to convert some certain grams of carbon to atoms of carbon or atoms of carbon to grams of carbon, the two ratios, or conversion factors we just derived are the ones we will use.

### Here is a model that shows the relationship between Mass, Mole, and Avogadro’s number

**How is the mole related to the dozen?**

We can relate the mole to the counting unit: **Dozen**. We buy eggs by the dozen, we buy soda by the dozen, we buy many things by the dozen, and we know that a dozen always contains 12 things. However, as we buy a dozen of this and a dozen of that, the only number that keeps changing is the mass of the items in the dozen. As a result, we can write a mathematical expression similar to the mole one. Let’s say if a dozen eggs weigh 10 g, then we can write something like this: 10 g = 1 Dozen = 12 eggs. If we divide through by 1 Dozen, we will get two ratios:

**10 g**/1Dozen and- 12eggs/1Dozen,

### Mole In Chemistry Examples

These ratios are the ones we will use to convert from grams of eggs to Dozen of eggs to number of eggs and in reverse order.

**How to generate mathematical relationships to convert from grams to molecules and vice versa**

Once you understand how grams of substance relate to moles, how moles of substance relate to Avogadro’s number and vice versa, you will always find mole problems easy to solve. Here is a diagram summarizing these relationships.

**Check you understanding**

- If you have a sample of 10 mol of carbon dioxide (CO
_{2}), how many molecules of CO_{2 }are in the sample? - Calculate the molar mass of sulfuric acid (H
_{2}SO_{4}) - If you have a sample of 5.0 g of sulfuric acid, how many mol of sulfuric acid are in the sample?