1. Atoms To Moles Calc
2. Moles To Atoms To Molecules
3. Converting Between Moles Atoms And Molecules

A mole of water molecules contains 2 moles of hydrogen atoms and 1 mole of oxygen atoms. 2 Sulfuric acid has the chemical formula H 2 SO 4. A certain quantity of sulfuric acid contains 4.89 × 10 25 atoms of oxygen. This online calculator converts moles to liters of a gas at STP (standard temperature and pressure) and liters of gas to moles. The conversion is straightforward and is based on the fact that the ideal gas equation is a good approximation for many common gases at standard temperature and pressure. » Moles Conversions: mol↔mmol 1 mol = 1000 mmol mol↔umol 1 mol = 1000000 umol mol↔nmol 1 mol = nmol mol↔pmol 1 mol = 000 pmol mol↔fmol 1 mol = 1.0E+15 fmol mol↔kmol 1 kmol = 1000 mol mol↔atoms 1 mol = 6.02E+23 atoms » Atoms Conversions: atoms↔mol 1 mol = 6.02E+23 atoms atoms↔mmol 1 mmol = 6.02E+20 atoms. Module Two – Atoms, Molecules and Moles mass units (amu), where 1 amu is defined as 1/12 of the mass of an atom of carbon-12. The atomic mass of carbon-12, therefore, is exactly 12 amu.

Learning Objective

• Convert between the number of moles and the number of atoms in a given substance using Avagadro’s number

Key Points

• Avogadro’s number is a very important relationship to remember: 1 mole = [latex]6.022times10^{23}[/latex]atoms, molecules, protons, etc.
• To convert from moles to atoms, multiply the molar amount by Avogadro’s number.
• To convert from atoms to moles, divide the atom amount by Avogadro’s number (or multiply by its reciprocal).

Terms

• moleThe amount of substance of a system that contains as many elementary entities as there are atoms in 12 g of carbon-12.
• Avogadro’s numberThe number of atoms present in 12 g of carbon-12, which is [latex]6.022times10^{23}[/latex] and the number of elementary entities (atoms or molecules) comprising one mole of a given substance.

Moles and Atoms

As introduced in the previous concept, the mole can be used to relate masses of substances to the quantity of atoms therein. This is an easy way of determining how much of one substance can react with a given amount of another substance.

From moles of a substance, one can also find the number of atoms in a sample and vice versa. The bridge between atoms and moles is Avogadro’s number, 6.022×10²³.

Avogadro’s number is typically dimensionless, but when it defines the mole, it can be expressed as 6.022×10²³ elementary entities/mol. This form shows the role of Avogadro’s number as a conversion factor between the number of entities and the number of moles. Therefore, given the relationship 1 mol = 6.022 x 10²³ atoms, converting between moles and atoms of a substance becomes a simple dimensional analysis problem.

Converting Moles to Atoms

Given a known number of moles (x), one can find the number of atoms (y) in this molar quantity by multiplying it by Avogadro’s number:

[latex]x moles cdot frac {6.022times10^{23} atoms}{1 mole} = y atoms[/latex]

For example, if scientists want to know how may atoms are in six moles of sodium (x = 6), they could solve:

[latex]6 moles cdot frac {6.022times 10^{23} atoms}{1 mole} = 3.61times 10^{24} atoms[/latex]

Note that the solution is independent of whether the element is sodium or otherwise.

Converting Atoms to Moles

Reversing the calculation above, it is possible to convert a number of atoms to a molar quantity by dividing it by Avogadro’s number:

[latex]frac{x atoms}{6.022times 10^{23} frac{atoms}{1 mole}} = y moles[/latex]

This can be written without a fraction in the denominator by multiplying the number of atoms by the reciprocal of Avogadro’s number:

[latex]x atoms cdot frac{1 mole}{6.022times 10^{23} atoms} = y moles[/latex]

For example, if scientists know there are [latex]3.5 cdot 10^{24} [/latex]atoms in a sample, they can calculate the number of moles this quantity represents:

[latex]3.5 times 10^{24} atoms cdot frac{1 mole}{6.022times 10^{23} atoms} = 5.81 moles[/latex]

Boundless vets and curates high-quality, openly licensed content from around the Internet. This particular resource used the following sources:

http://www.boundless.com/
Boundless Learning
CC BY-SA 3.0.

http://en.wiktionary.org/wiki/mole
Wiktionary
CC BY-SA 3.0.

http://en.wikipedia.org/wiki/Avogadro’s%20number
Wikipedia
CC BY-SA 3.0.

http://en.wikipedia.org/wiki/Avogadro_constant
Wikipedia
CC BY-SA 3.0.

Figure (PageIndex{1}) shows that we need 2 hydrogen atoms and 1 oxygen atom to make 1 water molecule. If we want to make 2 water molecules, we will need 4 hydrogen atoms and 2 oxygen atoms. If we want to make 5 molecules of water, we need 10 hydrogen atoms and 5 oxygen atoms. The ratio of atoms we will need to make any number of water molecules is the same: 2 hydrogen atoms to 1 oxygen atom.

One problem we have, however, is that it is extremely difficult, if not impossible, to organize atoms one at a time. As stated in the introduction, we deal with billions of atoms at a time. How can we keep track of so many atoms (and molecules) at a time? We do it by using mass rather than by counting individual atoms.

A hydrogen atom has a mass of approximately 1 u. An oxygen atom has a mass of approximately 16 u. The ratio of the mass of an oxygen atom to the mass of a hydrogen atom is therefore approximately 16:1.

If we have 2 atoms of each element, the ratio of their masses is approximately 32:2, which reduces to 16:1—the same ratio. If we have 12 atoms of each element, the ratio of their total masses is approximately (12 × 16):(12 × 1), or 192:12, which also reduces to 16:1. If we have 100 atoms of each element, the ratio of the masses is approximately 1,600:100, which again reduces to 16:1. As long as we have equal numbers of hydrogen and oxygen atoms, the ratio of the masses will always be 16:1.

The same consistency is seen when ratios of the masses of other elements are compared. For example, the ratio of the masses of silicon atoms to equal numbers of hydrogen atoms is always approximately 28:1, while the ratio of the masses of calcium atoms to equal numbers of lithium atoms is approximately 40:7.

So we have established that the masses of atoms are constant with respect to each other, as long as we have the same number of each type of atom. Consider a more macroscopic example. If a sample contains 40 g of Ca, this sample has the same number of atoms as there are in a sample of 7 g of Li. What we need, then, is a number that represents a convenient quantity of atoms so we can relate macroscopic quantities of substances. Clearly even 12 atoms are too few because atoms themselves are so small. We need a number that represents billions and billions of atoms.

Chemists use the term mole to represent a large number of atoms or molecules. Just as a dozen implies 12 things, a mole (abbreviated as mol) represents 6.022 × 10²³ things. The number 6.022 × 10²³, called Avogadro’s number after the 19th-century chemist Amedeo Avogadro, is the number we use in chemistry to represent macroscopic amounts of atoms and molecules. Thus, if we have 6.022 × 10²³ Na atoms, we say we have 1 mol of Na atoms. If we have 2 mol of Na atoms, we have 2 × (6.022 × 10²³) Na atoms, or 1.2044 × 10²⁴ Na atoms. Similarly, if we have 0.5 mol of benzene (C₆H₆) molecules, we have 0.5 × (6.022 × 10²³) C₆H₆ molecules, or 3.011 × 10²³ C₆H₆ molecules.

A mole represents a very large number! If 1 mol of quarters were stacked in a column, it could stretch back and forth between Earth and the sun 6.8 billion times.

Notice that we are applying the mole unit to different types of chemical entities. The word mole represents a number of things—6.022 × 10²³ of them—but does not by itself specify what “they” are. The chemical entities can be atoms,molecules, formula units and ions. This specific information needs to be specified accurately. Most students find this confusing hence, we need to review the composition of elements, covalent and ionic compounds.

Most elements are made up of individual atoms, such as helium. However, some elements consist of molecules, such as the diatomic elements, nitrogen, hydrogen, oxygen, etc. discussed in Section 2.2. One mole of He consists of 6.022 × 10²³ He atoms but one mole of nitrogen contains 6.022 × 10²³ N₂molecules. The basic units of covalent (molecular) compounds are molecules as well. The molecules of 'compounds' consist of different kinds of atoms while the molecules of 'elements' consist of only one type of atom. For example, the molecules of ammonia (NH₃) consist of nitrogen and hydrogen atoms while N₂ molecules have N atoms only. Compounds that are ionic, like NaCl, are represented by ionic formulas. One mole of NaCl, for example, refers to 6.022 × 10²³ formula units of NaCl. And, one formula unit of NaCl consists of one sodium ion and one chloride ion. Figure 6.1.2 summarizes the basic units of elements, covalent and ionic compounds

Conversion Between Moles and Atoms, Molecules and Ions

Using our unit conversion techniques learned in Chapter 1, we can use the mole relationship and the chemical formula to convert back and forth between the moles and the number of chemical entities (atoms, molecules or ions).

Because 1 N₂ molecule contains 2 N atoms, 1 mol of N₂ molecules (6.022 × 10²³ molecules) has 2 mol of N atoms. Using formulas to indicate how many atoms of each element we have in a substance, we can relate the number of moles of molecules to the number of moles of atoms. For example, in 1 mol of ethanol (C₂H₆O), we can construct the following relationships (Table (PageIndex{1})):

The following example illustrates how we can use these relationships as conversion factors.

Example (PageIndex{1})

If a sample consists of 2.5 mol of ethanol (C₂H₆O), how many moles of carbon atoms, hydrogen atoms, and oxygen atoms does it have?

Solution

Using the relationships in Table (PageIndex{1}), we apply the appropriate conversion factor for each element:

Note how the unit mol C₂H₆O molecules cancels algebraically. Similar equations can be constructed for determining the number of H and O atoms:

Atoms To Moles Calc

(mathrm{2.5: mol: C_2H_6O: moleculestimesdfrac{6: mol: H: atoms}{1: mol: C_2H_6O: molecules}=15: mol: H: atoms})

(mathrm{2.5: mol: C_2H_6O: moleculestimesdfrac{1: mol: O: atoms}{1: mol: C_2H_6O: molecules}=2.5: mol: O: atoms})

Exercise (PageIndex{1})

If a sample contains 6.75 mol of Na₂SO₄, how many moles of sodium atoms, sulfur atoms, and oxygen atoms does it have?

13.5 mol Na, 6.75 mol S and 27 mol O.

We can use Avogadro's number as a conversion factor, or ratio, in dimensional analysis problems. For example, if we are dealing with element X, the mole relationship is expressed as follows:

[text{1 mol X} = 6.022 times 10^{23} text{ X atoms}]

We can convert this relationship into two possible conversion factors shown below:

(mathrm{dfrac{1: mol: X: }{6.022times 10^{23}: X: atoms}}) or (mathrm{dfrac{6.022times 10^{23}: X: atoms}{1: mol: X: }})

If the number of 'atoms of element X' is given, we can convert it into 'moles of X' by multiplying the given value with the conversion factor at the left. However, if the number of 'mol of X' is given, the appropriate conversion factor to use is the one at the right.

If we are dealing with a molecular compound (such as C₄H₁₀), the mole relationship is expressed as follows:

[text{1 mol C4H10} = 6.022 times 10^{23} text{ C4H10 molecules}]

If working with ionic compounds (such as NaCl), the mole relationship is expressed as follows:

Moles To Atoms To Molecules

[text{1 mol NaCl} = 6.022 times 10^{23} text{ NaCl formula units}]

Example (PageIndex{2})

How many formula units are present in 2.34 mol of NaCl? How many ions are in 2.34 mol?

Buffalo port devices driver download for windows. Solution

Typically in a problem like this, we start with what we are given and apply the appropriate conversion factor. Here, we are given a quantity of 2.34 mol of NaCl, to which we can apply the definition of a mole as a conversion factor:

(mathrm{2.34: mol: NaCltimesdfrac{6.022times10^{23}: NaCl: units}{1: mol: NaCl}=1.41times10^{24}: NaCl: units})

Because there are two ions per formula unit, there are

(mathrm{1.41times10^{24}: NaCl: unitstimesdfrac{2: ions}{NaCl: units}=2.82times10^{24}: ions})

in the sample.

Exercise (PageIndex{2})

How many molecules are present in 16.02 mol of C₄H₁₀? How many atoms are in 16.02 mol?

9.647 x 10²⁴molecules, 1.351 x 10²⁶ atoms.

Converting Between Moles Atoms And Molecules

Answer

Key Takeaway

• A mole is 6.022 × 10²³ things.

Exercises

1. How many dozens are in 1 mol? Express your answer in proper scientific notation.

2. A gross is a dozen dozen, or 144 things. How many gross are in 1 mol? Drivers atel mobile phones & portable devices. Express your answer in proper scientific notation.

3. How many moles of each type of atom are in 1.0 mol of C₆H₁₂O₆?

4. How many moles of each type of atom are in 1.0 mol of K₂Cr₂O₇?

5. How many moles of each type of atom are in 2.58 mol of Na₂SO₄?

6. How many moles of each type of atom are in 0.683 mol of C₃₄H₃₂FeN₄O₄? (This is the formula of heme, a component of hemoglobin.)

7. Amedtec medizintechnik aue driver download. How many formula units are in 0.778 mol of iron(III) nitrate?

8. A sample of gold contains 7.02 × 10²⁴ atoms. How many moles of gold is this?

9. A flask of mercury contains 3.77 × 10²² atoms. How many moles of mercury are in the flask?

10. An intravenous solution of normal saline may contain 1.72 mol of sodium chloride (NaCl). How many sodium and chlorine atoms are present in the solution?

11. A lethal dose of arsenic is 1.00 × 10²¹ atoms. How many moles of arsenic is this?

Answers

3. 6.0 mol of C atoms, 12.0 mol of H atoms, and 6.0 mol of O atoms

5. 5.16 mol of Na atoms, 2.58 mol of S atoms, and 10.32 mol of O atoms

11. 1.04 × 10²⁴ Na atoms and 1.04 × 10²⁴ Cl atoms