Which of the following will determine the number of moles in a sample Dividing the mass of the sample by Avogadro’s number Multiplying the mass of the sample by Avogadro’s number Dividing the number of molecules in the sample by Avogadro’s number Multiplying the number of molecules in the sample by Avogadro’s number. A mole is a quantity that contains 6.02.10 23 atoms, molecules and ions. Avogadro’s number is the number of particles in a mole 6.02.10 23. The mole (or mol) represents a certain number of objects. The amount of a substance that contains the same number of entities as there are atoms in 12 g of carbon-12.

A mole is defined as the quantity of a substance that has the same number of particles as are found in 12.000 grams of carbon-12. This number, Avogadro's number, is 6.022x10 23. Avogadro's number may be applied to atoms, ions, molecules, compounds, elephants, desks, or any object. Mole Day - Avogadro's Number. Search this site. Happy Mole Day!! Celebrations of Mole Day. Additional Pages. To appreciate the magnitude of Avogadro’s number, consider a mole of pennies. Stacked vertically, a mole of pennies would be 4.5 × 10 17 mi high, or almost six times the diameter of the Milky Way galaxy. If a mole of pennies were distributed equally among the entire population on Earth, each person would have more than one trillion dollars.

The number of moles in a system can be determined using the atomic mass of an element, which can be found on the periodic table. This mass is usually an average of the abundant forms of that element found on earth. An element's mass is listed as the average of all its isotopes on earth.

Avogadro's Constant

One mole of oxygen atoms contains (6.02214179 times 10^{23}) oxygen atoms. Also, one mole of nitrogen atoms contains (6.02214179 times 10^{23}) nitrogen atoms. The number (6.02214179 times 10^{23}) is called Avogadro's number ((N_A)) orAvogadro's constant, after the 19^th century scientist Amedeo Avogadro.

Each carbon-12 atom weighs about (1.99265 times 10^{-23}; g); therefore,

[(1.99265 times 10^{-23}; g) times (6.02214179 times 10^{23}; atoms) = 12; g; text{ of carbon-12} nonumber ]

Applications of the Mole

The mass of a mole of substance is called the molar mass of that substance. The molar mass is used to convert grams of a substance to moles and is used often in chemistry. The molar mass of an element is found on the periodic table, and it is the element's atomic weight in grams/mole (g/mol). If the mass of a substance is known, the number of moles in the substance can be calculated. Converting the mass, in grams, of a substance to moles requires a conversion factor of (one mole of substance/molar mass of substance).

The mole concept is also applicable to the composition of chemical compounds. For instance, consider methane, CH₄. This molecule and its molecular formula indicate that per mole of methane there is 1 mole of carbon and 4 moles of hydrogen. In this case, the mole is used as a common unit that can be applied to a ratio as shown below:

[2 text{ mol H } + 1 text{ mol O }= 1 text{ mol } ce{H2O} nonumber]

In this this chemical reactions, the moles of H and O describe the number of atoms of each element that react to form 1 mol of (ce{H_2O}).

To think about what a mole means, one should relate it to quantities such as dozen or pair. Just as a pair can mean two shoes, two books, two pencils, two people, or two of anything else, a mole means 6.02214179×10²³ of anything. Using the following relation:

[text{1 mole} = 6.02214179 times 10^{23}]

is analogous to saying:

[text{1 Dozen} = text{12 eggs}]

It is quite difficult to visualize a mole of something because Avogadro's constant is extremely large. For instance, consider the size of one single grain of wheat. If all the people who have existed in Earth's history did nothing but count individual wheat grains for their entire lives, the total number of wheat grains counted would still be much less than Avogadro's constant; the number of wheat grains produced throughout history does not even approach Avogadro's Number.

Example (PageIndex{1}): Converting Mass to Moles

How many moles of potassium ((ce{K})) atoms are in 3.04 grams of pure potassium metal?

Solution

In this example, multiply the mass of (ce{K}) by the conversion factor (inverse molar mass of potassium):

[dfrac{1; mol; K}{39.10; grams ;K} nonumber ]

39.10 grams is the molar mass of one mole of (ce{K}); cancel out grams, leaving the moles of (ce{K}):

[3.04; cancel{g; K} left(dfrac{1; mol; K}{39.10; cancel{g; K}}right) = 0.0778; mol; K nonumber ]

Similarly, if the moles of a substance are known, the number grams in the substance can be determined. Converting moles of a substance to grams requires a conversion factor of molar mass of substance/one mole of substance. One simply needs to follow the same method but in the opposite direction.

Example (PageIndex{2}): Converting Moles to mass

How many grams are 10.78 moles of Calcium ((ce{Ca}))?

Solution

Multiply moles of Ca by the conversion factor (molar mass of calcium) 40.08 g Ca/ 1 mol Ca, which then allows the cancelation of moles, leaving grams of Ca.

[10.78 cancel{;mol; Ca} left(dfrac{40.08; g; Ca}{1; cancel{mol; Ca}}right) = 432.1; g; Ca nonumber ]

The total number of atoms in a substance can also be determined by using the relationship between grams, moles, and atoms. If given the mass of a substance and asked to find the number of atoms in the substance, one must first convert the mass of the substance, in grams, to moles, as in Example (PageIndex{1}). Then the number of moles of the substance must be converted to atoms. Converting moles of a substance to atoms requires a conversion factor of Avogadro's constant (6.02214179×10²³) / one mole of substance. Verifying that the units cancel properly is a good way to make sure the correct method is used.

Example (PageIndex{3}): Atoms to Mass

How many atoms are in a 3.5 g sample of sodium (Na)?

Solution

[3.5; cancel{g; Na} left(dfrac{1; mol; Na}{22.98; cancel{g; Na}}right) = 0.152; mol; Na nonumber ]

[0.152; cancel{mol; Na} left(dfrac{6.02214179times 10^{23}; atoms; Na}{1;cancel{ mol; Na}}right) = 9.15 times 10^{22}; atoms; of; Na nonumber ]

In this example, multiply the grams of Na by the conversion factor 1 mol Na/ 22.98 g Na, with 22.98g being the molar mass of one mole of Na, which then allows cancelation of grams, leaving moles of Na. Then, multiply the number of moles of Na by the conversion factor 6.02214179×10²³ atoms Na/ 1 mol Na, with 6.02214179×10²³ atoms being the number of atoms in one mole of Na (Avogadro's constant), which then allows the cancelation of moles, leaving the number of atoms of Na.

Using Avogadro's constant, it is also easy to calculate the number of atoms or molecules present in a substance (Table (PageIndex{1})). By multiplying the number of moles by Avogadro's constant, the mol units cancel out, leaving the number of atoms. The following table provides a reference for the ways in which these various quantities can be manipulated:

Example (PageIndex{4}): Mass to Moles

How many moles are in 3.00 grams of potassium (K)?

Solution

[3.00 ; cancel{g; K} left(dfrac{1; mol; K}{39.10; cancel{g; K}}right) = 0.0767; mol; K nonumber ]

In this example, multiply the mass of K by the conversion factor:

[dfrac{1; mol; K}{39.10; grams; K} nonumber ]

39.10 grams is the molar mass of one mole of K. Grams can be canceled, leaving the moles of K.

Example (PageIndex{5}): Moles to Mass

How many grams is in 10.00 moles of calcium (Ca)?

Solution

This is the calculation in Example (PageIndex{2}) performed in reverse. Multiply moles of Ca by the conversion factor 40.08 g Ca/ 1 mol Ca, with 40.08 g being the molar mass of one mole of Ca. The moles cancel, leaving grams of Ca:

[10.00; cancel{mol; Ca} left(dfrac{40.08; g; Ca}{1;cancel{ mol; Ca}}right) = 400.8; grams ;of ;Ca nonumber ]

The number of atoms can also be calculated using Avogadro's Constant (6.02214179×10²³) / one mole of substance.

Example (PageIndex{6}): Mass to Atoms

How many atoms are in a 3.0 g sample of sodium (Na)?

Solution

Convert grams to moles

[3.0; cancel{g; Na} left(dfrac{1; mol; Na}{22.98; cancel{g; Na}}right) = 0.130; mol; Na nonumber ]

Convert moles to atoms

[0.130548; cancel{ mol; Na} left(dfrac{6.02214179 times 10^{23}; atoms ;Na}{1; cancel{ mol; Na}}right) = 7.8 times 10^{22} ; atoms; of; ; Na nonumber ]

Summary

The mole, abbreviated mol, is an SI unit which measures the number of particles in a specific substance. One mole is equal to (6.02214179 times 10^{23}) atoms, or other elementary units such as molecules.

Problems

1. Using a periodic table, give the molar mass of the following:
   1. H
   2. Se
   3. Ne
   4. Cs
   5. Fe
2. Convert to moles and find the total number of atoms.
   1. 5.06 grams of oxygen
   2. 2.14 grams of K
   3. 0.134 kg of Li
3. Convert the following to grams
   1. 4.5 mols of C
   2. 7.1 mols of Al
   3. 2.2 mols of Mg
4. How many moles are in the product of the reaction
   1. 6 mol H + 3 mol O → ? mol H₂O
   2. 1 mol Cl + 1 mol Cl → ? mol Cl₂
   3. 5 mol Na + 4 mol Cl → ? mol NaCl

Answers

1. Question 2
   1. 1.008 g/mol
   2. 78.96 g/mol
   3. 20.18 g/mol
   4. 132.91g/mol
   5. 55.85 g/mol
2. Question 2

2. 5.06g O (1mol/16.00g)= 0.316 mol of O

0.316 mols (6.022x10²³ atoms/ 1mol) = 1.904x10²³ atoms of O

3. 2.14g K (1mol/39.10g)= 0.055 mol of K

0.055 mols (6.022x10²³ atoms/ 1mol) = 3.312x10²² atoms of K

4. 0.134kg Li (1000g/1kg)= 134g Li (1mol/6.941g)= 19.3 mols Li

19.3 (6.022x10²³ atoms/ 1mol) = 1.16x10²⁵ atoms of Li

Chemistry Mole And Avogadro's Number

3. Question 3
   1. 4.5 mols of C (12.011g/1mol) = 54.05 g of C
   2. 7.1 mols of Al (26.98g/1mol) = 191.56 g of Al
   3. 2.2 mols of Mg (24.31g/1mol) = 53.48 g of MG
4. Question 4
   1. 8. 6 mol H + 3 mol O → 3 mol H₂O
   2. 9. 1 mol Cl + 1 mol Cl → 1 mol Cl₂
   3. _{10. 5 mol Na + 4 mol Cl → 4 mol NaCl + 1 mol Na (excess)}

References

1. Keenan, Charles W. and Wood, Jesse H. . General College Chemistry. 4th ed. New York: Haper and Row, 1971.
2. Mortimer, Charles E. Chemistry a Conceptual Approach. 2nd ed. New York: Van Nostrand Reinhold, 1971.
3. Jones, Loretta and Atkins, Peter. Chemistry: Molecules, Matter, and Change. 4th ed. New York: W.H. Freeman, 2000.
4. Petrucci, Ralph H., Herring, Goeffrey F., Madura, Jeffrey D., and Bissonnette, Carey. General Chemistry: Principles and Modern Applications. 10th ed. New Jersey: Pearson Canada, 2011.

Mole Avogadro's Number Worksheet

Contributors and Attributions

Moles Times Avogadro's Number

• Ryan Benoit (UCD), Michael Thai (UCD), Charlie Wang (UCD), Jacob Gomez (UCD)