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.

1. Mass Of 1 Mole Of Nitrogen Atom Is Made
2. 1 Mole Of Nitrogen Gas
3. Mass Of 1 Mole Of Nitrogen Atom Is Measured

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,

The molar mass of an element is equal to its. Preview this quiz on Quizizz. The molar mass of an element is equal to its. Molar Mass DRAFT. 9th - 12th grade. What is the atomic mass of one atom of Nitrogen? Tags: Question 26.

1. Well, a mole of 'nitrogen atoms' has HALF the mass of a mole of 'nitrogen molecules'. The dinitrogen molecule, N-=N, contains TWO nitrogen atoms; and of course has twice the number of atoms, and twice the mass of an isolated nitrogen atom, N. Inorganic chemists often speak of the 'dinitrogen' or 'dihydrogen' or even the 'dioxygen molecule' to distinguish the molecular species from the.
2. If one mole of nitrogen molecule weighs 14 grams what is the mass in grams of one atom of nitrogen - Chemistry - TopperLearning.com 03u4kkouu.

[(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

Mass Of 1 Mole Of Nitrogen Atom Is Made

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

1 Mole Of Nitrogen Gas

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

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.

Contributors and Attributions

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

Question #b3926

1 Answer

Explanation:

The trick here is to realize that you're actually looking for the number of moles of atoms present in, presumably, #'7 g'# of nitrogen gas, #'N'_2#.

For starters, a gram-atom is simply Avogadro's constant of atoms, regardless if those atoms are combined in molecules or formula units or floating around on their own.

This is the important distinction between a mole and a gram-atom: a mole of a given substance contains Avogadro's constant of molecules, formula units, or atoms of said substance, while a gram-atom of a given substance contains Avogadro's constant of atoms, regardless of the nature of the substance (molecular, ionic).

In your case, a mole of nitrogen gas contains #6.022 * 10^(23)#molecules of nitrogen gas, #'N'_2# and #2#moles of nitrogen atoms, #'N'#.

You can thus say that a mole of nitrogen gas is equivalent to #2#gram-atoms of nitrogen, or that #1#gram-atom of nitrogen gas is equivalent to #1/2#moles of nitrogen gas.

Now, a mole of nitrogen gas has a mass of approximately #'28 g'# as given by the molar mass of nitrogen gas, which is equal to #'28 g mol'^(-1)#.

This means that you sample contains

#7 color(red)(cancel(color(black)('g'))) * '1 mole N'_2/(28color(red)(cancel(color(black)('g')))) = '0.25 moles N'_2#

You can thus say that the sample contains

#0.25 color(red)(cancel(color(black)('moles N'_2))) * '2 gram-atoms N'_2/(1color(red)(cancel(color(black)('mole N'_2)))) = color(darkgreen)(ul(color(black)('0.5 gram-atoms N'_2)))#

The answer is rounded to one significant figure.

Notice that you get the same answer is you assume that you're dealing with #'7 g'# of elemental nitrogen, #'N'#.

The molar mass of elemental nitrogen is approximately #'14 g mol'^(-1)#, which means that #'7 g'# will contain

#7 color(red)(cancel(color(black)('g'))) * '1 mole N'/(14color(red)(cancel(color(black)('g')))) = '0.5 moles N'#

Now, a gram-atom of nitrogen atoms simply means Avogadro's number of nitrogen atoms, so you can say that #1#mole of nitrogen atoms is equivalent to #1#gram-atom of nitrogen atoms. Iso 27001 checklist xls.

This implies that you once again have

#0.5 color(red)(cancel(color(black)('moles N'))) * '1 gram-atom N'_2/(1color(red)(cancel(color(black)('mole N')))) = color(darkgreen)(ul(color(black)('0.5 gram-atoms N'_2)))#

Mass Of 1 Mole Of Nitrogen Atom Is Measured

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