Mar 13, 2018  Use Avogadro's constant to easily convert one or more atoms of any element to grams. Write on a piece of paper the name of an element that interests you and the number of atoms of that element you wish to convert to grams. For example, you write 'Seven atoms of lithium.' You cannot directly convert grams to atoms. First you must covert your grams to moles, then you can take the moles and covert to atoms. If you take your 878 grams of fluorine and then look at. PRACTICE PROBLEMS: Complete grams and atoms conversions. Make sure you have this periodic table link open when answering these questions and use the conversion map if you need it. How many F atoms are in 20g of CaF 2? Answer: 3.08. 10 23 atoms F. Converting grams to moles is a problem that occurs when a measured amount of mass is known but the ratio for balanced reactions is needed. These two example problems show the best way to convert grams to moles and moles to grams of a molecule. However, these conversions are important to learn because they ultimately allow us to discover how one atom will interact with a greater number of atoms or molecules. One of the central conversion formulas is moles to grams conversion and the vice versa. Moles define the total amount of solute and grams represent the mass of an object.

• Conversion Of Atoms To Grams Weight
• Convert Number Of Atoms To Grams
• Conversion Of Atoms To Grams To Pounds
• Conversion Of Atoms To Grams 2
• Converting Atoms To Grams Worksheet

Avogadro Number Calculations II
How Many Atoms or Molecules?

The value I will use for Avogadro's Number is 6.022 x 10²³ mol¯¹.

Types of problems you might be asked look something like these:

1. 0.450 mole (or gram) of Fe contains how many atoms?
2. 0.200 mole (or gram) of H₂O contains how many molecules?

When the word gram replaces mole, you have a related set of problems which requires one more step. So keep in mind that there are 4 example problems just above.

1. Calculate the number of molecules in 1.058 mole (or gram) of H₂O
2. Calculate the number of atoms in 0.750 mole (or gram) of Fe

These problems use the reverse technique of the above. Once again, replacing mole with gram adds one step to the procedure.

Here is a graphic of the procedure steps:

Pick the box of the data you are given in the problem and follow the steps toward the box containing what you are asked for in the problem.

In example #10, I do a problem that will require three steps. The first two steps will be laid out below and I will then introduce the third step at example #10. Make sure to take a look at it.

Example #1: 0.450 mole of Fe contains how many atoms?

Solution:

Start from the box labeled 'Moles of Substance' and move (to the right) to the box labeled 'Number of Atoms or Molecules.' What do you have to do to get there? That's right - multiply by Avogadro's Number.

0.450 mol x 6.022 x 10²³ mol¯¹ =

Example #2: 0.200 mole of H₂O contains how many molecules?

Solution:

0.200 mol x 6.022 x 10²³ mol¯¹ =

The answers (including units) to the above two examples

The unit on Avogadro's Number might look a bit weird. It is mol¯¹ and you would say 'per mole' out loud. The question then is WHAT per mole?

The answer is that it depends on the problem. In the first example, I used iron, an element. Almost all elements come in the form of individual atoms, so the correct numerator with most elements is 'atoms.' (The exceptions would be the diatomic elements plus P₄ and S₈.)

So, doing the calculation and rounding off to three sig figs, we get 2.71 x 10²³ atoms. Notice 'atoms' never gets written until the end. It is assumed to be there in the case of elements. If you wrote Avogadro's Number with the unit atoms/mol in the problem, you would be correct.

The same type of discussion applies to substances which are molecular in nature, such as water. So the numerator I would use in example #2 is 'molecule' and the answer is 1.20 x 10²³ molecules.

Once again, the numerator part of Avogadro's Number depends on what is in the problem. Other possible numerators include 'formula units,' ions, or electrons. These, of course, are all specific to a given problem. When a general word is used, the most common one is 'entities,' as in 6.022 x 10²³ entities/mol.

Keep this in mind: the 'atoms' or 'molecules' part of the unit is often omitted and simply understood to be present. However, it will often show up in the answer. Like this:

So what we're going to do, we're going to work with the bolt, the green bolt in the middle of the other two elements here. Layer isolate autocad 2018.

0.450 mol x 6.022 x 10²³ mol¯¹ = 2.71 x 10²³ atoms

It's not that a mistake was made, it's that the 'atoms' part of atoms per mole was simply assumed to be there.

Example #3: 0.450 gram of Fe contains how many atoms?

Example #4: 0.200 gram of H₂O contains how many molecules?

Look at the solution steps in the image above and you'll see we have to go from grams (on the left of the image above) across to the right through moles and then to how many. So, for example #3, it would be like this:

Step One (grams ---> moles): 0.450 g divided by 55.85 g/mol = 0.0080573 mol

Step Two (moles ---> how many): 0.0080573 mol x 6.022 x 10²³ atoms/mol = 4.85 x 10²¹ atoms

and for example #4, the two steps are:

Step One: 0.200 g divided by 18.015 g/mol = 0.01110186 mol

Step Two: 0.01110186 mol times 6.022 x 10²³ molecules/mol = 6.68 x 10²¹ molecules

Example #5: Calculate the number of molecules in 1.058 mole of H₂O

Solution:

1.058 mol times 6.022 x 10²³ molecules/mol = 6.371 x 10²³ molecules

Example #6: Calculate the number of atoms in 0.750 mole of Fe

Solution:

0.750 mol times 6.022 x 10²³ atoms/mol = 4.52 x 10²³ atoms (to three sig figs)

Example #7: Calculate the number of molecules in 1.058 gram of H₂O

Solution:

(1.058 g divided by 18.015 g/mol) x 6.022 x 10²³ molecules/mole

Here is the solution set up in dimensional analysis style:

1 mol	6.022 x 1023
1.058 g x	–––––––––	x	––––––––––	= 3.537 x 1022 H2O molecules (to four sig figs)
18.015 g	1 mol
↑ grams to moles ↑		↑ moles to ↑ molecules

Example #8: Calculate the number of atoms in 0.750 gram of Fe

(0.750 gram divided by 55.85 g/mole) x 6.022 x 10²³atoms/mole

1 mol	6.022 x 1023
0.750 g x	–––––––––	x	––––––––––	= 8.09 x 1021 Fe atoms (to three sig figs)
55.85 g	1 mol

Example #9: Which contains more molecules: 10.0 grams of O₂ or 50.0 grams of iodine, I₂?

Solution:

Basically, this is just two two-step problems in one sentence. Convert each gram value to its mole equivalent. Then, multiply the mole value by Avogadro's Number. Finally, compare these last two values and pick the larger value. That is the one with more molecules.

1 mol	6.022 x 1023
10.0 g x	–––––––––	x	––––––––––	= number of O2 molecules
31.998 g	1 mol

1 mol	6.022 x 1023
50.0 g x	–––––––––	x	––––––––––	= number of I2 molecules
253.8 g	1 mol

Example #10: 18.0 g of H₂O is present. (a) How many oxygen atoms are present? (b) How many hydrogen atoms are present?

Solution:

1) Convert grams to moles:

18.0 g / 18.0 g/mol = 1.00 mol

2) Convert moles to molecules:

(1.00 mol) (6.02 x 10²³ mol¯¹) = 6.02 x 10²³ molecules

3) Determine number of atoms of oxygen present:

(6.02 x 10²³ molecules) (1 O atom / 1 H₂O molecule) = 6.02 x 10²³ O atoms

4) Determine number of atoms of hydrogen present:

(6.02 x 10²³ molecules) (2 H atoms / 1 H₂O molecule) = 1.20 x 10²⁴ H atoms (to three sig figs)

Notice that there is an additional step (as seen in step 3 for O and step 4 for H). You multiply the number of molecules times how many of that atom are present in the molecule. In one molecule of H₂O, there are 2 atoms of H and 1 atom of O.

Sometimes, you will be asked for the total atoms present in the sample. Do it this way:

(6.02 x 10²³ molecules) (3 atoms/molecule) = 1.81 x 10²⁴ atoms (to three sig figs)

The 3 represents the total atoms in one molecule of water: one O atom and two H atoms.

Bonus Example: A sample of C₃H₈ has 2.96 x 10²⁴ H atoms.

(a) How many carbon atoms does the sample contain?
(b) What is the total mass of the sample?

Solution to (a):

1) The ratio between C and H is 3 to 8, so this:

3	y
–––––––	=	––––––––––––––––
8	2.96 x 1024 H atoms

2) will tell us the number of carbon atoms present:

Conversion Of Atoms To Grams Weight

y = 1.11 x 10²⁴ carbon atoms

3) By the way, the above ratio and proportion can also be written like this:

3 is to 8 as y is to 2.96 x 10²⁴

Be sure you understand that the two different ways to present the ratio and proportion mean the same thing.

Solution to (b) using hydrogen:

1) Determine the moles of C₃H₈ present.

2.96 x 10²⁴ / 8 = 3.70 x 10²³ molecules of C₃H₈

Convert Number Of Atoms To Grams

2) Divide by Avogadro's Number:

3.70 x 10²³ / 6.022 x 10²³ mol¯¹ = 0.614414 mol <--- I'll keep some guard digits

3) Use the molar mass of C₃H₈:

0.614414 mol times 44.0962 g/mol = 27.1 g (to three sig figs)

(grams) x (6.02 x 1023) ÷ (mass number of specified element ingrams)

Find the mass of the specified element by using the atomic masson the periodic table. If it is a compound, add up the atomicmasses of each atom in the compound.

How to convert grams to atoms?

To convert grams into atoms, you have to convert them into moles first. Get the molar mass and multiply it by the number of moles to get the atoms.

Grams of mercury to Atoms of mercury?

Converting Grams into Atoms You must first convert grams into moles, then you can convert into atoms. Converting grams into moles: Grams of Mercury / 200.59 (Mass of 1 Mole of Mercury) Converting moles into atoms: Answer to the above * 6.02 x 1023 (Avogadro's Constant) Avogadro's Constant / Mole = 6.022 x 1023 Atomic Mass of Mercury = 200.59

How do you convert 2.2 grams in to atoms in nitrogen?

14 grams of nitrogen have 6.023 x 1023 atoms So 2.2 grams will have (6.023 x 1023 x 2.2)/14 = 29.15 x 1023 atoms

How do you convert from grams to atoms and from mass to atoms?

1 atomgram of a chemical element has 6,02214129(27)×1023 atoms. 1 atomgram=atomic weight of a chemical element exprimed in grams.

How do you convert grams to atoms with the avogadro's number?

(grams) x (6.02 x 10^23) / (mass number of specific element in grams)

How do you convert from mass to atoms?

To convert mass to atoms: Find the atomic mass of the element in the substance. You can find atomic masses on the periodic table. Ex. Lithium's atomic mass is 6.9 grams (round if you need to) Then find the mass of the substance in grams. Ex. you have 18.2 grams of a sample of Lithium. The mass of the sample is multiplied by 6.02 * 1023 and divided by the atomic mass. Ex. mass of…

How many Cs atoms are there in a 53.7 gram sample of Cs?

This is a two-step calculation. First convert grams Cs to moles Cs. Then convert moles Cs to atoms Cs. The atomic weight of cesium is 133 g/mol 1. To convert grams to moles: moles Cs= 53.7 g Cs1 mol = 0.404 mol Cs133 g Multiply by moles per gram. Grams cancel out. 2. To convert moles to atoms: atoms Cs = 0.404 mol Cs6.02 x 1023 atoms = 2.43E+23 atoms Csmol Multiply by atoms/mole. Moles…

How many grams are there in 2.3 x 1024 atoms of silver?

(2.3 x 1024 atoms Ag) x (1 mole Ag/ 6.022 x 1023 atoms Ag) x (107.0 g Ag/ 1 mole Ag) = 412.1056 g Ag Convert the atoms Ag to moles of silver. Then convert the moles to grams.

Conversion Of Atoms To Grams To Pounds

How do you convert moles of atoms to grams?

Multiply number of moles by the molecular mass of the element or compound

What is the mass of atoms in grams of 1.02X10 to the 24 atoms Mn?

1 mole manganese = 54.938049g 1 mole Mn atoms = 6.022 x 1023 atoms Convert atoms Mn to moles Mn. 1.02 x 1024 atoms Mn x 1mol/6.022 x 1023 atoms = 1.69mol Mn Convert moles Mn to mass in grams Mn. 1.69mol Mn x 54.938049g/mol = 92.8g

How do you convert 6.21021 uranium atoms to grams?

6.21021 uranium atoms (1mole U/6.022 X 10^23)(238.0 grams/1 mole U) = 2.45438 X 10^-21 grams of Uranium Not too massive!

How do you convert 50.0 grams into atoms?

50 grams of whatever ( 1 mole of whatever/ mass of whatever)6.022 X 10^23/1 mole whatever) = so many atoms of whatever

What is the mass in grams of 2.01 x 1022 atoms of sulfur?

Conversion Of Atoms To Grams 2

1 mole S atoms = 32.065 g S (atomic weight in grams) 1 mole S atoms = 6.022 x 1023 atoms S (Avogadro's number) Convert atoms to moles. 2.01 x 1022 atoms S x (1mol S/6.022 x 1023 atoms S) = 0.0334mol S Convert moles to mass in grams. 0.334mol S x (32.065g S/1mol S) = 10.7g S

How many dozens of copper atoms in a penny?

A penny weighs 2.5 grams and is 2.5% copper. Therefore, there is 2.5 grams × .025 = .0625 grams of copper in a penny Then you convert grams to atoms with the molecular weight of copper and Avogadro's constant .0625 grams ÷ 63.5 grams/mol × (6.02 × 1023 atoms) ÷ 12 in one dozen = 4.94 × 1019 dozens of copper atoms

How many atoms are in a sample of 85.979 g of iodine?

Converting Atoms To Grams Worksheet

1mole I atoms = 126.90447g 1 mole I atoms = 6.022 x 1023 atoms I Convert grams I to moles I 85.979g I x (1mol I/126.90447g I) = 0.67751mol I Convert moles I to atoms I 0.6775mol I x (6.022 x 1023 atoms I/1mol I) = 4.080 x 1023 atoms I

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