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The Mole Concept

The document discusses the mole concept and mole calculations. It explains that a mole is 6.02 x 1023 particles of a substance and that the formula mass in grams of a substance is equal to 1 mole. It provides examples of mole conversion problems involving grams to moles, moles to molecules/atoms, and vice versa. Finally, it provides practice problems for students to set up mole calculations using factor-label methods.

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Jay Dans
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183 views2 pages

The Mole Concept

The document discusses the mole concept and mole calculations. It explains that a mole is 6.02 x 1023 particles of a substance and that the formula mass in grams of a substance is equal to 1 mole. It provides examples of mole conversion problems involving grams to moles, moles to molecules/atoms, and vice versa. Finally, it provides practice problems for students to set up mole calculations using factor-label methods.

Uploaded by

Jay Dans
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as DOC, PDF, TXT or read online on Scribd
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The Mole Concept:

   
There will be a formal test before Lab Day. You will demonstrate on this test that you can
convert grams to moles, moles to molecules, and molecules to grams. Your paper periodic table
and a "hand-held" calculator may be used during the test, but nothing else.
A Mole Is:
23
 6.02 x 10 of anything.
 The formula mass in grams of a substance contains one
mole of particles.

 Na = Avogadroës Number = 6.02 x 1023

The mole is important because:


 It allows us to weigh atoms in the lab.

 It allows us to compare amounts of atoms in chemical reactions.

Basic mole calculations: convert mass to moles, and moles to molecules or atoms.

The following equalities are used in mole calculations:

1 mole = 6.02 x 1023 atoms or molecules = formula mass in


grams
 
Examples of Mole Conversion Problems:

These problems are set up correctly using Factor Label. Use a calculator to find each answer with
the proper number of significant digits.

1. Given 12.011 grams of carbon, how many atoms do you have?

2. Given 18 grams of water, how many molecules do you have?


3. Given 3.5 moles of sodium chloride, how many grams do you have?

4. What is the mass of 6.02 x 1023 molecules of silver nitrate?

Setting up the factor-label problem is just as important as the answer.

Form the habit of working neatly, canceling units, and circling the answer.

Remember, units are just as important as numbers in the answer.

Mole Calculation Practice Problems.


Show the factor-label calculation used to work each problem.
1. What is the mass in grams of 0.452 mole of C6H12O6?
2. Calculate the mass in kilograms of 0.681 mole of ammonia gas,
NH3.
3. Determine the number of potassium ions in 3.05 mole of K+.
4. How many molecules are in 39.0 grams of Fe2S3?
5. Calculate the mass in grams of 2.23 moles of nitrogen
molecules.
6. How many atoms are in 6.4 grams of copper?
7. A raindrop contains about 0.05 grams of water.
a. How many molecules of water are in a raindrop?
b. How many atoms of hydrogen are in a raindrop?

c. How many atoms of oxygen are in a raindrop?

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