Warm Up 11-18-151. Which atom did Avogadro based his

experiment on?

2. How many molecules are in 1 mol of oxygen gas?

3. The molar mass of 1 CO2 compound is ___

4. What is the mass of 3 CO2 compounds?

5. Define sophmole.HomeworkNov 20 - Quiz Unit 5Nov 21 - Online HW Unit 5Dec 9 - Deadline to retake quizzes and turn in absent work

AgendaNotes Unit 5-5Group solving problemsOnline HW

Notes Unit 5-5

Moles Conversion

Bubble Diagram• Using moles to convert between mass and

the amount of atoms in a compound

Conversion Types

• Moles to grams

• Moles to atoms/molecules

• Grams to moles

• Atoms/molecules to moles

• *Grams to atoms

• *Atoms to grams

Mole to Gram Conversions

1) What is the mass of 2.5 moles of phosphorus?

• Multiple the # of moles given by the molar mass

• Example: What is the mass of 2.5 moles of phosphorus?

• Molar mass=30.97 g/mol

2.5 mol P 30.97 g P=

2.5 x 30.97 g P= 77 g P

1 mol P 1

Mole to Gram Conversions

moles A grams AMolar mass

(from periodic table)

Gram to Mole Conversions

2) How many moles are in 12 grams of FeO?

• Multiply the # of grams given by the inverse of the molar mass.

• Example: How many moles of iron are in 12 grams of iron?

12 g Fe 1 mol FeO

=

12 mol Fe

=0.169

moles Fe71.85 g Fe

71.85

Gram to Mole Conversionsgrams A moles A

Molar mass

(from periodic table)

Mole to Atoms3) How many atoms are in 3.00 moles of Na?

• Multiple the # of moles given by Avogadro’s number

• Example: How many atoms are in 3.00 moles of Na?

Mole to Atoms

3.00 mol Na6.02 x 1023 atoms Na

=

3.00 x (6.02 x 1023) atoms Na

=1.81 x 1024 atoms Na1 mol Na 1

moles A atoms AAvogadro’s Number

(6.02 x 1023 particles/mol)

Atoms to Moles4) If you have 7.45 x 1025 molecules of O2

gas, how many moles do you have?

• Multiple the # of moles given by the inverse of Avogadro’s number

• Example: If you have 7.45 x 1024 molecules of Cu, how many moles do you have?

7.45 x 1025 molecules Cu 1 mol Cu

=7.45 x 1025 mol Cu

=124 mol Cu6.02 x 1023

molecules Cu6.02 x 1023

Atoms to Molesatoms A moles A

Avogadro’s Number

(6.02 x 1023 particles/mol)

Grams to Atoms

5) How many atoms are in 26 grams of cobalt?

• 2 steps! 1st multiply by the inverse of the molar mass, 2nd multiply by Avogadro’s number

• Example: How many atoms are in 26 grams of cobalt?

26 g Co 1 mol Co 6.02 x 1023 molecules Co=

2.7 x 1023 molecules Co58.93 g Co 1 mol Co

Grams to Moles to AtomsGrams A moles A molecules A

Avogadro’s Number

(6.02 x 1023 particles/mol)

Molar mass

(from periodic table)

Atoms to Grams 6) What is the mass of 8.60 x 1023 atoms of NaCl?

• 2 steps! 1st multiply by the molar mass, 2nd multiply by the inverse of Avogadro’s number

• Example: What is the mass of 8.60 x 1023 molecules of As?

8.60 x 1023 molecules As 1 mol As 74.92 g As

= 107 g As6.02 x 1023 molecules As

1 mol As

Atoms to Moles to Grams molecules A moles A Grams A

Avogadro’s Number

(6.02 x 1023 particles/mol)

Molar mass

(from periodic table)

Group work• Work on questions #1-9 with a partner

ANSWERS:1) 1 x 103

2) 7.16 x 10-3

3) 1.67 x 10-4

4) 4.454 x 1024

5) 2.53 x 1021

6) 3.01 x 1024

7) 96 grams8) 5.778 x 10-2

9) 722.16 grams

Assignments

• Summary

• Online HW https://quest.cns.utexas.edu/