1. be taken to the post-quiz.
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2. One mole of solid sulfur (an element) contains 6.022 x 1023 atoms.
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One mole of
solid  sulfur
(an element)
contains
6.022 x 1023
atoms.

3. One mole of liquid bromine (a compound)
contains
6.022 x 1023
molecules.

4. One mole of gaseous carbon dioxide (a compound) contains 6.022 x 1023
molecules.
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5. One mole solid SULFUR mass 32.066 g
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One mole solid
SULFUR
mass g

6. One mole liquid
BROMINE
mass g

7. One mole gaseous CARBON DIOXIDE
mass g
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8. approximate volume at room temperature and pressure 16 cm3
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One mole solid
SULFUR
approximate volume at room temperature and pressure 16 cm3

9. One mole liquid
BROMINE
approximate
volume at room
temperature and pressure 51 cm3

10. One mole gaseous CARBON DIOXIDE
approximate volume at room temperature and pressure 20,000 cm3 
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11. One mole of sulfur atoms
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ONE SULFUR ATOM
formula S atomic weight
32.066
One mole of sulfur atoms
mass g

12. ONE BROMINE
MOLECULE formula Br2 atomic weight
molecular weight
One mole bromine
molecules
mass g

13. MOLECULE formula CO2 atomic weights
ONE CARBON
DIOXIDE
MOLECULE formula CO2 atomic weights
carbon
oxygen molecular weight
44.010
One mole carbon
dioxide molecules
mass g
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14. 1. Convert 30 g carbon to moles.
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1. Convert 30 g carbon to moles.

15. C, atomic weight
1 mole C
( g)
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16. mass (g) carbon  moles carbon
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(Convert 30 g C to mol.)
mass (g) carbon  moles carbon
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17. 1 12.011 mole C g C _________ 30 g C x 30 mole C 12.011 = 2.5 mol C
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(Convert 30 g C to mol.)
mole C
g C
_________
30 g C x
30 mole C
12.011
= 2.5 mol C
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18. 2. Convert 3.5 liters of ammonia at S.T.P. to moles.  

19. 1 mole gaseous ammonia, NH3; volume 22.414 liters at S.T.P.
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(Convert 3.5 L NH3 at S.T.P. to mol.)
1 mole gaseous ammonia, NH3; volume liters at S.T.P.

20. volume (L) ammonia  moles ammonia
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(Convert 3.5 L NH3 at S.T.P. to mol.)
volume (L) ammonia 
moles ammonia
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21. 1 22.414 mol NH3 L NH3 ___________ 3.5 L NH3 x 3.5 mol NH3 22.414
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(Convert 3.5 L NH3 at S.T.P. to mol.) 1
22.414
mol NH3
L NH3
___________
3.5 L NH3 x
mol NH3
22.414
= 0.16 mol NH3
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22. 3. How many moles of glucose are in 10 mL of a 0
3. How many moles of glucose are in 10 mL of a 0.5 molar aqueous solution?

23. 0.5 moles/liter glucose in solution of
(# mol glucose in 10 mL 0.5 M soln?)
0.5 moles/liter glucose in solution of
10 mL

24. volume (mL) solution  volume (L) solution  moles solvent
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(# mol glucose in 10 mL 0.5 M soln?)
volume (mL) solution  volume (L) solution  moles solvent
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25. 1 1000 or 10 mL solution x 1 L 103 mL ______ L mL 10 mL solution x or
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(# mol glucose in 10 mL 0.5 M soln?) 1
1000 or
10 mL solution x L
103 mL
______ L mL
10 mL solution x or
10 mL solution x L
1 mL
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26. or or 10 mL solution x 1 L 1000 mL x mol glucose L solution 0.5 1
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(# mol glucose in 10 mL 0.5 M soln?)
10 mL solution x L
1000 mL
x mol glucose
L solution
0.5 1 or
x mol glucose
L solution
0.5 1
10 mL solution x L
103 mL or
10 mL solution x L mL
x mol glucose
L solution
0.5 1
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27. or 10 mL solution x 1 L x 0.5 mol glucose 1000 mL 1 L solution
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(# mol glucose in 10 mL 0.5 M soln?)
10 mL solution x L x 0.5 mol glucose
1000 mL L solution or
10 mL solution x L x 0.5 mol glucose mL L solution
10 mL solution x L x mol glucose mL L solution
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28. 10 x 0.5 mol glucose 1000 or 103 10 x 10-3 x 0.5 mol glucose
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(# mol glucose in 10 mL 0.5 M soln?)
10 x 0.5 mol glucose
1000 or
103
10 x 10-3 x 0.5 mol glucose
= or 5 x 10-3 mol glucose
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29. 4. How many atoms are
present in 4.0 moles of phosphine, PH3? 

30. (# atoms in 4.0 mol PH3?) H P
phosphine molecules

31. moles phosphine  molecules phosphine  atoms
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(# atoms in 4.0 mol PH3?)
moles phosphine  molecules phosphine  atoms
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32. _____________________ molecules PH3 mol PH3
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(# atoms in 4.0 mol PH3?)
4.0 mol PH3 x
6.02 x 1023 1
_____________________
molecules PH mol PH3
x atoms
molecule PH3
4 1
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33. 4.0 x 6.02 x 1023 x 4 atoms = 9.6 x 1024 atoms ___________________
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(# atoms in 4.0 mol PH3?)
4.0 mol PH3 x 6.02 x molecules PH3
mol PH3
x atoms
1 molecules PH3
___________________
4.0 x 6.02 x 1023 x 4 atoms
= 9.6 x atoms
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34. 5. How many electrons are lost by ionization of 0.65 moles of calcium?

35. (# electrons lost by 0.65 mol Ca?)
+ +
+ e
+ +
+ e
+ +
+ e e e e
+ +
+ e e
+ +
+ e e
+ +
+ e
+ +
+ e e e e e
+ +
+ e + e
+ +
+ e + e

36. moles calcium  atoms calcium  electrons
(# electrons lost by 0.65 mol Ca?)
moles calcium  atoms calcium  electrons
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37. 6.02 x 1023 2 1 1 atoms Ca mol Ca __________________ 0.65 mol Ca x
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(# electrons lost by 0.65 mol Ca?)
6.02 x 1023 1
atoms Ca
mol Ca
__________________
0.65 mol Ca x
x electrons atoms Ca 2 1
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38. 0.65 mol Ca x 6.02 x 1023 atoms Ca 1 mol Ca x 2 electrons 1 atoms Ca
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(# electrons lost by 0.65 mol Ca?)
0.65 mol Ca x x 1023 atoms Ca mol Ca x 2 electrons atoms Ca
0.65 x 6.02 x 1023 x 2 electrons
= 7.8 x 1023 electrons
END OF TUTORIAL
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