1. Stoichiometry
Lesson # 1

2. Stoichiometry: the relationship between the amount of reactants used in a chemical reaction and the amounts of products produced by the reaction

3. Coefficients in a Reaction Equation:
2Mg + O2 → 2MgO
the coefficient 2, means two magnesium atoms react with one oxygen molecule to produce two molecules of magnesium oxide
if you double the amounts of Mg and O2, what will happen to the amount of MgO???
if you use 10 times the amount of reactants, what will happen to the amount of MgO???

4. *the balanced equation describes the ratio in which the substances combine
In terms of MOLES: (remember 1 mole =6.02x1023 molecules)
2(6.02 x 1023)Mg + (6.02 x 1023)O2 → 2(6.02 x 1023)MgO
2 mol Mg mol O2 → 2 mol MgO
The ratio Mg = mol Mg
O mol O2

5. Balanced chemical equations can be used to relate the amounts of reactants and products in chemical reactions.
2Fe2O3 + 3C → 4Fe + 3CO2
The coefficients mean that 2 moles of Fe2O3 react with 3 moles of C to produce 4 moles of Fe and 3 moles of CO2.
The coefficients are a chemical recipe that describes the exact amounts of reactants required to make exact amounts of products in moles.

6. So, how do we relate these amounts of moles to determine the relationship.
THE MOLE BRIDGE!!
It is the MOLE that allows us to compare the amounts (grams) or Atoms required or produced in the reaction.

7. 1. How many grams of Fe2O3 are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g

8. 1. How many grams Fe2O3 of are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g
105 g Fe

9. 1. How many grams Fe2O3 of are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g
105 g Fe x 1 mole
55.8 g

10. 1. How many grams Fe2O3 of are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g
105 g Fe x 1 mole x mole Fe2O3
55.8 g 4 mole Fe

11. 1. How many grams Fe2O3 of are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g
105 g Fe x 1 mole x mole Fe2O3 x g
55.8 g 4 mole Fe mole

12. 1. How many grams Fe2O3 of are required to produce 105 g of Fe?
2Fe2O3 + 3C → 4Fe + 3CO2
?g g
105 g Fe x 1 mole x mole Fe2O3 x g = g
55.8 g 4 mole Fe 1 mole

13. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g

14. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g
155 g Fe2O3

15. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g
155 g Fe2O3 x 1 mole
159.6 g

16. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g
155 g Fe2O3 x 1 mole x 3 mole C
159.6 g 2 mole Fe2O3

17. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g
155 g Fe2O3 x 1 mole x 3 mole C x g
159.6 g 2 mole Fe2O3 1 mole

18. 2. How many grams of C are require to consume 155 g of Fe2O3?
2Fe2O3 + 3C → 4Fe + 3CO2
155g ? g
155 g Fe2O3 x 1 mole x 3 mole C x g = g
159.6 g 2 mole Fe2O3 1 mole

19. 3. How many grams of Al2(CO3)3 are produced by the complete
3. How many grams of Al2(CO3)3 are produced by the complete reaction of 452 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
452 g ? g

20. 3. How many grams of Al2(CO3)3 are produced by the complete
3. How many grams of Al2(CO3)3 are produced by the complete reaction of 452 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3 2
452 g ? g
452 g Al(NO3)3

21. 3. How many grams of Al2(CO3)3 are produced by the complete
3. How many grams of Al2(CO3)3 are produced by the complete reaction of 452 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3 2
452 g ? g
452 g Al(NO3)3 x 1 mole
213.0 g

22. 3. How many grams of Al2(CO3)3 are produced by the complete
3. How many grams of Al2(CO3)3 are produced by the complete reaction of 452 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3 2
452 g ? g
452 g Al(NO3)3 x 1 mole x 1 mole Al2(CO3)3
213.0 g 2 mole Al(NO3)3

23. 3. How many grams of Al2(CO3)3 are produced by the complete
3. How many grams of Al2(CO3)3 are produced by the complete reaction of 452 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3 2
452 g ? g
452 g Al(NO3)3 x 1 mole x 1 mole Al2(CO3)3 x g = g
213.0 g 2 mole Al(NO3)3 1 mole

24. 4. How many moles of Na2CO3 are required to completely
4. How many moles of Na2CO3 are required to completely consume 152 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
152 g ? moles

25. 4. How many moles of Na2CO3 are required to completely
4. How many moles of Na2CO3 are required to completely consume 152 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
152 g ? moles
152 g Al(NO3)3

26. 4. How many moles of Na2CO3 are required to completely
4. How many moles of Na2CO3 are required to completely consume 152 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
152 g ? moles
152 g Al(NO3)3 x 1 mole
213.0 g

27. 4. How many moles of Na2CO3 are required to completely
4. How many moles of Na2CO3 are required to completely consume 152 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
152 g ? moles
152 g Al(NO3)3 x 1 mole x 3 mole Na2CO3
213.0 g 2 mole Al(NO3)3

28. 4. How many moles of Na2CO3 are required to completely
4. How many moles of Na2CO3 are required to completely consume 152 g of Al(NO3)3?
2Al(NO3) Na2CO3 → Al2(CO3) NaNO3
152 g ? moles
152 g Al(NO3)3 x 1 mole x 3 mole Na2CO3 = moles
213.0 g 2 mole Al(NO3)3

29. Molar Volume
of a Gas at
STP
Lesson # 2

30. The molar volume of any gas at STP standard temperature (0 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.

31. The molar volume of any gas at STP standard temperature (25 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs

32. The molar volume of any gas at STP standard temperature (25 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs x kg
2.21 lbs

33. The molar volume of any gas at STP standard temperature (25 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs x kg x g
2.21 lbs kg

34. The molar volume of any gas at STP standard temperature (0 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs x kg x g x 1 mole
2.21 lbs kg g

35. The molar volume of any gas at STP standard temperature (0 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs x kg x g x 1 mole x L
2.21 lbs kg g mole

36. The molar volume of any gas at STP standard temperature (0 0C) and pressure (101kPa) is 22.4 L.
Molar Volume is 22.4 L
1 mole memorize!
1. Calculate the volume of 10.0 lbs of CO2 at STP.
10.0 lbs x kg x g x 1 mole x L = x 103 L
2.21 lbs kg g mole

37. 2. Calculate the volume of O2 gas produced at STP for the
2. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO.
2HgO → 2Hg + O2
12.5 g ? L
12.5 g HgO

38. 2. Calculate the volume of O2 gas produced at STP for the
2. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO.
2HgO → 2Hg + O2
12.5 g ? L
12.5 g HgO x 1mole
216.6g

39. 2. Calculate the volume of O2 gas produced at STP for the
2. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO.
2HgO → 2Hg + O2
12.5 g ? L
12.5 g HgO x 1mole x 1 mole O2
216.6g mole HgO

40. 2. Calculate the volume of O2 gas produced at STP for the
2. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO.
2HgO → 2Hg + O2
12.5 g ? L
12.5 g HgO x 1mole x 1 mole O x L
216.6g mole HgO mole

41. 2. Calculate the volume of O2 gas produced at STP for the
2. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO.
2HgO → 2Hg + O2
12.5 g ? L
12.5 g HgO x 1mole x 1 mole O x L = L
216.6g mole HgO mole

42. g of a common diatomic gas occupies 8.50 L at STP. Calculate the molar mass of the gas and determine the gas.
8.50 L x 1 mole = moles
22.4 L
Molar Mass = grams
moles
= g = 28.0 g/mole
moles
The gas is N2