2. The following problems refer to FeSO4.
Is the compound ionic or molecular? How do you know?
Calculate the oxidation state of the iron.
Write the proper name of the compound.
Calculate the oxidation state of the sulfur in the SO42- ion.
Write the reaction that would occur between FeSO4 and NaCl.
Calculate how many moles of NaCl are needed to react with 15.4 moles of FeSO4.

3. Reaction Stoich. What coefficients mean: 2 Na + Cl2  2NaCl

4. Reaction Stoichiometry
2 Na + Cl2  2NaCl
6 moles Na
10 atoms Na
ONLY WORKS FOR
MOLES, MOLECULES, ATOMS

5. 1. How many moles of H2 and O2 must react to form 6 moles of H2O?
2. How many moles of water must react with 0.25 moles of CaC2?
CaC H2O  C2H2 + Ca(OH)2

6. 3. How many moles of KCl and O2 are formed from the decomposition of 6 moles of KClO3?
4. How many grams of oxygen are needed to react with 4.41 g of Li to form Li2O? (Ans: g)

7. 5. How many grams of oxygen are needed to react with 17. 5 g of Al
5. How many grams of oxygen are needed to react with 17.5 g of Al? (Ans: 15.6)
Al + O2  Al2O3
6. How many grams of oxygen will react with 25.0 g of C2H6? (Ans: g)
C2H O2  CO H2O

8. 7. How many grams of P4 and O2 are needed to make 3. 62 g of P2O5
7. How many grams of P4 and O2 are needed to make 3.62 g of P2O5? (Ans: g, 2.04 g)
P O2  P2O5

9. Calculate the mass of aluminum required to produce 750. 0 g of iron
Calculate the mass of aluminum required to produce g of iron. Also calculate the formula units of Fe2O3 that are used in the process.
Al Fe2O3  Al2O Fe
363 g Al, 4.05 X 1024

10. What mass of oxygen is needed to react with 16
What mass of oxygen is needed to react with 16.7 g of iron to form Iron(III)oxide? How many molecules of O2 are used?
4Fe + 3O2  2Fe2O3
Ans: g, 1.35 X 1023 atoms

11. Lead(II)Nitrate reacts with potassium iodide to form potassium nitrate and lead(II)iodide.
Write the balanced reaction
What type of reaction is this?
Calculate the grams of potassium nitrate formed from the reaction of 18.0 g of lead(II)nitrate.
Calculate atoms of iodine in the lead(II) iodide

12. Limiting Reactant Sandwich analogy: 14 slices of bread
4 pieces of turkey (low fat)
Maximum # of sandwiches?
2. Limiting Reactant – Totally consumed in a reaction. No leftovers

13. How many grams of H2SO4 can be formed from the rxn of 5
How many grams of H2SO4 can be formed from the rxn of 5.00 moles of SO3 and 2.00 moles of H2O?
SO3 + H2O  H2SO4
(Ans: 196 g)

14. 2. How many grams of H2O can be formed from the rxn of 6
2. How many grams of H2O can be formed from the rxn of 6.00 moles of H2 and 4.00 moles of O2?
O2 + H2  H2O

15. 3. How many grams of NaCl can be formed from the reaction of 0
3. How many grams of NaCl can be formed from the reaction of mol of Na and mol of Cl2? (Ans: 11.7 g)
2Na + Cl2  2NaCl

16. 4. How many grams of Ag can be formed from the rxn of 2
4. How many grams of Ag can be formed from the rxn of 2.00 g of Zn and 2.50 g of silver nitrate? How much excess reactant remains?
Zn + AgNO3  Ag + Zn(NO3)2
(Ans: g Ag, g xs zinc)

17. 5. How many grams of Ag2S can be formed from the rxn of 15
5. How many grams of Ag2S can be formed from the rxn of 15.6 g of Ag and 2.97 g of H2S? (Assume O2 is in excess)
4Ag + 2H2S + O2  2Ag2S + 2H2O
(Ans: 18.0 g)

18. 6. How many grams of CO2 can be formed from the rxn of 40
6. How many grams of CO2 can be formed from the rxn of 40.0 g of CH3OH and 46.0 g of O2?
2CH3OH O2  2CO2 + 4H2O
(Ans: 42.2 g)

19. Na3PO4 + Ba(NO3)2  Ba3(PO4)2 + NaNO3
How many grams of Ba3(PO4)2 can be formed from the rxn of 3.50 g of Na3PO4 and 6.40 g of Ba(NO3)2? (Ans: 4.92 g)
Na3PO Ba(NO3)2  Ba3(PO4)2 + NaNO3

20. Percent Yield
Formula:
Actual Yield X 100 = % Yield
Theoretical Yield

21. What is the % yield if you start with 10. 00 grams of C and obtain 1
What is the % yield if you start with grams of C and obtain 1.49 g of H2 gas?
C + H2O  CO + H2
(Ans: 89.2%)

22. Carbon was heated strongly in sulfur(S8) to form carbon disulfide
Carbon was heated strongly in sulfur(S8) to form carbon disulfide. What is the percent yield if you start with g of sulfur and collect 12.5 g of CS2?
4C + S8  4CS2
(Ans: 78.0%)

23. An aluminum ladder oxidizes according the following unbalanced equation:
Al + O2  Al2O3
100.0 grams of aluminum reacted with excess oxygen. Calculate the theoretical yield. (189 g)
If the percent yield was 67.4%, calculate the actual yield. (127 g)
Calculate how many grams of oxygen were used. (88.9 g)
Identify the type of reaction that occurred.

24. 11. 5 grams of sodium reacts with 15
11.5 grams of sodium reacts with 15.0 grams of chlorine (Cl2) to form sodium chloride grams of NaCl are collected.
Write the balanced chemical equation.
Identify the limiting reactant.
Calculate the theoretical yield of NaCl. (24.7g)
Calculate the percent yield. (73.7%)
If the percent yield for a different trial (starting with same amounts) was only 60.4%, calculate the actual yield.
Identify the type of reaction that occurred.

25. Molarity 1. Molarity = measure of the concentration of a solution
2. Molarity = moles/liter
Similar to Density = g/L

26. Molarity
3. Which is more concentrated?
1 M HCl 3 M HCl

27. Molarity
1. What is the molarity of a soln that contains g of H2SO4 in enough water to make mL of soln? (Ans: M)
2. What is the molarity of a soln made by dissolving 23.4 g of Na2SO4 in enough water to make 125 mL of soln? (Ans: M)

28. Molarity
3. What mass of HCl is present in 155 mL of M HCl? (Ans: g)
4. How many grams of NaOH are in 5.00 mL of M NaOH? (Ans: g)

29. Molarity
5. What volume of M NaOH is needed to provide moles? (Ans: mL)
6. What volume of M HCl is needed to provide g of HCl?(Ans: 25 mL)

30. Mixing From a Solid 1. Mixing from a solid
2. How would you prepare mL of M Na2SO4?

32. Mixing From a Solid
3. Write directions for the preparation of mL of M KMnO4 (10.5g)
4. Write directions for the preparation of mL of M NaOH (0.02 g)

33. Diluting from a Solution
1. Dilution Formula:
M1V1 = M2V2
2. Used when you are starting with a more concentrated soln. (Grape juice concentrate, Coke syrup)

34. Diluting from a Solution
3. What is the molarity of a soln of KCl that is prepared by diluting 855 mL of M soln to a volume of 1.25 L? (Ans: M)
4. You have a 3.00 L bottle of 11.3 M HCl. What volume of it must be diluted to make 1.00 L of M HCl? (Ans: mL)

35. The following questions refer to a 0.0987 M solution of NaNO3.
Calculate how many grams of NaNO3 are present in 50.0 mL of the solution. (0.419 g)
Calculate the volume of the solution required to provide grams of NaNO3. (22.4 mL)
State how you would prepare mL of the solution starting with solid NaNO3. (4.19 g)
State how you would prepare mL of the solution starting with a large 3-L bottle of 2.00 M NaNO3(aq) (24.7 mL)

36. 1) Mass 4.19 g of NaNO3
2) Place in a small volume of water to dissolve
3) Dilute to 500 mL
1) Measure 24.7 mL of M NaNO3
2) Dilute to 500 mL

37. The following questions refer to this equation:
H2SO4 + NaOH  H2O + Na2SO4
Calculate how many moles of NaOH are present in 25.0 mL of M NaOH.
Calculate how many grams of Na2SO4 are produced if the 25.0 mL of M NaOH reacts.
Calculate the moles of H2SO4 that would be required.
Calculate the volume of H2SO4 required if the concentration is M.
State what type of reaction occurred.

38. The following questions refer to the following unbalanced reaction of ethanol (C2H5OH )
C2H5OH + O2  CO2 + H2O
State what type of reaction is occurring.
Calculate the grams of oxygen needed to react with grams of ethanol.
Calculate the number of CO2 molecules produced.
The density of ethanol g/cm3. Calculate the volume of ethanol needed to provide grams.

39. a) mol b) mol
a) g b) g c) g
a) g b) mol c) 279 g
d) g e) 175 g
363 g Fe, 4.05 X 1024 Fe2O3
g Cu
323 g Cl2
a) mol b) mol c) 2.81 mol
d) mol
39.4 g
g CO2, 10.4 g HCl

40. 47.0%
13.8 g
16.4 g g L M L mL

41. Sodium bicarbonate (NaHCO3) was decomposed to compare the actual mass of sodium carbonate (Na2CO3) to the theoretical mass. About two grams of NaHCO3 was placed in a petri dish. The dish was heated on a hotplate, allowed to cool, and then massed. The theoretical mass of Na2CO3 was calculated from the chemical equation and compared to the actual mass. This experiment was accurate, with a percent error of 5.3%. The experiment was not precise because it produced a range of 0.80 grams in the actual mass of Na2CO3.

42. 1 2 3 4 5 6 7 8 9 10 C D B A 11 12 13 14 15
4. Na2S(s)  2Na+(aq) + S2-(aq)

43. Lab Notes
Goggles
Use aluminum pans instead of petri dishes
4 trials total – Mark your dishes
Wash dishes out at end and leave all materials at station
BE CLEANER ABOUT THE BALANCE!!!!!
Ignore back of sheet, use AP lab report format
All work must be unique