1. 20 Sept. 2011 Objective: You will be able to:
Review making calculations and manipulating measurements
Determine the formula for copper (II) sulfate hydrate
Homework Quiz: Week of Sept. 19
How will you know when to stop heating your copper (II) sulfate sample? Why?

2. Agenda Turn in Problem Set 2 Problem Set 1: Commonly missed questions
Finish lab procedure
Clean up
Homework:
Quiz on chapters 1-2: tomorrow
Lab notebook due Thurs.

3. Clean Up CuSO4 in trash All equipment washed and hung up to dry
Ring stands, Bunsen burners and strikers, etc. back in cabinets
Wipe down counters
Start planning out your calculations

4. Homework
Quiz on ch. 1-2 tomorrow!

5. Safety
Wear goggles until all your equipment has been cleaned and returned.
A hot crucible looks just like a cold crucible! Always use crucible tongs.
Work efficiently but carefully.

6. Technical notes
Heat the crucible uncovered or with the cover tilted to allow water vapor to escape.
Cool the crucible with the cover on.
Cool the crucible in the desiccator for very best results.
Never mass a hot or warm crucible.
Oil from your fingers will stick to the crucible and effect your data.

7. Work Ethic
Work quickly. If you have “down time,” think: “What can I do now to save time later?”
Set up data tables and calculations while you wait.

8. This period Carry out your procedure and collect data.
Begin calculations as soon as you can!
Percent of water in the hydrate by mass.
Mole ratio of anhydrous CuSO4 to H2O in your sample.
Work to show how you got your number of molecules of water of hydration.

9. Homework Ch. 2 problem set: tomorrow Quiz on chapters 1-2: tomorrow
Lab notebook due Thurs.

10. 21 September 2011 Objective: You will be able to:
show what you know about chapters 1 and 2: calculations and compounds
Do now: Questions?

11. Quiz Flip it over when you’re done.
Zero tolerance policy for disruptions.
When you finish: Work on lab calculations silently.

12. Homework Check chapter 3 summer assignment answers online: Tomorrow
Lab notebook: calculations: tomorrow

13. 22 September 2011 Take Out: Lab Notebook
Objective: You will be able to:
review Avogadro’s number, moles, molar mass, conversions, empirical and molecular formulas
Homework Quiz:
How many atoms of silver are equal to moles of silver?
Calculate the molar mass of silver nitrate. (Nitrate is NO3-)

14. Agenda
Homework Quiz
Review of Avogadro’s number, moles, molar mass, conversions, empirical and molecular formulas
Challenge problem!
Homework: p. 110 #18, 22, 26, 30, 44, 54: Mon.

18. The Mole
Atoms are so tiny; how do we quantify their masses?

19. The mole Mole: The unit for amount of substance
=6.02x1023 atoms or molecules
Avogadro’s Number = 6.02x1023
This is equal to the number of atoms of carbon in 12 grams of Carbon-12.

20. Example How many moles of helium atoms are in 6.46 g of He?
How many atoms is this?

21. Problems How many moles of magnesium are there in 87.3 g of Mg?
How many atoms is this?
Zinc is a silvery metal that is used in making brass (with copper). How many grams of Zn are in mole of Zn?

22. Sulfur is a nonmetallic element present in coal
Sulfur is a nonmetallic element present in coal. When coal is burned, sulfur is converted to sulfur dioxide and eventually to sulfuric acid that gives rise to the acid rain phenomenon. How many atoms are in 16.4 g of S?
Calculate the number of atoms in g of potassium.

23. Molar Mass The mass of a molecule. Calculate the molar mass of:
sulfur dioxide (SO2)
caffeine (C8H10N4O2)
methanol (CH4O)
SWBAT convert between grams, moles and number of particles of elements and compounds.

24. Using Molar Mass
Methane (CH4) is the principal component of natural gas. How many moles of methane are present in 6.07 g of CH4?
Calculate the number of moles of chloroform (CHCl3) in 198 g of chloroform.

25. Particles, Moles and Mass
Calculate the mass of 1.2x1024 molecules of carbon dioxide.
How many molecules of glucose are in 2.50x10-3 grams of glucose?
Calculate the mass of 1 molecule of water.
How many molecules of carbon dioxide are there in grams of carbon dioxide?
SWBAT convert between grams, moles and number of particles of elements and compounds.

26. Percent Composition by Mass
the percent by mass of each element in a compound.
Can be used to determine the purity of a substance by comparing empirical data to known composition.

27. Practice Problems
Calculate the percent by mass of each element in hydrogen peroxide.
Phosphoric acid (H3PO4) is a colorless, syrupy liquid used in detergents, fertilizers, toothpastes and in carbonated beverages for a “tangy” flavor. Calculate the percent composition by mass of H, P and O in this compound.

28. Empirical Formulas
Given the percent composition, you can determine the empirical formula of a compound (reverse of calculating percent composition)
This data is often found by experiment.

29. Practice Problems
Ascorbic acid (vitamin C) cures scurvy. It is composed of 40.92% carbon, 4.58% hydrogen and 54.50% oxygen by mass. Determine its empirical formula.
A sample of a compound contains 1.52 grams of nitrogen and 3.47 grams of oxygen. The molar mass of this compound is between 90 and 95 g. Determine its molecular formula and accurate molar mass.

30. More practice problems
Determine the empirical formula of a compound having the following percent composition by mass: K: 24.75%, Mn: %, O: 40.51%
A sample of a compound containing boron and hydrogen contains 6.444g of boron and g of hydrogen. The molar mass of the compound is about 30 g. What is its molecular formula and exact molar mass?

31. One more…
Chalcopyrite (CuFeS2) is a principal mineral of copper. Calculate the number of kilograms of copper in 3.71x103 kg of chalcopyrite.

32. Challenge!
A g sample of menthol (composed of C, H and O) is combusted, producing g of CO2 and g of H2O. What is the empirical formula? (Hint: Be aware that some oxygen in the product comes from the air, and some from the menthol!)
the compound has a molar mass of 156 g/mol what is the molecular formula?

33. Homework
p. 110 #18, 22, 26, 30, 44, 54: Mon.
Finish challenge problem

34. 26 September 2011 Objective: You will be able to:
write and balance chemical equations and calculate mole to mole and mass to mass stoichiometry.
Homework Quiz
Calculate the mass of 1 atom of palladium.
Calculate the empirical formula of a compound composed of H, O and S, which has 2.1 percent H and 65.3 percent O.

35. Agenda Homework Quiz Go over homework
Review writing and balancing equations, mole and mass stoichiometry
Practice Problems
Homework: 112 #60c, e, g, h, k and l, 64, 66, 71, 74: tomorrow
Correct Quiz for a small quiz grade: Weds.

36. Decoding Chemical Equations
2H2(g) + O2(g) → 2H2O(l)

37. Balancing Chemical Equations
Ex 1. KClO3  KCl + O2 Ex 2. C2H6 + O2  CO2 + H2O

38. Write and balance:
Ammonia gas reacts with oxygen gas to produce nitrogen monoxide gas and liquid water.
Solid lithium reacts with nitrogen gas to produce solid lithium nitride.
Nitroglycerin (C3H5N3O9) decomposes explosively to produce nitrogen gas, carbon dioxide gas, water vapor and oxygen gas.
Carbon dioxide gas reacts with potassium hydroxide to produce potassium carbonate and water vapor.

39. Mole Ratios
Coefficients indicate the number of moles (or molecules) of each compound
Ex 1. N2(g) + 3H2(g)  2NH3(g)
How many moles of hydrogen gas react with 1 mole of nitrogen gas?
How many moles of ammonia gas are produced by the reaction of 3 moles of hydrogen gas in excess nitrogen gas?

40. N2(g) + 3H2(g)  2NH3(g)
How many moles of hydrogen gas are required to react with 15 moles of nitrogen gas?
How many moles of hydrogen gas are required to produce 25.0 moles of ammonia gas?
If 10 moles of nitrogen gas was reacted with 10 moles of hydrogen gas, which would be completely reacted? Which would be excess?

41. Mass to mass stoichiometric relationships: Ex 1.
The food we eat is degraded in our bodies to provide energy for growth and function. A general equation for this very complex process is: C6H12O6 + 6O2  6CO2 + 6H2O If 856 g of C6H12O6 is consumed by a person over a certain period, what is the mass of CO2 produced?

42. Example 2
All alkali metals react with water to produce hydrogen gas and the corresponding alkali metal hydroxide. A typical reaction is that between lithium and water:
2Li(s) + 2H2O(l)  2LiOH(aq) + H2(g)
How many grams of Li are needed to produce 9.89 grams of H2?

43. Example 3 Methanol (CH3OH) burns in air according to the equation
2 CH3OH + 3O2  2CO2 + 4H2O
If 209 g of methanol are used up in the combustion process, what is the mass of H2O produced?

44. Homework
112 #60c, e, g, h, k and l, 64, 66, 71, 74

45. 27 September 2011 Objective: You will be able to:
determine which reactant is the limiting reagent and calculate percent yield.
Homework Quiz
Balance: P4O10 + H2O → H3PO4
If 10.0 grams of tetraphosphorus decaoxide is reacted with excess water, calculate the number of grams of phosphoric acid produced.
Bonus: What mass of water reacts with grams of P4O10?

46. Agenda Homework Quiz Go over homework
Review limiting reagent and percent yield
Practice Problems
Homework: p. 114 #84, 85, 89, 93, 107, 131
Correct Quiz for a small quiz grade: Weds.
Ch. 1-3 test Thursday.

47. Example 4
The reaction between nitric oxide and oxygen to form nitrogen dioxide is a key step in photochemical smog formation:
2NO(g) + O2(g)  2NO2(g)
How many grams of O2 are needed to produce 2.21 g of NO2?

48. Limiting Reagents Ex 1.
Urea is prepared by reacting ammonia with carbon dioxide:
2NH3(g) + CO2(g) (NH2)2CO(aq) + H2O(l)
In one process, g of NH3 are treated with g of CO2.
a) Which of the two reactants is the limiting reactant?
b) Calculate the mass of (NH2)2CO formed.
c) How much excess reagent (in grams) is left at the end of the reaction?

49. Example 2
The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000oC and is used in welding metals:
2Al + Fe2O3  Al2O3 + 2Fe
In one process, 124 g of Al are reacted with 601 g of Fe2O3.
a) Calculate the mass (in grams) of Al2O3 formed.
b) How much of the excess reagent is left at the end of the reaction?

50. 30 Sept. 2010
Objective: SWBAT determine limiting reagent, and calculate percent yield.
Do now:
TiCl4(g) + 2Mg(l)  Ti(s) + 2MgCl2(l)
If 3.54x107 g of TiCl4 are reacted with 1.13x107 g of Mg, calculate the limiting reagent and the theoretical yield of Ti.

51. Reaction Yield
theoretical yield: the amount of product that would result if all of the limiting reagent reacted. actual yield: amount of product actually obtained from a reaction

52. 28 September 2011
Objective: You will be able to:
practice all chapter 3 skills
Homework Quiz
P4O10 + 6H2O → 4H3PO4
In the lab, grams of tetraphosphorus decaoxide were reacted with 5.00 grams of water. Determine the number of grams of phosphoric acid produced.
If 12.5 grams of H3PO4 were produced when this reaction was performed in the lab, calculate the percent yield.

53. Agenda Homework Quiz Hand in Quiz Corrections Go over homework
Chapter 3 Problem Set
Homework: Ch. 1-3 test Tuesday (new unit starts tomorrow!)
Chapter 3 Problem Set: Tuesday

54. Percent Yield Ex 1
Titanium is a strong, lightweight, corrosion- resistant metal that is used in rockets, aircraft, jet engines and bicycle frames. It is prepared by the reaction of titanium (IV) chloride with molten magnesium between 950oC and 1150oC:
TiCl4(g) + 2Mg(l)  Ti(s) + 2MgCl2(l)
3.54x107 g of TiCl4 are reacted with 1.13x107 g of Mg. a) Calculate the theoretical yield of Ti in grams. g) Calculate the percent yield if 7.91x106 g of Ti are actually obtained.

55. Ex 2.
Industrially, vanadium metal, which is used in steel alloys, can be obtained by reacting vanadium(V) oxide with calcium at high temperatures:
5Ca + V2O5  5CaO + 2V
1.54x103 g of V2O5 is reacted with 1.96x103 g of Ca. a) Calculate the theoretical yield of V. b) Calculate the percent yield if 803 g of V are obtained.

56. On the test Classification and states of matter
Physical and chemical properties
Measurement, handling numbers
Dimensional analysis
Atomic theory and structure
Atomic number, mass number, isotopes
Molecules and Ions
Chemical formulas and names (incl. acids)
Avogadro’s number, moles, molar mass
% composition by mass
Empirical and molecular formulas
Chemical reactions and equations
Mole to Mole and Mass to Mass Stoichiometry
Limiting reagents, reaction yield

57. Review Game!
With your partner, solve the problem and show all your work.
Raise your hand when you are done.
First group with the correct answer gets the point and a chance at the bonus point.

58. An unfortunate tree is carrying on photosynthesis in the forest
An unfortunate tree is carrying on photosynthesis in the forest. One morning, it wakes up with dew on its leaves. The sunshine immediately begins to evaporate the dew. Suddenly, a storm rolls in and a giant wind knocks the tree to the ground. A limb is struck by lighting and partially burns. Over the next year, the remaining parts of the tree rot away. List all the physical changes in one column and the chemical changes in another.

59. One gallon of gasoline in an automobile’s engine produces on the average 9.5 kg of carbon dioxide. Calculate the annual production of CO2 in kilograms if there are 40 million cars in the US and each car covers a distance of 5000 mi. at a consumption rate of 20 miles per gallon.

60. A transition metal with 26 protons and 24 electrons forms a bond with a polyatomic ion consisting of phosphorus and four atoms of oxygen with a charge of 3-.
a) What type of bond holds this compound together?
b) Write the name and formula for this compound.

61. Imagine this compound contains hydrogen instead of iron.
a) What type of compound is it?
b) Write the name and formula for this compound.

62. Imagine that acid lost one oxygen
Imagine that acid lost one oxygen. Name and write the formula for the newly formed acid.

63. Calculate the molar mass of this acid, and the percent by mass of each element.

64. A compound is formed by one carbon atom and four chlorine atoms.
a) What type of bond holds these atoms together?
b) Write the name and formula of this compound.

65. Carbohydrates contain C, H and O, in which the hydrogen to oxygen ratio is 2:1. A certain carbohydrate contains 40.0% carbon by mass. Calculate the empirical and molecular formulas if the molar mass is about 178 g.

66. Lysine, an essential amino acid in the human body contains C, H, O and N. In one experiment, the complete combustion of g of lysine gave 3.94 g CO2 and g H2O. In a separate experiment, g of lysine gave g NH3. a) Calculate the empirical formula.
b) If the molar mass is about 150 g, calculate the molecular formula.

67. Hydrogen gas can be prepared by reacting propane gas (C3H8) with steam at about 400oC. The products are carbon monoxide and hydrogen gas. a) Write a balanced equation.
b) How many kilograms of hydrogen gas can be obtained from 2.84x103 kg of propane?

68. Solid elemental sulfur reacts with a solution of nitric acid to produce a solution of sulfuric acid, nitrogen dioxide gas and water. Write and balance a chemical equation.

69. When potassium cyanide reacts with acids, a deadly poisonous gas, hydrogen cyanide, is given off.
KCN(aq) + HCl(aq)  KCl(aq) + HCN(g)
If a sample of g of KCN is treated with an excess of HCl, calculate the amount of HCN formed, in grams.

70. Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide, a dark brown gas.
In one experiment, mol of nitric oxide is mixed with mol of oxygen gas. Calculate which is the limiting reagent. How many moles of nitrogen dioxide are produced?

71. When heated, lithium reacts with nitrogen to form lithium nitride.
What is the theoretical yield of lithium nitride in grams with 12.3 grams of lithium are heated with 33.6 grams of nitrogen?
If the actual yield of lithium nitride is grams, what is the percent yield?