1. Bell Work 1 / Balancing Equations
Balance the following equations: first do an Atom Count, Determine the type of reaction, then balance.
1. _____ Na + _____ O2 --> _____ Na2O2
2. _____ Ag2O --> _____ Ag + _____ O2
3. _____ Ba(OH)2 + _____ H3PO4 --> _____ BaHPO4 + _____ H2O
4. _____ C3H8 + _____ O2 --> _____ CO2 + H2O
5. _____ Al + _____ HCl --> _____ AlCl3 + _____ H2

2. Bell Work 2 / Balancing and Type

3. Bell Work 3 / Stoichiometry Road Map
Draw the stoichiometry road map and include all the mathematical relationships that exist.

4. Single Displacement Reactions
Bell Work 4 / Predicting
Single Displacement Reactions
Use the activity series from your resource packet to write a balanced chemical reaction for each of these single replacement reactions.
1. Au + KNO3 →
2. Zn + AgNO3 →
3. Al + H2SO4 →
4. Cu + H2O →
5. Zn H2SO4 

5. Single Displacement Reactions
Bell Work 5 / Predicting
Single Displacement Reactions
Chlorine gas is bubbled through a solution of sodium bromide.
____Cl ___NaBr →
1. What type of reaction is this?
a. single replacement b. double replacement c. synthesis d. decomposition e. combustion
2. What product(s) will be predicted for this reaction? (Bubble the 2 that apply)
a. no products form b. Na c. Br d. NaCl e. Br2
3. Which set of coefficients correctly balances it?
a) 1, 2, 2, 1 b) 1, 1, 1, 1 c) 3, 1, 3, 1 d) 2, 1, 2, 1
4. How many Liter of Chlorine gas will be consumed if you start with liters of sodium bromide at STP.

6. Bell Work 6 / Stoichiometry
1. What mass of glucose can be produced from a photosynthesis reaction that occurs using 10.0 mol CO2 ?
CO2 + H2O → C6H12O O2
2. How many moles of mercury (II) oxide, HgO , are needed to produce 125 grams of oxygen gas?
___HgO → ___O ___Hg

7. Bell Work 6 / Stoichiometry
1. What mass of glucose can be produced from a photosynthesis reaction that
occurs using 10.0 mol CO2 ?
6CO H2O → C6H12O O2
10 mol CO2 x 1 mol C6H12O6 x g = g C6H12O6
6 mol CO mol   
2. How many moles of mercury (II) oxide, HgO , are needed to produce 125 grams of oxygen gas?
__2_HgO → ___O _2__Hg
  125 g O2 x 1 mole O2 x 1 mol HgO = mol HgO
1 mol HgO g

8. Bell Work 7 / Stoichiometry % mass
1. If we mix 25 grams of sodium bromide with a large amount of potassium chloride, what will our theoretical yield of sodium chloride be in grams? Start by writing the BALANCED chemical equation. ____NaBr + ___KCl → ____NaCl + ____KBr 2) If our actual yield from this reaction was 12.6 grams of sodium chloride, what would our percent yield for this reaction be?

9. AgNO3 + ZnCl2  AgCl + Zn(NO3)2
Bell Work 7 / Precipitates
1. Predict, on the basis of the solubility rules, which of the following salts are soluble and which are insoluble. 
        
a.   AgI                                    c.   BaSO4                                  e.   NiCO3
    
b.   Na3PO4                            d.   (NH4)2SO4                            f.    Cu(OH)2
2. If you start with 6.54 grams of zinc chloride.
AgNO ZnCl2  AgCl Zn(NO3)2
1. Balance the Equation.
2. What type of reaction?
3. Use your solubility rules and determine the precipitates if any!
4. Write the complete ionic equation.
5. Write the net ionic equation.
6. How many moles of the precipitate are formed?

10. AgNO3 + ZnCl2  AgCl + Zn(NO3)2
Bell Work 7 / Precipitates
1. Predict, on the basis of the solubility rules, which of the following salts are soluble and which are insoluble. 
        
a.   AgI                                    c.   BaSO4                                  e.   NiCO3
    
b.   Na3PO4                            d.   (NH4)2SO4                            f.    Cu(OH)2
2. If you start with 6.54 grams of zinc chloride.
AgNO ZnCl2  AgCl Zn(NO3)2
1. Balance the Equation.
2. What type of reaction?
3. Use your solubility rules and determine the precipitates if any!
4. Write the complete ionic equation.
5. Write the net ionic equation.
6. How many moles of the precipitate are formed?

11. Bell Work 8 / Net Ionic Equation
_____ Al + _____ HCl --> _____ AlCl3 + _____ H2
Balance the equation
2. What type of reaction is this?
3. Use your solubility rule to determine if there are any precipitants.
4. Write the Complete Ionic Equation.
5. Write the Net Ionic Equation

12. Bell Work 9 / How to Make a Dilution
If you have a stock solution of 6.25 M NaCl How much would you need to use to make 250 mL of M NaCl?
Describe how you would make this dilution in the Lab.( hint use the following: graduated cylinder, graduated flask, stock solution, distilled water)

13. Bell Work 7 / Solution
Define the following:
solute
solvent
saturated
unsaturated
super saturated
How do the following affect the solubility?
Pressure is increased
Temperature is increased
Solids and Liquids
Gases

14. Bell Work 3 / Decomposition and Stoichiometry
1. Decomposition of potassium chlorate
___KClO3 → ___KCl + ___O2
I. Balanced equation
2. Stoichiometry: How many grams of oxygen are produced in the decomposition of 5.00 g potassium chlorate?

15. Bell Work 3 / Decomposition and Stoichiometry
1. Decomposition of potassium chlorate
___KClO3 → ___KCl + ___O2
I. Balanced equation
  1. 2_KClO3 → _2_KCl + _3_O2
2. Stoichiometry: How many grams of oxygen are produced in the decomposition of 5.00 g potassium chlorate?
5.00 g KClO3 x 1 mole x 3 moles O2 x g O2 = g O2
122.6 g moles KClO mole

16. Bell Work Percent Yield Calculations
1) Balance this equation and state which of the six types of reaction is taking place:
____ Mg + ____ HNO3  ____ Mg(NO3)2 + ____ H2
Type of reaction: __________________________
2) If I start this reaction with grams of magnesium and an excess of nitric acid, what is the theoretical yield of hydrogen gas in grams that will produced?
3) If 1.7 grams of hydrogen is recovered through gravimetric analysis, what is my percent yield of hydrogen?

17. Bell Work 9 / The Mole
Find the empirical formula of a compound that is 48.38% carbon, 8.12% hydrogen, and 53.5% oxygen by mass.

18. Bell Work 10 / Molarity
Determine the molarity of a solution made by dissolving 20.0 g of NaOH in sufficient water to yield a 482 mL of solution.

19. Bell Work 12 / Characteristics of Acid and Base

20. Bell Work 13 / Acid Base Titration
mL of M HCl reacts with 30.0 mL of KOH solution of unknown concentration.
mL of M NaOH reacts with 22.5 mL of HC2H3O2 solution of unknown concentration.

21. Bell Work 2 / balancing Equations
1. _____ Na + _____ O2 --> _____ Na2O2
2. _____ Ag2O --> _____ Ag + _____ O2
3. _____ Ba(OH)2 + _____ H3PO4 --> _____ BaHPO4 + _____ H2O
4. _____ C3H8 + _____ O2 --> _____ CO2 + H2O
5. _____ Al + _____ HCl --> _____ AlCl3 + _____ H2