Balance the following reactions

 

Section #1: Simple Balancing

 

Steps for balancing:

1. Since these are written in symbol form, DO NOT mess with the subscripts.

 

2. Place Co-efficients IN FRONT of elements and/or compounds. NEVER in between compounds. Example: 2H2O is correct. H22O is not correct.)

 

3. Balance both sides so that you have the same number of elements on the reactants side as on the products side

 

1. HgO Hg + O2

2. H2 O H2 + O2

3. Al + Pb (NO3) 2 Al(NO3) 3 + Pb

4. Cu + AgNO3 Cu(NO3) 2 + Ag

5. K + H2O KOH + H2

6. MnO2 + HCl MnCl 2 + Cl2 + H2O

7. Cl2 + LiI LiCl + I2

8. F2 + H2O HF + O2

9. AgNO3 + K2SO4 Ag2SO4 +KNO3

10. Na + Cl2 NaCl

11. Br2 + H2O + SO2 HBr + H2SO4

12. CaO + H2O Ca(OH) 2

13. P2O5+ BaO Ba3(PO4) 2

14. Mg + O2 MgO

15. Fe + O2 Fe2O3

16. H2O + N2O3 HNO2

17. Na2O + H2O NaOH

18. Fe + H2O Fe3O4 + H2

 

 

 

Section #2: Names into Symbols, then balance

 

Write and Balance equations for the following chemical reactions

 

Steps for balancing:

1. Change the names into symbols.

 

2. Remember, names ending in ide are monoatomic ions. (Except for hydroxide and cyanide). Names ending in ate or ite are polyatomic ions.

 

3. Dont forget your seven diatomic atoms (H2, N2, O2, F2, Cl2, Br2, I2)

 

4. Write the oxidation numbers for each element ABOVE the element so that you can balance the charges within the compound. Remember, if an element stands alone, its oxidation number plays no role until it is combined with another element (for example, Al is +3, but when it is alone, the +3 doesnt do anything. But, when you put Al together with Cl, it becomes AlCl3).

 

5. Remember that the roman numerals tell you the POSITIVE oxidation number of the first element in the compound. Example: Copper (II) Nitrate means that copper has a +2 oxidation state. ALSO, if there is a Roman numeral but you expect the oxidation state to be different, go with the Roman numeral. Example: Nitrogen (II) Oxide. I know that you think nitrogen should be 3 from the chart, but the (II) makes it +2.

 

6. Once you have all of your subscripts in place, balance with co-efficients.

 

1. Magnesium Bromide + Chlorine Magnesium chloride + Bromine

2. Chlorine + Sodium Iodide Sodium Chloride + iodine

3. Aluminum Nitrate + Sodium Hydroxide Aluminum hydroxide + sodium nitrate

4. Sulfur trioxide sulfur dioxide + oxygen

(Sulfur trioxide is: SO3 , sulfur dioxide is: SO2)

5. Phosphoric acid + Magnesium hydroxide Magnesium phosphate + water

(Phosphoric acid is: H3PO4)

6. Ammonium nitrite nitrogen + water

(Ammonium is: NH4+ and ammonia is: NH3)

7. Ammonia + oxygen nitrogen (II) oxide + water

8. Barium Chloride + sodium sulfate sodium chloride + barium sulfate

9. Iron (III) oxide + carbon monoxide iron + carbon dioxide

10. Magnesium hydroxide + ammonium phosphate magnesium phosphate

+ ammonia + water

11. Aluminum + Copper (II) chloride aluminum chloride + copper

12. Iron + silver (I) acetate iron (II) acetate + silver

 

Section #3: Combustion Reactions

Steps for Balancing Combustion Reactions:

1. Balance the Cs and the Hs First.

 

2. Write a fraction in front of the O2 on the reactants side such that the numerator of the fraction is equal to the number of oxygens you need divided by 2. Example: For question #1, you will write 7/2O2.

 

3. Multiply the entire equation through by 2

1. C2H6 + O2 ---------- CO2 + H2O

2. C4H10 + O2 ---------- CO2 + H2O

3. C6H14 + O2 ---------- CO2 + H2O

4. C8H18 + O2 ---------- CO2 + H2O

5. C10H22 + O2 ---------- CO2 + H2O

6. CH3OH + O2 ---------- CO2 + H2O

7. C2H5OH + O2 ---------- CO2 + H2O

8. C3H7OH + O2 ---------- CO2 + H2O

9. C4H9OH + O2 ---------- CO2 + H2O

10. C5H11OH + O2 ---------- CO2 + H2O

 

Section #4: Predict the Products

Balance and predict the products

Look in your textbook (pages 256-263) for types of chemical reactions.

1. Aluminum + hydrochloric acid

2. Iron + copper (II) sulfate (iron II compound is formed).

3. Zinc (II) + sulfuric acid (sulfuric acid: H2SO4) (Zn is +2 oxidation)

4. Chlorine + magnesium iodide

5. Magnesium + hydrochloric acid

6. Magnesium + oxygen

9. Iron metal (III) + oxygen

10. Magnesium hydroxide + phosphoric acid

11. Iron (II) sulfide + hydrochloric acid

12. Ammonium sulfide + iron (II) nitrate

13. Sulfuric acid + potassium hydroxide

14. Aluminum sulfate + calcium phosphate

15. Barium carbonate + hydrochloric acid

16. Silver (I) acetate + potassium chromate

17. Ammonium phosphate + barium hydroxide

18. Chromium (III) sulfite + sulfuric acid

19. Calcium hydroxide + nitric acid (nitric acid: HNO3)