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. Don’t 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 doesn’t 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 C’s and the H’s First.

2. Write a fraction in front of the O₂ on the reactant’s side such that the numerator of the fraction is equal to the number of oxygen’s 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 ----------à CO₂ + H₂O

2. C₄H₁₀ + O₂ ----------à CO₂ + H₂O

3. C₆H₁₄ + O₂ ----------à CO₂ + H₂O

4. C₈H₁₈ + O₂ ----------à CO₂ + H₂O

5. C₁₀H₂₂ + O₂ ----------à CO₂ + H₂O

6. CH₃OH + O₂ ----------à CO₂ + H₂O

7. C₂H₅OH + O₂ ----------à CO₂ + H₂O

8. C₃H₇OH + O₂ ----------à CO₂ + H₂O

9. C₄H₉OH + O₂ ----------à CO₂ + H₂O

10. C₅H₁₁OH + O₂ ----------à 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)