![[object Object],For every chemical reaction, the Law of Conservation of Mass must be followed. The Law of Conservation of Mass states: atoms can not be created or destroyed. Therefore, the number of atoms in the reactants must equal the number of products. Why do we need to balance a chemical equation?](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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Balancing Chemical Reactions
- 1. How to balance a chemical equation
- 3. Example of an “Unbalanced” Chemical Equation Na + Cl2 -> NaCl REACTANT SIDE Na : 1 Cl : 2 PRODUCT SIDE Na : 1 Cl : 1 NOTICE: There are TWOChlorineson the reactants side, but only ONEchlorine on the products side.
- 4. To balance a chemical equation, chemists use COEFFICIENTS. Coefficients are a small whole number that appears as a factor in front of a formula in a chemical equation. Example: N2 + 2H3-> 2NH3 WE DO NOT ADD COEFFICIENTS AND SUBSCRIPTS TOGETHER! How to “balance” a chemical equation
- 5. Example of a “Balanced” Chemical Equation Na + Cl2 -> NaCl REACTANT SIDE Na : 1 Cl : 2 PRODUCT SIDE Na : 1 Cl : 1 NOTICE: Now that we have balanced this equation using coefficients, there are TWO Clon the reactants side, and TWO Clon the products side.
- 6. The acronym MINOH makes balancing chemical reactions a little easier. TitleExamples M – Metals Fe, Na, Mg I – Ions (such as polyatomics) SO42-, PO33- N – Non-Metals Cl, Br, B O – Oxygen H – Hydrogen The acronym CHO makes combustion reactions much easier to balance. Title C – Carbon H – Hydrogen O – Oxygen The “Easy” Way to Balance
- 7. Balancing Example #2 Fe + O 2 -> Fe3O2 REACTANT SIDE Fe : 1 O : 2 PRODUCT SIDE Fe : 3 O: 2 NOTICE: Subscripts indicate how many are present to the LEFT.
- 8. Balancing Example #2 Fe + O 2 -> Fe3O2 REACTANT SIDE Fe : 1 O : 2 PRODUCT SIDE Fe : 3 O: 2 NOTICE: Now Fe and O2have the same number of atoms when they react to form Fe3O2.
- 9. Balancing Example #3 C4H8 + O2 -> CO2+ H2O REACTANT SIDE C : 4 H : 8 O :2 PRODUCT SIDE C: 1 H : 2 O: 2 + 1 = NOTICE: On the PRODUCT side, O is present in BOTH products.
- 10. Balancing Example #3 C4H8 + O2 -> CO2+ H2O REACTANT SIDE C : 4 H : 8 O :2 PRODUCT SIDE C: 1 H : 2 O: 2 + 1 = NOTICE:All atoms have the same numbers in both Products and Reactants. Coefficients Only: 1, 6, 4, 4.
- 11. Balancing Example #4 Ag2S+ KCN-> KAg(CN)2+ K2S REACTANT SIDE Ag : 2 S : 1 K : 1 CN: 2 PRODUCT SIDE Ag: 1 S : 2 K : 1 + 2 CN : 2 NOTICE:All atoms have the same numbers in both Products and Reactants. Coefficients Only: 1, 4, 2, 1.
- 12. Balancing Example #5 Hg(OH)2 + H3PO4-> Hg3(PO4)2+ HOH REACTANT SIDE Hg: 1 OH: 2 H:3 PO4: 1 PRODUCT SIDE Hg:1 OH: 1 H: 2 PO4 :2 NOTICE: All atoms have the same numbers in both Products and Reactants. Coefficients Only: 3, 2, 1, 6.
- 13. Balancing Example #6 I2 + HNO3 -> HIO3 + NO2 + H2 I: H: NO3: IO3: H: N: O: NOTICE: All atoms have the same numbers in both Products and Reactants. Coefficients Only: 1, 6, 2, 6, 3.
- 14. Balancing Example #7 C4H10 + Cl2 + O2-> CO2 + CCl4 + H2O C: H: Cl: O: C: H: Cl: O: NOTICE: All atoms have the same numbers in both Products and Reactants. Coefficients Only: 2, 8, 9, 4, 4, 10.
- 16. In-Class & Homework Assignment In-Class: Worksheet: Classification of Chemical Reactions, 1-10 by balancing the equations. Homework: Worksheet: Balancing Chemical Equations, 1-25