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Balancing Chemical Equations

Balancing Chemical Equations. CONSERVATION OF MATTER. Conservation of Matter : states that matter cannot be created or destroyed by a chemical change

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Balancing Chemical Equations

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  1. Balancing Chemical Equations

  2. CONSERVATION OF MATTER Conservation of Matter: states that matter cannot be created or destroyed by a chemical change EXAMPLE: When a log burns, the wood disappears and ashes are left. Although the ashes seem much smaller than the wooden log, the log has the same mass as the ashes. As the log burns, in addition to the ashes, water and carbon dioxide are produced. If you could find the mass of these products and add them together, you would find that they equal the mass of the original log.

  3. BALANCING CHEMCIAL EQUATIONS The amount of matter present in the products must always equal the amount of matter present in the reactants. A chemical equation shows the atoms and molecules that are involved in the reaction. When the number of atoms of each element is the same on both sides of the equation, the equation is said to be balanced. EXAMPLE: Na + Cl2 NaCl 1 atom of sodium 2 atoms of chlorine 1 atom of sodium and chlorine This is not a balanced equation because the number of atoms for each element on both sides of the arrow are not equal.

  4. Coeffiecients A coefficient has to be added in front of Na on the reactants side of the reaction and the NaCl on the products side of the reaction to balance the equation. EXAMPLE: 2Na + Cl22NaCl 2 atoms of sodium 2 atoms of chlorine 2 atoms of sodium and chlorine

  5. TO BALANCE A CHEMICAL EQUATION: 1. Write a formula equation with correct symbols and formulas. 2. Count the number of atoms of each element on each side of the arrow.

  6. 3. Balance atoms by using coefficients. (A coefficient, or whole number, is written before the formulas for reactants and products. The number shows how many molecules of a substance are involved in a chemical reaction.) 4. Check your work by counting atoms of each element.

  7. N2(g) + 3H2(g)  2NH3(g) __2___N__1_2__ 6_2___H__3_6__

  8. Zn + HCl  ZnCl2 + H2 1 Zn 1_ 1 H 2_ 1 Cl 2_

  9. Al + FeO  Al2O3 + Fe 1 Al 2_ 1 Fe 1_ 1 O 3_

  10. Al2(SO4)3 + Ca(OH)2 Al(OH)3 +CaSO4 2 Al 1_ 3 SO4 1_ 1 Ca 1_ 2_OH 3_

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