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Chemical equations
Chemical equations
Chemical equations
Chemical equations
Chemical equations
Chemical equations
Chemical equations
Chemical equations
Chemical equations
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Chemical equations

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  • 1. Chemical Equations 6CO 2 + 6H 2 O Carbon Dioxide + Water (yields) Glucose + Oxygen + Energy C 6 H 12 O 6 + 6O 2 + Energy Light
  • 2. Goals: <ul><li>To learn how to balance chemical equations </li></ul><ul><li>To understand the Law of Conservation of Mass. </li></ul>
  • 3. Describing Chemical Reactions <ul><li>Cellular phone messages make use of symbols and abbreviations to express ideas in shorter form. Similarly, chemists often use chemical equations in place of words. </li></ul>
  • 4. Chemical Equations <ul><li>What does the information from the first slide represent? </li></ul>C 6 H 12 O 6 + 6O 2 + Energy Light 6CO 2 + 6H 2 O The substances that undergo a change are called the REACTANTS. They are written before the “yields” arrows. The new substances that are formed are called the PRODUCTS and are written after the arrows.
  • 5. Practice <ul><li>Write a chemical equation showing the formation of carbon dioxide from carbon and oxygen. </li></ul><ul><li>Write a chemical equation showing the formation of water from hydrogen and oxygen. </li></ul><ul><li>Write a chemical equation showing the formation of table salt from sodium and chlorine. </li></ul>
  • 6. Conservation of Mass <ul><li>Created by Antoine Lavoisier, this law states that: </li></ul><ul><li>mass is neither created nor destroyed in a chemical reaction. </li></ul><ul><li>the total mass of the products must always equal the total mass of the reactants. </li></ul><ul><li>the total number of atoms on one side of the equation MUST equal the total number of atoms on the other side. </li></ul>
  • 7. Conservation of Mass <ul><li>The principle of conservation of mass states that in a chemical reaction, the total mass of the reactants must equal the total mass of the products. </li></ul>
  • 8. Balancing Chemical Equations <ul><li>Magnesium metal (Mg) reacts with oxygen gas (O 2 ), forming magnesium oxide (MgO). To write a balanced equation for this reaction, first write the equation using the formulas of the reactants and products, then count the number of atoms of each element. </li></ul><ul><li>Balance all C-H-O elements 1 st . The remaining elements will usually balance themselves after. </li></ul>
  • 9. Practice <ul><li>The Burning of Hydrazine Balance the equation and then explain: </li></ul><ul><li>N 2 H 4 + O 2 = N 2 + H 2 O </li></ul><ul><li>What are the reactants? </li></ul><ul><li>What are the products? </li></ul><ul><li>How many molecules of each element or compound are needed for this reaction to take place? </li></ul>

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