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Balancing Equations

Balancing Equations. Balancing, Writing, and Naming Equations. Warm Up 10/2. Please get your Science Scoring Log out and be prepared to update it (on back of Unit 1 Packet) Cross off 1-E1 from Assignment list and add Law of Conservation of Mass Lab in its place. Balancing Equations.

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Balancing Equations

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  1. Balancing Equations Balancing, Writing, and Naming Equations

  2. Warm Up 10/2 Please get your Science Scoring Log out and be prepared to update it (on back of Unit 1 Packet) Cross off 1-E1 from Assignment list and add Law of Conservation of Mass Lab in its place.

  3. Balancing Equations

  4. Balancing Equations • Law of Conservation of Matter: • In a chemical reaction, matter can be neither created nor destroyed. • In a chemical reaction, the amount of reactants equals the amount of products.

  5. Balancing Equations • Also known as: • Law of Conservation of Atoms: • The number of atoms of each type of element must be the same on each side of the equation.

  6. Balancing Equations Hydrogen + oxygen water H2 + O2 H2O • Hydrogen and oxygen are diatomic elements (won’t exist alone!). • Their subscripts cannot be changed. • The subscripts on water cannot be changed. • Can only add coefficients until balanced

  7. Balancing Equation Steps 1. First, identify the reactant side and the product side. 2. Draw a line coming down from the yield sign (arrow) 3. List the elements on each side of the arrow 4. Count the elements on each side of the arrow 5. Begin balancing (might have to go back and forth a few times until everything is balanced!)

  8. Balancing Equation Steps H2 + O2 H2O 1. Count the atoms on each side and ALWAYS write it out like this: ReactantSideProduct Side H=2 H=2 O=2 O=1

  9. Balancing Equations H2 + O2 H2O • If the subscripts cannot be altered, how can the atoms be made equal? • Adjust the number of molecules by changing the coefficients.

  10. Balancing Equations H2 + O22H2O ReactantSideProduct Side H=2 H=4 O=2 O=2 • H is no longer balanced.

  11. Balancing Equations 2H2 + O22H2O ReactantSideProduct Side H=4 H=4 O=2 O=2 • It is now balanced because the proper amounts of coefficients were added!

  12. Balancing Equations N2 + H2 NH3 Nitrogen + hydrogen ammonia ReactantSideProduct Side N=2 N=1 H=2 H=3

  13. Balancing Equations • Nothing is balanced. • Balance the nitrogen first by placing a coefficient of 2 in front of the NH3. N2 + H22NH3 ReactantSideProduct Side N=2 N=1 2 H=2 H=3 6

  14. Balancing Equations • Hydrogen is not balanced. • Place a 3 in front of H2 N2 + 3H22NH3 ReactantSideProduct Side N=2 N=1 2 H=2 6 H=3 6

  15. What about Polyatomic Ions? -Follow the same steps as normal EXCEPT, do NOT break apart the polyatomic ions! ReactantSideProduct Side Ca= 3 Ca= 1 PO4= 2 PO4= 1 H= 2 H= 3 SO4= 1 SO4= 1 Ca3(PO4)2 + H2SO4 CaSO4 + H3PO4

  16. Balancing Equations Balance the metal first by placing a coefficient of 3 in front of CaSO4. Ca3(PO4)2 + H2SO4 CaSO4 + H3PO4 Ca3(PO4)2 + H2SO43CaSO4 + H3PO4 ReactantSideProduct Side Ca= 3 Ca= 1 3 PO4= 2 PO4= 1 H= 2 H= 3 SO4= 1 SO4= 1 3

  17. Balancing Equations • Next, balance the ion groups • Last, balance the rest of the atoms Ca3(PO4)2 + 3H2SO43CaSO4 + H3PO4 3 sulfate groups are needed on the reactant side so place a coefficient of 3 in front of H2SO4.

  18. Balancing Equations Ca3(PO4)2 + 3H2SO43CaSO4 + H3PO4 ReactantSideProduct Side Ca= 3 Ca= 1 3 PO4= 2 PO4= 1 H= 2 6 H= 3 SO4= 1 3 SO4= 1 3 Neither H nor PO4 is balanced!

  19. Balancing Equations A coefficient of 2 placed in front of H3PO4 balances both hydrogen and phosphate. Congratulations! You are now finished!!! Ca3(PO4)2 + 3H2SO43CaSO4 + 2H3PO4

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