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How to Balance a Chemical Reaction

CaCl 2 (aq) + 2AgNO 3 (aq) → Ca(NO 3 ) 2 (aq) + 2AgCl(s) Ca 2+ + 2Cl - + 2Ag + + 2NO 3 - → Ca 2+ + 2NO 3 - + 2AgCl(s) 2Cl - (aq) + 2Ag + (aq) → 2AgCl(s) Ag + + Cl - → AgCl(s) H + + OH - → H 2 O 2 H + + CO 3 2- → H 2 O + CO 2 NaCl(aq)+AgNO 3 (aq)→AgCl(s)+NaNO 3 (aq)

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How to Balance a Chemical Reaction

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  1. CaCl2(aq) + 2AgNO3(aq) → Ca(NO3)2(aq) + 2AgCl(s) • Ca2+ + 2Cl- + 2Ag+ + 2NO3- → Ca2+ + 2NO3- + 2AgCl(s) • 2Cl-(aq) + 2Ag+(aq) → 2AgCl(s) • Ag+ + Cl- → AgCl(s) • H+ + OH- → H2O • 2 H+ + CO32- → H2O + CO2 • NaCl(aq)+AgNO3(aq)→AgCl(s)+NaNO3(aq) • Na + O2 → Na2O • 2Na + O2 → Na2O • 2Na + O2 → 2Na2O • 4Na + O2 → 2Na2O • P4 + O2 → 2P2O5 • P4 + 5O2 → 2P2O5 • 2Mg(s)  +  O2(g)  →    2MgO(s) • C(s)  +  O2(g)  →    CO2(g) • MgO(s)  +   H2O(l)  →    Mg(OH)2(s) • CO2(g)  +  H2O(l)  →     H2CO3(aq) • 2 Na(s)  +  Cl2(g)  →    2NaCl(s) • 2P(s)  +  3Cl2(g)  →    2PCl3(g) • N2(g)  +  3H2(g)  →    2NH3(g) • NH3(g)  +  H2O(l)  →    NH4OH(aq) • CaCO3(s)  →    CaO(s)  +  CO2(g) • Ca(OH)2(s)  →    CaO(s)  +  H2O(g) • 2KClO3(s)  →    2KCl(s)  +  3O2(g) • H2SO4  →    H2O(l)  +  SO3(g) • 2HgO(s)  →    2Hg(l)  +  O2(g) • 2NaCl(l)  →    2Na(s)  +  Cl2(g) How to Balance a Chemical Reaction By Zanman and By Kthxbie2 http://www.chem.vt.edu/RVGS/ACT/notes/Types_of_Equations.html http://en.wikipedia.org/wiki/Chemical_equation

  2. The Law of Conservation of Mass • The Law of Conservation of Mass states that matter cannot be either created or destroyed. • This means that during a chemical reaction, the amount of matter in the reactant prior to the equation will be the exact amount as the product the reaction. • So when balancing an equation, you must have the same number of the same type of atoms on either side of the reaction. http://www.800mainstreet.com/6/0006-002-balancing.html

  3. Balancing an Equation • When balancing an equation, think of a seesaw. • This is not what you want your seesaw to look like…… http://www.cagle.com/artists/Lester/LesterSamples/seesaw-01.jpg

  4. Balancing an Equation (cont.) Your seesaw should look like this. http://www.jeffmilleronline.com/images/discography/seesaw.jpg (edited with Microsoft Paint)

  5. Balancing an Equation (cont.) Here’s an example: In this equation, you will be combining aluminum and oxygen to make aluminum oxide. Al + O2 → Al2O3 1 2 2 3 There is one aluminum atom on the left and two on the right, and there are two oxygen atoms on the left and three on he right. The entire point of balancing equations is to get the same number of the same atom on each side of the equation. http://richardbowles.tripod.com/chemistry/balance.htm

  6. Balancing Equations Rules • When balancing a chemical equation you can’t destroy atoms but you can change the amount that there are on each side. • Observe as on the reactant side you only have 3 atoms in all but on the product side you have 5. • This cannot be because it is as if you are creating atoms, which is against the Law of Conservation of Mass. Al + O2 → Al2O3

  7. 1 2 2 3 • Put a two in front of the Al203 and a 3 in front of the 02 to make it so there are six oxygen atoms on each side. Al + 3O2 → 2Al2O3 4 1 6 6 Balancing the Equation (cont.) • Now lets start balancing this equation: • First choose which part to balance out first. • In this equation you should balance out the oxygen first. Al + O2 → Al2O3

  8. Al + 3O2 → 2Al2O3 • Put a four in front of the aluminum on the left side of the equation. 4Al + 3O2 → 2Al2O3 4 6 4 6 Balancing the Equation (cont.) • Now you need to balance the aluminum. • There need to be four aluminum atoms on the left side of the equation. 1 6 4 6

  9. 4Al + 3O2 → 2Al2O3 4 6 4 6 Now You’re Done!!! • Now there are four aluminum atoms and six oxygen atoms on each side of the equation so it is a balanced equation!!! http://richardbowles.tripod.com/chemistry/balance.htm

  10. Quick Notes - • The subscripts that you start with such as H2 can’t be changed which is why you have to multiply so it equals the amount of mass on the end product or reactant. • Such as (random example) • H2 + O2  H2O • You can’t substract the 2 from H2 but you can only multiply. • So 2H2 + O2 -> 2H2O Http://richardbowles.tripod.com/chemistry/balance.htm

  11. Bibliography • General Notes of G.C.S.E. and A-Level Chemistry • http://richardbowles.tripod.com/chemistry/balance.htm • Dr. Walt Volland • http://www.800mainstreet.com/6/0006-002-balancing.html

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