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Chemical Equations & Reactions: Understanding Atom Counting

Learn how to balance chemical equations, count atoms, and predict products in reactions. Discover the types of reactions, catalysis, and the law of conservation. Practice with examples and solve missing reactant or product problems.

josephnicholas
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Chemical Equations & Reactions: Understanding Atom Counting

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  1. Chapter 8Chemical equations & Reactions Finding (Counting) the numbers of atoms or moles of atoms in a compound (NH4)2SO4 N= S= H= O= Total Number of atoms=

  2. Now put a Coefficient in front of that compound4(NH4)2SO4 N= S= H= O= Total Number of atoms=Mg3(PO4)2 Mg= P= O=3Mg3(PO4)2 Mg= P= O=

  3. Try TheseH2SO45 H2SO4(NH4)3PO44(NH4)3PO4Al(NO3)33 Al(NO3)3

  4. Hydrates can be Troublesome!CuSO4*5H2O4 CuSO4*5H2O6CaCl2*5H2O

  5. I. Chemical Equations: show the chemical formulas and the amounts of reactants & products. Show phases in chemical rxn! s,l,g,aq preciptate

  6. Law of Conservation of Matter, Mass, Energy and Charge all apply to chemical equations. None are created nor destroyed, just rearrangedReactants=Products Review endo A + B + Energy C exo A + B C + energy B. coefficients”# in front of formula that tells the #of molecules, moles, atoms or formula units(ionic) taking part in rxn. Ex: 2H2 + O2 2H2O sum of coefficients= ___molecules(moles) of hydrogen and ___molecules(moles) of oxygen yield/makes___molecules(moles) of water

  7. II. A Is the equation Balanced? Yes or Norules: 1. List all atoms 2. Count atoms on both the reactant and product side Ex: 2Na + 2H2O  2NaOH + H2

  8. Zn + 2HCl  ZnCl2 + H2

  9. B. Writing chemical Equations from word equations1. Write formulae(remember diatomics)2.Determine coefficients to balance equationsHint: Table K /L for acids and bases Chlorine + Sodium Bromide  Bromine + Sodium Chloride

  10. Aluminum + oxygen  aluminum oxide

  11. Aluminum sulfate + calcium chloride  aluminum chloride + calcium sulfate

  12. 1A. 5NH3 N=5 H=15 B. Ca(OH)2 Ca=1 O=2 H=2 C. 3BaSO4*5H2O Ba=3 S=3 O= 12 + 15 =27 H=30 D. 6Na(C2H3)4 Na=6 C=48 H=72 2. Silicon tetrachloride(g) + magnesium(s) silicon(s)+ magnesium chloride (s) 3A Yes Zn + 2HCl  ZnCl2 + H2

  13. B. No H2SO4 + 2NaOH  H2O + Na2SO4 c. No Pb(NO3)2+ 2NaI  PbI2 + NaNO3 D. No Na + O2 Na2O E. No Cu + S  Cu2S F. Yes CuO + H2 Cu + H2O G. Yes Ba(OH)2 + CO2 BaCO3 + H2O

  14. 1a Ok Zn + H2SO4 ZnSO4 + H2 b. 2K + Br2 2KBr c. 2 H2O  O2 +2 H2 d. Cl2 + 2KI  2KCl + I2 e. Ok HNO3 + LiOH  H2O + LiNO3 • 2 N2 + O2 2 N2O • Ok NH4Cl + NaOH NH4OH + NaCl

  15. 2a Na(s) + I2(S) NaI(s) 2Na(s) + I2(S)2 NaI(s) B. Zn(s) + HBr(aq)  ZnBr2(s) + H2(g) Zn(s) + 2HBr(aq)  ZnBr2(s) + H2(g) C. KOH(s)  K2O(s) + H2O(l) 2KOH(s)  K2O(s) + H2O(l)

  16. D Mg(s) + H2O(l)  Mg(OH)2(aq) + H2(g) Mg(s) + 2H2O(l)  Mg(OH)2(aq) + H2(g)

  17. pg3 1.A Ca + O2  CaO 1B. 2Ca + O2 2 CaO 2A H2O  H2 + O2 2B 2 H2O  2H2 + O2 3A. Br2 + NaCl  NaBr + Cl2 3B Br2 + 2NaCl  2NaBr + Cl2 4A. Mg + FeCl3  MgCl2 + Fe 4B. 3Mg + 2FeCl3 3 MgCl2 + 2Fe

  18. 5A. KOH + AlI3  KI + Al(OH)3 5B 3 KOH + AlI3  3KI + Al(OH)3 6A. FeCl2 + BaSO4  FeSO4 + BaCl2 6B. FeCl2 + BaSO4  FeSO4 + BaCl2 7A. Al2S3 + LiNO3  Al(NO3)3 + Li2S 7B Al2S3 + 6LiNO3 2 Al(NO3)3 +3 Li2S

  19. III. Types of Reactions • Synthesis (Direct Combination)- put together Ex. A+B C Element + Element  Compound C + E  C

  20. B. Decomposition (Analysis)- to break apart( Most require a catalyst (speeds up the rate of rxn without being altered or changed) • Name 3 catalysts • . Heat • Electricity • Chemicals • Catalyst can be placed above arrow • Ex ABA+B C E +E

  21. p. 27822a sodium + oxygen  sodium oxide 4Na + O2  2Na2O22b. Magnesium + fluorine  magnesium fluoride Mg + F2  MgF2

  22. 23A. 2HgO  2Hg + O223B 2 H2O  2H2 + O223C 2Ag2O  4Ag + O223D. CuCl2  Cu + Cl2

  23. 38 A potassium + chlorine  potassium chloride 2K + Cl2  2KCl38B hydrogen + iodine  hydrogen iodide H2 + I2  2HI38C magnesium + oxygen  magnesium oxide 2Mg + O2  2MgO

  24. C. Single Replacement-one element switches or cuts in Ex. Metals (cations) C + AB CB + A m only replace m Nonmetals(anions) C + AB AC + B nm only replace nm E + C  E + C

  25. Will SR occur? Use Table Jelement that is coming in must be higher on the chart than element in compound Cr + FeSO4 Zn + AgNO3 

  26. Cl2 + NaF F2 + NaI--->

  27. D. Double Replacement -2 elements switch or cut in What drives DR? Must form water, gas ppt(s ) AB + CD  AD + CB C + C C + C Ex. AgNO3 + NaCl  AgCl + NaNO3

  28. p. 27935a Ni + CuCl2 NiCl2 + Cu35b Zn + Pb(NO3)2  Zn(NO3)2 + Pb35c. Cl2 + 2KI 2KCl + I235d no rxn35e Ba + 2H2O  H2 + Ba(OH)2

  29. 36a 2Ca + O2 2CaO36b. 2Ni + O2  2NiO36 c no rxn

  30. p. 27825a AgNO3 + NaCl  NaNO3 + AgCl25b. Mg(NO3)2 + 2KOH  Mg(OH)2 + 2KNO325c 3LiOH + Fe(NO3)3  3LiNO3 + Fe(OH)3

  31. IV. Missing Reactant or product • List atoms 2. Find what is not equal Ex: 2Na + 2H2O  X + 2NaOH

  32. CaCO3 CaO + ________________

  33. 2Al + _______  2AlCl3 + 3H2

  34. V. Determine Missing Mass Law of Conservation of Mass: Total mass of reactants = total mass of products Ex#1 If 103.0g of potassium chlorate are decomposed to form 62.7g of potassium chloride and oxygen gas according to the equation, how many grams of oxygen are formed? 2KClO3 2KCl + 3O2

  35. Ex#2 Reactant (s) Product(s)Magnesium + Oxygen  Magnesium Oxide ? g + 16.0g  40.3gBased on the Law of Conservation of Mass predict the minimum amount of magnesium that will react with 16.0g of oxygen to produce 40.3 g of magnesium oxide.

  36. Ex#3Reactant(s) Product(s)Magnesium + Oxygen  Magnesium Oxide 12.2g + 8.0g  ?gAssuming that magnesium and oxygen will react completely with one another, predict the mass of magnesium oxide that will be produced.

  37. Ex#4 Reactant(s) Product(s)Magnesium + Oxygen  Magnesium Oxide + Oxygen 48.6g + 50.0g  80.6g + ?gPredict the mass of oxygen that will be left over after the reaction of 48.6 grams of magnesium with 50.0 g of oxygen

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