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Visualizing a Chemical Reaction

Visualizing a Chemical Reaction. 2. 2. Na + Cl 2 NaCl. 10. 5. 10. 10. ?. 10. 5. ___ mole Na. ___ mole Cl 2. ___ mole NaCl. Formation of Ammonia. Ratio of eggs to cookies. Proportional Relationships. 2 1/4 c. flour

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Visualizing a Chemical Reaction

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  1. Visualizing a Chemical Reaction 2 2 Na + Cl2 NaCl 10 5 10 10 ? 10 5 ___ mole Na ___ mole Cl2 ___ mole NaCl

  2. Formation of Ammonia

  3. Ratio of eggs to cookies Proportional Relationships 2 1/4 c. flour 1 tsp. baking soda 1 tsp. salt 1 c. butter 3/4 c. sugar 3/4 c. brown sugar 1 tsp vanilla extract 2 eggs 2 c. chocolate chips Makes 5 dozen cookies. I have 5 eggs. How many cookies can I make? Conversion Factor 5 dozen 5 eggs 2 eggs 150 cookies = 12.5 dozen cookies Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  4. Proportional Relationships • Stoichiometry • mass relationships between substances in a chemical reaction • based on the mole ratio • Mole Ratio • indicated by coefficients in a balanced equation 2 Mg + O2 2 MgO Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  5. Stoichiometry Steps 1. Write a balanced equation. 2. Identify known & unknown. 3. Line up conversion factors. • Mole ratio - moles  moles • Molar mass - moles  grams • Molarity - moles  liters soln • Molar volume - moles  liters gas • Mole ratio - moles  moles Core step in all stoichiometry problems!! 4. Check answer. Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  6. StandardTemperature&Pressure 0°C and 1 atm Molar Volume at STP 1 mol of a gas=22.4 L at STP Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  7. Molar Volume at STP LITERS OF GAS AT STP Molar Volume (22.4 L/mol) MASS IN GRAMS NUMBER OF PARTICLES MOLES Molar Mass (g/mol) 6.02  1023 particles/mol Molarity(mol/L) LITERS OF SOLUTION Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  8. Stoichiometry Problems • How many moles of KClO3 must decompose in order to produce 9 moles of oxygen gas? 2KClO3 2KCl + 3O2 ? mol 9 mol 9 mol O2 2 mol KClO3 3 mol O2 = 6 mol KClO3 Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

  9. 1. 2 Sb + 3 Cl22 SbCl3 2. 2 Mg + O2 2 MgO 3. CaCl2 Ca + Cl2 4. 2 NaClO3 2 NaCl + 3 O2 5. Fe + 2 HCl FeCl2 + H2 6. CuO + H2 Cu + H2O 7. 2 Al + 3 H2SO4 Al2(SO4)3 + 3 H2

  10. = 2 3 5 mol x mol 1. 2 Sb + 3 Cl22 SbCl3 2 x = 15 excess 5 mol 7.5 mol excess x mol x mol x = 7. 5 mol How many moles of chlorine gas are required to react with 5 moles of antimony? 3 mol Cl2 x mol Cl2 = 5 mol Sb = 7.5 mol Cl2 2 mol Sb How many moles of SbCl3 are produced from 5 moles of antimony and excess Cl2? 2 mol SbCl3 x mol SbCl3 = 5 mol Sb = 5 mol SbCl3 2 mol Sb How many moles of SbCl3 are produced from 7.5 moles of Cl2 and excess Sb? 2 mol SbCl3 x mol SbCl3 = 7.5 mol Cl2 = 5 mol SbCl3 3 mol Cl2

  11. 2. 2 Mg + O2 2 MgO 10 mol x L x mol How many moles of magnesium oxide are produced from the burning of 10 mol of Mg? 2 mol MgO x mol MgO = 10 mol Mg = 10 mol MgO 2 mol Mg How many liters of oxygen are needed to burn 10 mol of Mg? Assume 1 mol O2 = 22.4 L 1 mol O2 22.4 L O2 x L O2 = 10 mol Mg = 5 mol O2 = 112 L O2 2 mol Mg 1 mol O2 1 mol O2 22.4 L O2 x L O2 = 10 mol Mg = 112 L O2 2 mol Mg 1 mol O2

  12. 3. CaCl2 Ca + Cl2 8 mol x mol How many moles of calcium metal are produced from the decomposition of 8 mol of calcium chloride? and chlorine gas 1 mol Ca x mol Ca = 8 mol CaCl2 = 8 mol Ca 1 mol CaCl2 How many moles of calcium metal and chlorine gas are produced from the decomposition of 8 mol of calcium chloride? 1 mol Cl2 x mol Cl2 = 8 mol CaCl2 = 8 mol Cl2 1 mol CaCl2

  13. NO31– NO31– NO31– NO31– Pb2+ Pb2+ Na1+ Na1+ I1– I1– Ions in Aqueous Solution Print Copy of Lab Pb(NO3)2(s) + H2O(l) Pb(NO3)2(aq) Pb2+(aq) + 2 NO31–(aq) add water in solution dissociation: NaI(s) + H2O(l) NaI(aq) Na1+(aq) + I1–(aq) Mix them and get… Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  14. NO31– NO31– NO31– NO31– Pb2+ Pb2+ Na1+ Na1+ Na1+ Na1+ I1– I1– I1– I1– + 2 Na1+(aq) + 2 I1–(aq) Pb2+(aq) + 2 NO31–(aq) + 2 Na1+(aq) PbI2(s) + 2 NO31–(aq) Pb2+(aq) + 2 I1–(aq) PbI2(s) Solubility Chart Mix them and get… PbI2 + NaNO3 (aq) (s) Pb(NO3)2(aq) + 2 NaI(aq) + 2 Na1+(aq) PbI2(s) + 2 NO31–(aq) solid in solution Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  15. Zn(NO3)2(aq) + Ba(OH)2(aq) + Ba2+(aq) Zn(OH)2(s) + 2 NO31–(aq) OH1– NO31– Ba2+ Zn2+ NO31– OH1– + Ba2+(aq) + 2OH1–(aq) Zn2+(aq) + 2 NO31–(aq) + Ba2+(aq) Zn(OH)2(s) + 2 NO31–(aq) Zn2+(aq) + 2 OH1–(aq) Zn(OH)2(s) Solubility Chart Mix together Zn(NO3)2(aq) and Ba(OH)2(aq): Mix them and get… Ba(NO3)2 and Zn(OH)2 (ppt) (aq) Zn(NO3)2(aq) Ba(OH)2(aq) Zn2+(aq) + 2 NO31–(aq) Ba2+(aq) + 2 OH1–(aq) Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  16. ? 6 2 3 + (NH4)3PO4 + Mg(OH)2 Mg3(PO4)2 NH4OH ammonium phosphate ammonium hydroxide magnesium phosphate magnesium hydroxide OH1- NH41+ Now you try… AlCl3 + Li2CO3  Al2(CO3)3 + LiCl 3 6 2

  17. Identify the spectator ions and write a net ionic equation when an aqueous solution of aluminum sulfate is mixed with aqueous ammonium hydroxide. Al3+ Al3+ NH41+ SO42- OH1- OH1- NH41+ SO42- aluminum aluminum sulfate + hydroxide  ammonium ammonium aluminum hydroxide + ammonium sulfate (ppt) (aq) Al2(SO4)3(aq) + 6 NH4OH(aq)  2 Al(OH)3 + 3 (NH4)2SO4 2 Al3+(aq) + 3 SO42-(aq) + 6 NH41+(aq) + 6 OH1-(aq)  2 Al(OH)3(ppt) + 6 NH41+(aq) + 3 SO42-(aq) “spectator ions” 2 Al3+(aq) + 6 OH1-(aq)  2 Al(OH)3(ppt) Net Ionic Equation

  18. Meaning of Coefficients 2 atoms Na 1 molecule Cl2 2 molecules NaCl 2 Na + Cl2 2 NaCl 2 g sodium 1 g chlorine 2 g sodium chloride + = 2 mol sodium 1 mol chlorine 2 mol sodium chloride (1 mol Cl2) x (71 g/mol) (2 mol Na) x (23 g/mol) (2 mol NaCl) x (58.5 g/mol) 117 g 46 g 71 g 117 g

  19. Classes of Reactions Chemical reactions Precipitation reactions Oxidation-Reduction Reactions Acid-Base Reactions Combustion Reactions

  20. Summary of Classes of Reactions Chemical reactions Precipitation reactions Oxidation-Reduction Reactions Acid-Base Reactions Combustion Reactions Synthesis reactions (Reactants are elements.) Decomposition reactions (Products are elements.)

  21. Summary of Classes of Reactions Chemical reactions Precipitation reactions Oxidation-Reduction Reactions Acid-Base Reactions Combustion Reactions Synthesis reactions Decomposition reactions

  22. IONIC BONDING: Formation of Magnesium Chloride Cl Cl Mg Mg2+ Cl Cl Loses 2e- Each gains 1e- One magnesium ion Two chloride ions Mg2+ Cl1- [(2+) 2 (1-) = 0] MgCl2 magnesium chloride

  23. IONIC BONDING: Formation of Magnesium Chloride Cl Cl Mg2+ Mg Mg2+ Cl Cl Loses 2e- Each gains 1e- One magnesium ion Two chloride ions Mg2+ Cl1- [(2+) 2 (1-) = 0] MgCl2 magnesium chloride

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