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Chapter 7 Preparation

Chapter 7 Preparation. 1 6 6 5. (a) ____C 6 H 10 O 5 (s) + ____O 2 (g) → ____CO 2 (g) + ____H 2 O(g) (c) ____Sc 2 O 3 (s) + ____H 2 O(ℓ) → ____Sc(OH) 3 (s)

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Chapter 7 Preparation

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  1. Chapter 7 Preparation

  2. 1 6 6 5 (a)____C6H10O5(s) + ____O2(g) → ____CO2(g) + ____H2O(g) (c)____Sc2O3(s) + ____H2O(ℓ) → ____Sc(OH)3(s) (e)____ CH3COOH(ℓ) + ____O2(g)→ ____CO2(g)+ ____H2O(g) (g)____C3H8(g) + ____O2(g) → ____CO2(g) + ____H2O(g) (i)____Ca(s) + ____C(s) + ____O2(g) → ____CaCO3(s) (k)____S2Cl2(ℓ) + ____NH3(g) → ____S4N4(s) + ____S8(s) + ____NH4Cl(s) (m)____Ag(s) + ____O2(g) + ____H2(g) → ____AgOH(s) (o)____CrCl2(aq)+ ____Mg(s) → ____MgCl2(aq) + _____Cr(s) (q)____C8H18(ℓ) + ____O2(g) → ____CO2(g) + ____H2O(g) (s)____Cu(s) + ____S8(s) + ____O2(g) → ____CuSO3(s) (u)____CuSO4(s) → ____Cu(s) + ____S8(s) + ____O2(g) (w)____Pb(s) + ____S8(s)+ ____O2(g)→ ____PbSO4(s) (y)____BCl3(g) + ____H2O(ℓ) → ____H3BO3(s) + ____HCl(g) 1 3 2 BLM 7.0.3 1 2 2 2 1 5 3 4 2 2 3 2 6 16 11 12 2 1 1 2 1 1 1 1 2 25 16 18 8 1 12 8 8 8 1 16 8 1 16 8 1 3 1 3

  3. 1. Cyclopentane, C5H10(ℓ), reacts with oxygen to produce carbon dioxide and water vapour.  3. Phosphoric acid is neutralized by cesium hydroxide solution to produce cesium phosphate solution and liquid water. 5. Lead(II) acetate solution reacts with zinc metal to form zinc acetate solution and solid lead. 7. Calcium chlorate solution reacts with lithium sulfate and calcium sulfate solid forms in a lithium chlorate solution.  9. Octane (C8H18(ℓ)) reacts with oxygen gas to produce carbon dioxide and liquid water in a bomb calorimeter. 2 C5H10(l) + 15 O2(g)  10 CO2(g) + 10 H2O(g) BLM 7.04 Supply formulas and balance 1 H3PO4(aq) + 3 CsOH(aq)  3 HOH(l) + 1 Cs3PO4(aq) Note: HOH(l) = H2O(l) 1 Pb(CH3COO)2(aq) + 1 Zn(s)  1 Zn(CH3COO)2(aq) + 1 Pb(s) 1 Ca(ClO3)2(aq) + 1 Li2SO4(aq)  1 CaSO4(aq) + 2 LiClO3(aq) 2 C8H18(l) + 25 O2(g)  16 CO2(g) + 18 H2O(l)

  4. (F) • 1. Ethylene (ethene), C2H2(g), forms from its elements. • 3. Methanal, CH2O(ℓ), burns in oxygen gas. • 5. Cyclohexane, C6H12(ℓ), undergoes combustion. • 7. Benzene, C6H6(ℓ), combusts. • 9. ________ + ________ → ____ PCl3(g) • 11. ____C7H8(ℓ) + ________ → 2 C(s) + 1 H2(g)  1 C2H2(g) • 2. Dihydrogen dioxide (hydrogen peroxide), H2O2(ℓ), decomposes into its elements. (SD) 1 H2O2(l)  1 H2(g) + 1 O2(g) BLM 7.0.5 Predictions: C, SD, F (C) 1 CH2O(l) + 1 O2(g)  1 CO2(g) + 1 H2O(g) (C) 1 C6H12(l) + 9 O2(g)  6 CO2(g) + 6 H2O(g) Review info about states on WS (C) 2 C6H6(l) + 15 O2(g)  12 CO2(g) + 6 H2O(g) Hint: determine reaction type 1st 1 P4(s) 6 Cl2(g) 4 (F) 1 9 O2(g) 7 CO2(g) + 4 H2O(g) (C)

  5. (SR) 1. Liquid bromine reacts with a sodium iodide solution. 3. Calcium chloride solution reacts with ammonium sulphide solution. 5. Ethanoic acid reacts with a solution of potassium hydroxide. 7. Magnesium metal is put into a silver nitrate solution. 9. Silver nitrate solution is mixed with a lithium chloride solution. 11. Aluminium metal is added to a chromium(II) sulfate solution. 13. Aqueous chlorine is mixed with a solution of sodium selenide. 1 Br2(l) + 2 NaI(aq)  2 NaBr(aq) + 1 I2(s) or (aq) BLM 7.0.6 Predictions: SR and DR (DR) 1 CaCl2(aq) + 1 (NH4)2S (aq)  1 CaS(s) + 2 NH4Cl(aq) (DR) Review info about states on WS 1 CH3COOH(aq) + 1 KOH(aq)  1 KCH3COO(aq) + 1 HOH(l) (SR) 1 Mg(s) + 2 AgNO3(aq)  1 Mg(NO3)2(aq) + 2 Ag(s) (DR) Determine reaction type 1st 1 AgNO3(aq) + 1 LiCl(aq)  1 AgCl(s) + 1 LiNO3(aq) (SR) 2 Al(s) + 3 CrSO4(aq)  1 Al2(SO4)3(aq) + 3 Cr(s) (SR) 2Cl2(aq) + 2Na2Se(aq)  4 NaCl(aq) + 1 Se2(s)

  6. Chemistry 20 Chapter 7 PowerPoint presentation by R. Schultz robert.schultz@ei.educ.ab.ca

  7. 7.1 Reactions in Aqueous Solution • Solution reaction equations are often written as net-ionic equations • Consider reaction of lead (II) nitrate solution with potassium iodide solution: 1 Pb(NO3)2(aq) + 2 KI(aq) 1 PbI2(s) + 2 KNO3(aq) equation called completebalanced equation or formula equation Recall from previous unit that electrolytes dissociate (or ionize) in water

  8. 7.1 Reactions in Aqueous Solution • leads to the ionic equation or total ionic equation • dissociate all aqueous electrolytes and write all strong acids in ionic form 1 Pb2+(aq) + 2 NO3‾(aq) + 2 K+(aq) + 2 I‾(aq) 1 PbI2(s) + 2 K+(aq) + 2 NO3‾(aq) note that numbers from balanced equation are part of ionic equation • now look for spectators, chemical entities that don’t change • cancel them out • this leads to net ionic equation………

  9. 7.1 Reactions in Aqueous Solution • net ionic equation: + 2 NO3‾(aq) + 2K+(aq) 1 Pb2+(aq) + 2 I‾(aq) 1 PbI2(s) + 2 K+(aq) + 2 NO3‾(aq) 1 Pb2+(aq) + 2 I‾(aq) 1 PbI2(s) all precipitation reactions will have this basic type of net-ionic equation try Practice Problem 2a, page 264: write ionicandnet-ionic equations – note: original equation is unbalanced

  10. 7.1 Reactions in Aqueous Solution Practice Problem 2a, page 264 • balanced: • ionic: • net ionic: 3 Ba(ClO3)2(aq) + 2 Na3PO4(aq) 1 Ba3(PO4)2(s) + 6 NaClO3(aq) 3Ba2+(aq)+6ClO3‾(aq)+6Na+(aq)+2PO43‾(aq) 1Ba3(PO4)2(s)+6Na+(aq)+6ClO3‾(aq) 3Ba2+(aq)+2PO43‾(aq) 1Ba3(PO4)2(s)

  11. 7.1 Reactions in Aqueous Solution • Single replacement example: • complete balanced equation: • ionic equation: • net-ionic equation: 1 Zn(s) + 1 Cu(NO3)2(aq) 1 Zn(NO3)2(aq) + 1 Cu(s) 1 Zn(s) + 1 Cu2+(aq) + 2 NO3‾(aq) 1 Zn2+(aq) + 2 NO3‾(aq) + 1 Cu(s) 1 Zn(s) + 1 Cu2+(aq) 1 Zn2+(aq) + 1 Cu(s) metal ions and metal elements are different! Try Practice Problem 1c, page 264 (equation is balanced)

  12. 7.1 Reactions in Aqueous Solution • ionic • net-ionic 2 Al(s) + 3 Cu2+(aq) + 6 Cl‾(aq) 3 Cu(s) + 2 Al3+(aq) + 6 Cl‾(aq) 2 Al(s) + 3 Cu2+(aq) 3 Cu(s) + 2 Al3+(aq) all metal with ionic solution reactions will be similar do worksheet BLM 7.1.2 questions 1-7 note that questions 3 and 7 are special – talk to me

  13. 7.1 Reactions in Aqueous Solution • Techniques of Qualitative Analysis • solution colour – see chart page 11 of Data Booklet • flame colour – see chart page 6 of Data Booklet: I don’t like chart titles – metals themselves don’t give colours – metal ions do what is present, nothing about amount – concentration, mass, etc

  14. 7.1 Reactions in Aqueous Solution Thought Lab 7.1 page 267 • Red flame and ppt with OH‾(aq): • Red flame and ppt with SO42‾(aq): 3. If all traces of Ca2+(aq) and Sr2+(aq) are removed, flame colour? • selective precipitation – solutions are added to the unknown solution to see whether or not precipitates form Ca2+(aq) Ca2+(aq), Sr2+(aq) solubility chart page 6 Data Booklet also need flame test colour chart, page 6 and ion colour chart, page 11 yellow because NaOH(aq) and Na2SO4(aq) have been added

  15. 7.1 Reactions in Aqueous Solution • Thought Lab 7.1, question 4a) colourless solution; no ppts • b) • c) • d) blue solution; ppt with e.g. no ppt with e.g. colourless solution ppt with e.g. no ppt with e.g. blue solution ppt with e.g. no ppt with e.g. Worksheet BLM 7.1.5

  16. 7.2 Stoichiometry and Quantitative Analysis • Stoichiometry – a method of predicting quantities of reactants or products of a chemical reaction from quantities of another substance in the reaction figure 7.7, page 271 concept is based on mole ratios just as # sandwiches is based on #’s of each type of piece to double # sandwiches, double # of each sandwich piece

  17. 7.2 Stoichiometry and Quantitative Analysis • Type 1: Gravimetric Stoichiometry • Example: Practice Problem 12, page 278 based on mass 2 Mg(s) + 1 O2(g) 2 MgO(s) n n1 n2 m 4.86 g xs ?

  18. 7.2 Stoichiometry and Quantitative Analysis • Example: Practice Problem 15, page 278 • Unbalanced equation given – balance it • P4(s) + Cl2(g) PCl3(l) 6 1 4 n n1 n2 m ? 323 g not part of molar mass Do Worksheet 30, Investigation 7.B.1

  19. 7.2 Stoichiometry and Quantitative Analysis based on solution concentrations and volumes, but same general strategy • Type 2: Solution Stoichiometry • Example: Practice Problem 16, page 282 1 MgCl2(aq) + 2 AgNO3(aq) 2 AgCl(s) + 1 Mg(NO3)2(aq) n10.30 mol/L60 mL n20.50 mol/LV=?

  20. 7.2 Stoichiometry and Quantitative Analysis • Note that in both types of stoichiometry: • step 1 is to write a balanced equation • step 2 is to convert the given quantity into moles • step 3 is to convert the moles of the given quantity into moles of the quantity you are looking for • step 4 is to convert the moles of the quantity you are looking for into the needed variable this is true in all types of stoichiometry!

  21. 7.2 Stoichiometry and Quantitative Analysis • Type 3: Gas Stoichiometry • You will learn how to do this in our Gases Unit (next unit)

  22. 7.2 Stoichiometry and Quantitative Analysis

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