Chapter 7 Preparation
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Transcript of Chapter 7 Preparation
Chapter 7 Preparation
CHAPTER 7
Identifying Reaction Types (continued)
BLM 7.0.1
ASSESSMENT
9. Classify each of these reactions into one of the following reaction types: formation (F),single replacement (SR), simple decomposition (SD), double replacement (DR), combustion (C), or other (O).
F (a) Ti(s) + 2Cl2(g) → TiCl4(ℓ) SD (c) HCOOH(ℓ) → C(s) + H2(g) + O2(g) C (e) CH3COOH(ℓ) + 2O2(g) → 2CO2(g) + 2H2O(g)
F (g) 2C(s) + 4H2(g) + O2(g) → 2CH3OH(ℓ) SR (i) Br2(ℓ) + 2NaI(aq) → 2NaBr(aq) + I2(s) SD (k) 8H2SO4(ℓ) → 8H2(g) + S8(s) + 16O2(g)
SR (m) Sn(NO3)2 (aq) + Cd(s) → Sn(s) + Cd(NO3)2(aq) F (o) 2Ag(s) + O2(g) + H2(g) → 2AgOH(s) DR (q) H3PO4(aq) + 3NaOH(aq) → 3HOH(ℓ) + Na3PO4(aq)
DR (s) Ba(NO3)2(aq) + 2NaCl(aq) → BaCl2(s) + 2NaNO3(aq)
SR (u) I2(s) + Na2Se(aq) → 2NaI(aq) + Se(s)
F (w) 2Au(s) + 3Cl2(g) → 2AuCl3(s)
C (y) 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)
BLM 7.0.3
(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 6 6 5
1 3 2
1 2 2 2
1 5 3 4
2 2 3 2
6 16 1 1 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
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.
BLM 7.04
Supply formulas and balance
2 C5H10(l) + 15 O2(g) 10 CO2(g) + 10 H2O(g)
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)
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) + ________ →
BLM 7.0.5
Predictions: C, SD, F
2. Dihydrogen dioxide (hydrogen peroxide), H2O2(ℓ), decomposes into its elements.
Hint: determine reaction type 1st
(F)
(SD)
(C)
(C)
(C)
(F)
(C)
2 C(s) + 1 H2(g) 1 C2H2(g)
Review info about states on WS
1 H2O2(l) 1 H2(g) + 1 O2(g)
1 CH2O(l) + 1 O2(g) 1 CO2(g) + 1 H2O(g)
1 C6H12(l) + 9 O2(g) 6 CO2(g) + 6 H2O(g)
2 C6H6(l) + 15 O2(g) 12 CO2(g) + 6 H2O(g)
1 P4(s) 6 Cl2(g) 4
1 9 O2(g) 7 CO2(g) + 4 H2O(g)
BLM 7.0.6
Predictions:SR and DR
Review info about states on WS
Determine reaction type 1st
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)
1 CaCl2(aq) + 1 (NH4)2S (aq) 1 CaS(s) + 2 NH4Cl(aq)
(SR)
(DR)
(DR)
(SR)
(DR)
(SR)
(SR)
1 CH3COOH(aq) + 1 KOH(aq) 1 KCH3COO(aq) + 1 HOH(l)
1 Mg(s) + 2 AgNO3(aq) 1 Mg(NO3)2(aq) + 2 Ag(s)
1 AgNO3(aq) + 1 LiCl(aq) 1 AgCl(s) + 1 LiNO3(aq)
2 Al(s) + 3 CrSO4(aq) 1 Al2(SO4)3(aq) + 3 Cr(s)
2 Cl2(aq) + 2 Na2Se(aq) 4 NaCl(aq) + 1 Se2(s)
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 complete balanced equation or formula equation
Recall from previous unit that electrolytes dissociate (or ionize) in water
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)
• now look for spectators, chemical entities that don’t change
• cancel them out
• this leads to net ionic equation………
note that numbers from balanced equation are part of ionic equation
7.1 Reactions in Aqueous Solution
• net ionic equation:
1 Pb2+(aq) + 2 I‾(aq) 1 PbI2(s)+ 2 NO3‾(aq) + 2 K+
(aq)+ 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 ionic and net-ionic equations – note: original equation is unbalanced
7.1 Reactions in Aqueous Solution
• balanced:
• ionic:
• net ionic:
3 Ba2+(aq) + 6 ClO3‾(aq) + 6 Na+(aq) + 2 PO43‾(aq) 1 Ba3(PO4)2(s) + 6 Na+(aq) +
6 ClO3‾(aq)
3 Ba(ClO3)2(aq) + 2 Na3PO4(aq) 1 Ba3(PO4)2(s) + 6 NaClO3(aq)
3 Ba2+(aq) + 2 PO43‾(aq) 1
Ba3(PO4)2(s)
Practice Problem 2a, page 264
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)
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)
do worksheet BLM 7.1.2 questions 1-7
note that questions 3 and 7 are special – talk to me
all metal with ionic solution reactions will be similar
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
7.1 Reactions in Aqueous Solution
Thought Lab 7.1 page 2671. Red flame and ppt with
OH‾(aq): 2. Red flame and ppt with
SO42‾(aq):
3. If all traces of Ca2+(aq) and Sr2+(aq) are removed, flame colour?
solubility chart page 6 Data Booklet
also need flame test colour chart, page 6 and ion colour chart, page 11
Ca2+(aq)
Ca2+(aq), Sr2+(aq)
yellow because NaOH(aq) and Na2SO4(aq) have been added
selective precipitation – solutions are added to the unknown solution to see whether or not precipitates form
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 solutionppt with e.g.
no ppt with e.g.
blue solutionppt with e.g.
no ppt with e.g.
Worksheet BLM 7.1.5
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
concept is based on mole ratios just as # sandwiches is based on #’s of each type of piece
figure 7.7, page 271
to double # sandwiches, double # of each sandwich piece
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 ?
1
4.860.200
24.31gmol
gn mol
2
20.200 0.200
2n mol mol
? 0.200 40.31 8.06gmolm mol g
looking for
given
7.2 Stoichiometry and Quantitative Analysis
• Example: Practice Problem 15, page 278• Unbalanced equation given – balance it
• P4(s) + Cl2(g) PCl3(l)461
nm 323 g ?
n1 n2
1
3234.56
70.90gmol
gn mol
not part of molar mass
2
44.56 3.04
6n mol mol
? 3.04 137.32 417gmolm mol g
looking forgiven
Do Worksheet 30, Investigation 7.B.1
7.2 Stoichiometry and Quantitative Analysis
• Type 2: Solution Stoichiometry• Example: Practice Problem 16, page 282
based on solution concentrations and volumes, but same general strategy
1 MgCl2(aq) + 2 AgNO3(aq) 2 AgCl(s) + 1 Mg(NO3)2(aq) n1
0.30 mol/L60 mL
n2
0.50 mol/LV=?
1 0.30 0.060 0.018molLn c V L mol
0.0090
0.018 or 18 mL0.50mol
L
molV L
2
10.018 0.0090
2n mol mollooking for
given
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!
7.2 Stoichiometry and Quantitative Analysis
• Type 3: Gas Stoichiometry
• You will learn how to do this in our Gases Unit (next unit)
7.2 Stoichiometry and Quantitative Analysis