Chemical Equilibrium Chapter 18 Modern Chemistry
description
Transcript of Chemical Equilibrium Chapter 18 Modern Chemistry
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
1
ChemicalEquilibriumChapter 18
Modern ChemistrySections 1 & 2
The Nature of Chemical EquilibriumShifting Equilibrium
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
2
Shifting Equilibrium
Section 18.2
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
3
Seesaws and Equilibrium
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
4
LeChatelier’s PrincipleA play in one act.
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
5
TEACHER: “Let’s put stress on the equilibrium!”STUDENTS: “How?” (puzzled)
TEACHER: “Change the T, P, or concentration.”
LECHATELIER: “A new equilibrium will be attained.”
STUDENTS: “How?” (amazed)
TEACHER: “One of the reactions will go faster,
for a while, to relieve the stress.”
STUDENTS: “I understand.” (with confidence)
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
6
The End.
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
7
LeC
hate
lier’
s P
rin
cip
le
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
8
If a system at equilibrium is subjected to a stress, the equilibrium is shifted in the direction that tends to relieve the stress…and a new equilibrium is achieved.
LeChatelier’s Principle
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
9
Changing the concentration Adding a reactant or product Removing a reactant or product
Changing the temperature. Changing the pressure
How is a system “stressed”?
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
10
Affects only eq. with gases Increasing the pressure favors the side
with the fewest particles Leading to a decrease in pressure
Decreasing the pressure favors the side with the most particles Leading to an increase in pressure
If particle are equal, pressure has no effect.
Increasing pressure by adding a gas that is not a reactant or a product cannot affect the eq.
Changes in Pressure
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
11
2NO2 (g) N2O4 (g) + Energy
O2 (g) + 2SO2 (g) + Energy 2SO3 (g)
N2 (g) + 3 H2 (g) 2NH3 (g) + Energy
2HI (g) + Energy H2 (g) + I2 (g)
O2 (g) + N2 (g) 2NO2 (g) Keq = 4.5 x 10-31 at 25 ° C Keq = 6.7 x 10-10 at 627 °C
Balanced Equation
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
12
Central Metal Surrounded by
ligands Examples of
ligands H2O NH3
CN1-
Cl1-
Complex Ions
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
13
Increase the concentration of reactants the forward reaction is favored
Increase the concentration of products the reverse reaction is favored
Up, Up and AwayUp, Up and Away
Take Away TowardsTake Away Towards
Changes in Concentration
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
14
[Cu(H2O)4 ] 2+ + 4Cl1- [CuCl4]2- + 4H2O
Complex Cu Ion System
1.Increase Cl1-
2.Shift is forward
3.Products increase, reactants decrease
4.The Keq is the same – before and after
AWAYUP, UP
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
15
[Cu(H2O)4 ] 2+ + 4Cl1- [CuCl4]2- + 4H2O
Complex Cu Ion System
1.Increase H2O
2.Shift is reverse
3.Reactants increase, products decrease
4.The Keq is the same – before & after
AWAY UP, UP
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
16
[CoCl4]2- + 6H2O [Co(H2O)6]2+ + 4Cl-
Complex Co Ion System
1.Decrease H2O
2.Shift is reverse
3.Reactants increase, products decrease
4.The Keq is the same – before & after
TOWARDS
TAKE AWAY
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
17
2NO2 (g) N2O4 (g) + Energy
O2 (g) + 2SO2 (g) + Energy 2SO3 (g)
N2 (g) + 3 H2 (g) 2NH3 (g) + Energy
2HI (g) + Energy H2 (g) + I2 (g)
O2 (g) + N2 (g) 2NO2 (g) Keq = 4.5 x 10-31 at 25 ° C Keq = 6.7 x 10-10 at 627 °C
Balanced Equation
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
18
2NO2 (g) N2O4 (g) + Energy In a reversible reaction one direction is
exothermic and the other direction is endothermic.
In the reaction above which direction is exothermic?
forward endothermic?
reverse
Changes in Temperature
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
19
2NO2 (g) N2O4 (g) + Energy Increasing the energy favors the endothermic
reaction Decreasing the energy favors the exothermic
reaction Keq is dependant on temperature A change in temp, changes the Keq.
Changes in Temperature
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
20
Equilibrium Constants Table
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
21
NO2 N2O4 System
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
22
2NO2 (g) N2O4 (g) + Energy
NO2 N2O4 System
1.Increase Energy (temperature)
2.Shift is reverse
3.Products decrease, reactants increase
4.The Keq is decreasing
AWAYUP, UP
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
23
2NO2 (g) N2O4 (g) + Energy
NO2 N2O4 System
1.Decrease Energy (temperature)
2.Shift is forward
3.Products increase, reactants decrease
4.The Keq is increasing
TOWARDS TAKE AWAY
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
24
Changes in Temperature
engine runningstoring energythat is taken in
engine not runningusing energy that isgiven off
Pb(s) + PbO(s) + 2H2SO4(aq) 2PbSO4(s) + 2H2O(l) + E
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
25
2NO2 (g) N2O4 (g) + Energy
O2 (g) + 2SO2 (g) + Energy 2SO3 (g)
N2 (g) + 3 H2 (g) 2NH3 (g) + Energy
2HI (g) + Energy H2 (g) + I2 (g)
O2 (g) + N2 (g) 2NO2 (g) Keq = 4.5 x 10-31 at 25 ° C Keq = 6.7 x 10-10 at 627 °C
Balanced Equation
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
26
Eff
ect
of
T,
P &
Con
c
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
27
CO2(g) CO2(aq) H2CO3(aq) H+ + HCO3- (aq)
H+ + CO3-2
(aq) + Ca2+ CaCO3(s)
Chickens Lose Equilibrium
EGGSHELL
CHICKENBREATH
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
28
If a product leaves the system the reaction will not reverse. It will go to completion.
Formation of a gas. H2CO3 (aq) H2O(l) + CO2(g)
Formation of a precipitate. Na+
(aq)+Cl−(aq)+Ag+(aq)+NO3−
(aq) Na+(aq)+NO3−
(aq)+AgCl (s)
Reactions that go to completion
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
29
Com
mon
Ion
Eff
ect
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
30
The addition of HCl caused the NaCl to increase and precipitate out of solution.
Common-ion Effect - the addition of an ion common to two solutes brings about precipitation or reduced ionization.
Common Ion Effect
HCl (g) H+(aq) + Cl−(aq)
AWAYUP, UP
NaCl (s) Na+(aq) + Cl−(aq)
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
31
Adding acetate ion from the dissociation of sodium acetate causes a reverse shift.
Ionization is reduced. [H3O] is reduced.
Common Ion EffectNaC2H3O2 Na+ + C2H3O2
-
AWAY UP, UPHC2H3O2 (aq)H2O(l) H3O
(aq)C2H3O2−
(aq)
Chapter 18 Section 2 Shifting Equilibrium p. 598-604
32
Ch 18 Sec 2 Homework
LeChatelier’s Principle Worksheet