The Concept of Equilibrium - Mister Chemistry · gaseous reactants the sum of the coefficients of...
Transcript of The Concept of Equilibrium - Mister Chemistry · gaseous reactants the sum of the coefficients of...
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The Concept of Equilibrium
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As the concentrations of the reactants decrease the rate of reaction in the forward direction decreases.
Reversible reactions
As the concentrations of the products increase the rate of reaction in the reverse direction increases.
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reached when rates of the forward and reverse reactions are equal and the concentrations of the reactants and products no longer change with time
Chemical equilibrium is dynamic: chemical reactions take place ,but concentrations of reactants and products remain unchanged
Chemical Equilibrium
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equilibrium constant
Consider a simple case:
Bk
Ak ʹ′
(assume single unimolecular elementary step for forward and reverse processes)
Rate of forward reaction = k [A]
Rate of backward reaction = k ʹ′ [B]At equilibrium: k [A] = k ʹ′ [B]
[B]
[A]k
k ʹ′ = K=
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The Law of Mass Action
c Ca A + b B + d D
equilibrium constant
[C]c [D]d k =
[A]a [B]b
products k =
reactants
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The NO2 - N2O4 system at 25 ° C
2NO2N2O4 (g) (g)
Init: 0.670 M 0.000 M
equil: 0.643 M 0.0547 M
4.65 x 10-3 =[NO2]2
[N2O4](0.0547) 2
0.643=
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The NO2 - N2O4 system at 25 ° C
2NO2N2O4 (g) (g)
Init: 0.500 M 0.0300 M
equil: 0. 491 M 0.0475 M
4.60 x 10-3 =(0.0475 M) 2
0. 491 M
[NO2]2
[N2O4]=
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The NO2 - N2O4 system at 25 ° C
2NO2N2O4 (g) (g)
Init: 0.000 M 0.200 M
equil: 0.0898 M 0.0204 M
[NO2]2
[N2O4]4.63 x 10-3 =
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Conc
Time
Change in concentrations
N2O4 (g) 2NO2 (g)
reactant
2N2O4 (g)
productNO2 (g)
Initially only N2O4 is present
Equilibrium concentrations
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Conc
Time
Change in concentrations
Equilibrium concentrations
reactant2N2O4 (g)
product
NO2 (g)
Initially only NO2 is present
N2O4 (g) 2NO2 (g)
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Equilibrium Can Be Reached from Either Direction
It doesn’t matter whether we start with NO2 or whether we start with N2O4, we will have the same proportions of the two substances at equilibrium.
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The magnitude of the equilibrium constant
depends on temperature
depends on reaction
3O22O3 (g) (g) K = 2.5 x 10122300°C
2ClCl2 (g) (g) K = 1.4 x 10-3825°C
H2 (g) +CO(g) + H2O (g) CO2 (g)K = 5.1
830°C
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Ways of Expressing Equilibrium Constants
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Homogeneous equilibria
Heterogeneous equilibria
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Homogeneous Equilibria
equilibrium constant can be expressed in terms of pressure or concentration
all reacting species are in the same phasegas phase
solution phase
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Example: homogeneous gas-phase
2NO2N2O4 (g) (g)
=[NO2]2
[N2O4]Kc
Where Kc is the equilibrium constant when concentrations are expressed in moles/liter
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Alternatively:
2NO2N2O4 (g) (g)
=P2 NO2
P N2O4
Kp
Where Kp is the equilibrium constant when concentrations are expressed in pressure units
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COCl2 (g)CO(g) + Cl2(g)
Practice Exercise
The equilibrium concentrations for the reaction
=[COCl2]
[CO] [Cl2]Kc
Are [CO] = 1.2 x 10-2 M, [Cl2] = 0.054 M and [COCl2] = 0.14 M. Calculate the equilibrium constant (Kc).
=0.14
(1.2 x 10-2) (0.054)= 2.2 x 102
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2NO2 (g) 2NO (g) + O2(g)
Practice Exercise
The equilibrium constant Kp for the reaction shown as 158 at 1000 K. calculate the partial pressure of O2
P(O2) = 347 atm
0.400 atm 0.270 atm ?
= P ( O2)( 0.400 )2 (158)
( 0.270 )2=
( 0.270 )2 P ( O2)
( 0.400 )2158
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Kp = Kc ( RT ) Δn
Relationship between Kp and Kc
Gas-phase concentrations can also be expressed in terms of partial pressures
PV = nRT
Therefore, =Pn
VR T
i.e.:
=P (molar concentration) R T
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Δn =
the sum of the coefficients of the gaseous reactants
the sum of the coefficients of the gaseous products
-
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Homogeneous Equilibria
equilibrium constant can be expressed in terms of pressure or concentration
all reacting species are in the same phasegas phase
solution phaseconcentration term for the solvent does not appear in the expression for the equilibrium constant
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CH3COH (aq)
O
H2O( l )+
Example: homogeneous aqueous-phase reaction
CH3CO- (aq)
O
H3O+ ( aq)+
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HOAc (aq) H2O( l )+
Example: homogeneous aqueous-phase reaction
-OAc (aq) H3O+ ( aq)+
[-OAc ] [H3O+ ] Kʹ′ =
[HOAc] [H2O]
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HOAc (aq) H2O( l )+
Example: homogeneous aqueous-phase reaction
-OAc (aq) H3O+ ( aq)+
[-OAc ] [H3O+ ] K ʹ′ [H2O] =
[HOAc]
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HOAc (aq) H2O( l )+
Example: homogeneous aqueous-phase reaction
-OAc (aq) H3O+ ( aq)+
[-OAc ] [H3O+ ] Kc =
[HOAc]
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Heterogeneous Equilibria
concentration term for solid or liquid does not appear in the expression for the equilibrium constant
all reacting species are not in the same phase
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CaOCaCO3(s) (s) + CO2(g)
= [CO2]Kc
Example
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Equilibrium29
Increasing the surface area of the solid increases the rate forward and reverse reactions equally.
CaCO3(s) CO2(g) + CaO(s)
The amount of CO2 above the solid remains the same.
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Ni Ni(CO)4 (g)(s) + 4CO (g)
Practice Exercise
What is the expression for Kc and Kp for the reaction shown
=[Ni(CO)4]
[CO]4Kc =
P(Ni(CO)4)
P 4(CO)
Kp
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NH3NH4HS (s) (g) + H2S (g)
Practice ExerciseWhat is the value for Kc and Kp for the equilibrium shown at 295 K?
= PNH3Kp PH2S
0.265atm 0.265atm
= (0 .265)2 Kp
= 0 .0702Kp
Kp = Kc ( RT ) Δn
Kc
Kp
( RT )2=
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NH3NH4HS (s) + H2S (g)
Practice ExerciseWhat is the value for Kc and Kp for the equilibrium shown at 295 K?
(g)
= PNH3Kp PH2S
0.265atm 0.265atm
= (0 .265)2 Kp
= 0 .0702Kp
Kp = Kc ( RT ) Δn
Kc
0.0702
( .0821 Latm/mol K(295K) )2=
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NH3NH4HS (s) (g) + H2S (g)
Practice ExerciseWhat is the value for Kc and Kp for the equilibrium shown at 295 K?
= PNH3Kp PH2S
0.265atm 0.265atm
= (0 .265)2 Kp
= 0 .0702Kp
Kp = Kc ( RT ) Δn
Kc = 0.00012
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Multiple Equilibria
If a reaction can be expressed as the sum of two or more individual reactions, the equilibrium constant for the overall reaction is the product of the equilibrium constants of the individual reactions.
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Multiple Equilibria
If a reaction can be expressed as the sum of two or more individual reactions, the equilibrium constant for the overall reaction is the product of the equilibrium constants of the individual reactions.
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Practice ExerciseGiven:
H+H2S (aq) (aq) + HS- (aq)
Kʹ′c = 9.5 x 10-8
K ʹ′ʹ′c = 1.0 x 10-19
H+HS- (aq) (aq) + S2-
(aq)
2H+(aq) + S2- (aq)
Calculate the equilibrium constant for:
H2S (aq)
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Practice Exercise
2H+(aq) + S2- (aq)H2S(aq)
[H+] [S2-][HS-]
H+HS- (aq) (aq) + S2-
(aq)
K =[H+]2 [S2-]
[H2S]
(aq)H+H2S (aq) + HS- (aq)
[H+] [HS-][H2S]
K = = Kʹ′c K ʹ′ʹ′c
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Practice Exercise
H+H2S (aq) (aq) + HS- (aq)
Kʹ′c = 9.5 x 10-8
K ʹ′ʹ′c = 1.0 x 10-19
H+HS- (aq) (aq) + S2-
(aq)
2H+(aq) + S2- (aq)H2S (aq)
K ʹ′ʹ′cKʹ′c (9.5 x 10-8 )(1.0 x 10-19)= = 9.5 x 10-27
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The Form of K and the Equilibrium Equation
When the equation for a reversible reaction is written in the opposite direction,the equilibrium constant becomes the reciprocal of the original equilibrium constant.
The value of K also depends on how the equilibrium constant is balanced.
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Practice Exercise
N22NH3(g) (g) + 3H2 (g)
What is the expression for Kc for:
=[NH3]2
[H2]3Kc
[N2]Kc = 1.2 at 375°C
N2 2NH3(g)(g) + 3H2 (g)
[NH3]2
[H2]3[N2] =[H2]3
( )[NH3]2
[N2]
-10.83=
= 1.2
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Practice Exercise
=[NH3]2
[H2]3Kc
[N2]Kc = 1.2 at 375°C
=[H2]3
( )[NH3]2
[N2]
1/21.1=
= 1.2
N2 2NH3(g)(g) + 3H2 (g)
What is the expression for Kc for:
N2 NH3 (g)(g) H2 (g)21 + 2
3
[H2]3/2
[NH3]
[N2]1/2
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Practice Exercise
4 moles of gases on the left; 2moles of gases on the right
Kc = 1.2 at 375°CN2 2NH3(g)(g) + 3H2 (g)
Kp = Kc ( RT )−2
Kp = 1.2[ ( 0.0821 Latm/molK )(648 K)]−2
Kp = 0.00043
What is Kp for the reaction
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Summary of Guidelines for Writing Equilibrium Constant Expressions
• The concentrations of the reacting species in solution are expressed in mol/L.
• In the gas phase, concentrations are expressed in mol/L or in atm.
Kp = Kc ( RT ) Δn
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Summary of Guidelines for Writing Equilibrium Constant Expressions
• The concentrations of pure solids, pure liquids, and solvents do not appear in the equilibrium constants expressions.
• Equilibrium constants do not have units.
• The balanced equation must be shown when the value for an equilibrium constant is given.
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Summary of Guidelines for Writing Equilibrium Constant Expressions
• If a reaction can be expressed as the sum of two or more individual reactions, the equilibrium constant for the overall reaction is the product of the equilibrium constants of the individual reactions.
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Summary of Guidelines for Writing Equilibrium Constant Expressions
• When the equation for a reversible reaction is written in the opposite direction, the equilibrium constant become the reciprocal of the original equilibrium constant .
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47
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2NH3 (g)N2 (g) + 3H2 (g)
[H2]3
[NH3] 2
[N2]
3.6 x 10^8 at 25 C