chapter 15
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Chapter 15. Chemical equilibria. Closed vial of NO 2 : NO 2 (g) + NO 2 (g) N 2 O 4 (g) brown colorless Brown color becomes less intense, then, after some time period, color change stops. Concentrations of products and reactants remain constant with time (equilibrium) - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 15
Chemical equilibria
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Chemical Equilibrium Closed vial of NO2:
NO2(g) + NO2(g) N2O4(g)
brown colorless Brown color becomes less intense, then, after some time
period, color change stops.
Concentrations of products and reactants remain constant with time (equilibrium)
Applies to all reactions
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Dynamic EquilibriumH2O(g) + CO(g) H2(g) + CO2(g)
Start off with closed flask of CO and H2O. Equilibrium sets up (chemical reaction occurring).
What happens to amounts of H2O(g) + CO(g) ?
What happens to amounts of H2(g) + CO2(g) ?
Reaction still occurring past dotted line (although concentrations don’t change): Dynamic Equilibrium
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Dynamic Equilibrium
H2O(g) + CO(g) H2(g) + CO2(g)
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Equilibrium Expression and K Law of mass action
jA + kB lC + mD
K = [C]l [D]m Equilibrium Expression [A]j [B]k
Concentrations of species at equilibrium K = equilibrium constant
H2O(g) + CO(g) H2(g) + CO2(g)
2NO2(g) N2O4(g)
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Value of Equilibrium Constant3H2(g) + N2(g) 2NH3(g)
Value for K is always the same for a particular reaction,
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Magnitude of K Equilibrium position (does equilibrium lie towards products or
reactants?); is this important (Synthesis of Aspirin) Large K
K1
Small K
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Writing equilibrium expressionsAlways predicted from the balanced equation:
4NH3(g) + 7O2(g) 4NO2(g) + 6H2O(g)
I2(g) + H2(g) 2HI(g)
C4H10(g) + O2(g) CO2(g) + H2O(g)
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Calculating values of K
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Eq. laws for gaseous reactions3H2(g) + N2(g) 2NH3(g)
K = [NH3]2 Equilibrium constant found in terms of
[H2]3 [N2] concentrations of species (Kc)
K can also be found in terms of partial pressures (Kp)
PV = nRT
Kp = PNH32
(PH23)(PN2)
Relationship between Kp and Kc:
Kp = Kc(RT)ng
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Heterogeneous Equilibria More than one phase exists in reaction mixture Thermal decomposition of CaCO3(s) CaO(s) + CO2(g)
Concentrations of pure solids and pure liquids are always constant (thus, can be removed from eq. expression)
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Heterogeneous Equilibria Write equilibrium expressions (in terms of both K and Kp
for each of the following):
1. CaO(s) + SO2(g) CaSO3(s)
2. Decomposition of solid phosphorous pentachloride to liquid phosphorous trichloride and chlorine gas
3. Deep blue solid copper(II)sulfate pentahydrate is heated to drive off water vapor to form white solid copper(II)sulfate
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Reaction Quotient, Q In which direction will a particular reaction shift to reach
equilibrium?
3H2(g) + N2(g) 2NH3(g)
If [NH3]0 = 0, shift to right to achieve equilibrium.
If [H2]0 or [N2]0 = 0, shift to left to achieve equilibrium.
If initial concentrations of all three species are nonzero, which way will shift occur to achieve equilibrium? More difficult to predict.
Use Reaction Quotient, Q Q is obtained by applying law of Mass Action to initial
concentrations of species involved.
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Reaction Quotient, Q3H2(g) + N2(g) 2NH3(g) Q = [NH3]o
2
[H2]o3 [N2]o
Then, to determine in which direction a system will shift to reach equilibrium, compare values of Q and K:
1. Q = K System is at equilibrium
2. Q > K Ratio of initial conc. of products to initial conc. of reactants is too large.
System shifts to the left to reach equilibrium.
3. Q < K Ratio of initial conc. of products to initial conc. of reactants is too small.
System shifts to the right to reach equilibrium
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‘ICE’ Tables
Calculating Equilibrium Concentrations
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Le Chatelier’s Principle ‘If an outside influence upsets an equilibrium, the system
undergoes a change in the direction that counteracts the disturbing influence, and, if possible, returns the system to equilibrium.’
Outside influences?
Adding / removing a reactant / product Changing volume/pressure of gaseous reactions Changing T
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Adding/removing a reactant or product Eq. shifts in direction that will partially consume a reactant or
product added Eq. shifts in direction that will partially replace a reactant or
product removed
3H2(g) + N2(g) 2NH3(g
Add some N2 to above equilibrium; which way will it shift to re-establish equilibrium?
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Changing volume/pressure Reducing volume (what happens to the pressure?) – eq. shifts to
side with smaller # of gas molecules
3H2(g) + N2(g) 2NH3(g
Increasing volume? What would happen here?
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Changing volume/pressure
2NO2(g) N2O4(g)
brown colorless
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Changing T Increasing T shifts an equilibrium in direction that produces an
endothermic change (need to know energy involved in reaction to predict which direction this is)
3H2(g) + N2(g) 2NH3(g) H= -46.19 kJ/mol
Exothermic or endothermic reaction?
Increasing T: Decreasing T:
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Changing T
Is this reaction exo- or endothermic?
2NO2(g) N2O4(g)
brown colorless