instructor: dr. marinella sandros 1 nanochemistry nan 601 reaction mechanisms and catalysis
TRANSCRIPT
Instructor: Instructor:
Dr. Marinella SandrosDr. Marinella Sandros
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NanochemistrNanochemistryy
NAN 601NAN 601
Reaction mechanisms and Catalysis
“A sequential series of simple reactions which combine to form a larger, balanced chemical equation.”
For the overall reactionNO2 + CO CO2 + NO
The elementary reactions of the mechanism are
2NO2 NO + NO3 R1 = k1[NO2]2
molecularity = 2
NO3 + CO NO2 + CO2 R2 = k2[NO3][CO]molecularity = 2
For any elementary reaction◦ the order of the reaction wrt a reactant is its stoichiometric
coefficient in that step◦ the molecularity of the reaction is the sum of the stoichiometric
coefficients for that step. The molecularity corresponds to the number of molecules that actually collide in that step!
◦ NO3 is an intermediate.
Rule #1For any step, the order of that step w.r.t. a reactant is its stoichiometric coefficient in that step.For step 2 in the previous reaction
NO3 + CO NO2 + CO2 R2 = k2[NO3][CO]
NO2 + CO CO2 + NO
Two elementary reactions:2NO2 NO + NO3 (slow) R1 =
k1[NO2]2
NO3 + CO NO2 + CO2 (fast) R2 = k2[NO3][CO]
Overall reaction:NO2 + CO CO2 + NO Rate =
R1 =k1[NO2]2
The rate law for the overall reaction is the rate law for the
rate-limiting step!
Rule #2For a multistep reaction in which one step is much slower than the others,
overall rate = rate of slowest step
For any step, the order of that step w.r.t. a reactant is its stoichiometric coefficient in that step.
For a multi-step reaction in which one step is much slower than the others, the overall rate is equal to the rate of the slowest step
Write the rate equation for the overall reaction in terms of the reactants in the net reaction.
Step 1: NO (g) + NO (g) N2O2 (g) (fast)
Step 2: N2O2 (g) + Br2(g) 2 NOBr (g) (slow)
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K1
K-1
k2
2 NO (g) + Br2(g) 2NOBr (g)
Experimentally determined rate law:rate= k [NO]2[Br]
Show the following mechanism also produces a rate law consistent with experimentally
observed one?
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Step 1: NO (g) + NO (g) N2O2 (g) (fast)
Step 2: N2O2 (g) + Br2(g) 2 NOBr (g) (slow)
K1
K-1
k2
Step 2 is rate limiting!!!
Rate= k2 [N2O2][Br2]
K1[NO]2 = k-1 [N2O2 ]
K1[NO]2 = [N2O2 ]k-1
Rate= k2 K1[NO]2 [Br2] = k [NO]2[Br2]
k-1
A catalyst (Greek: καταλύτης, catalytēs) is a substance that accelerates the rate of a chemical reaction without itself being transformed or consumed by the reaction. (wikepedia)
A + B
C
ΔG
Ea
uncatalyzed
A + B +catalyst
C + catalyst
ΔG
Ea′
catalyzed
k(T) = k0e-Ea/RT
Ea′ < Ea
k0′ > k0
k′ > k
ΔG = ΔG
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Catalyst ??Efficiency depends on activity, properties & life of
the catalyst
• Examples:
• Ammonia synthesis – Promoted iron
• SO2 oxidation – Venadium Pentaoxide
• Cracking – Sylica, alumina
• Dehydrogenation – Platinum, Molybdenum
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A reaction may have a large, negative ΔGrxn, but the rate may be so slow that there is no evidence of it occurring.
Kinetic Vs. Thermodynamic
Conversion of graphite to diamonds is a thermodynamic favor process (ΔG -ve ).
C (graphite) --> C (diamond)
Kinetics makes this reaction nearly impossible (Requires a very high pressure and temperature over long time)
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This means , the catalyst changes the reaction path by lowering its activation energy and consequently the catalyst increases the rate of reaction.
A catalyst that is present in the same phase as the reacting molecules.
Example:
The Decomposition of aqueous hydrogen peroxide
2 H2O2 (aq) 2H2O (l) + O2 (g)
Very very very slow!!!!!!
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Catalyzed by Bromine:
Br2 (aq) + H2O2 (aq) 2 Br- (aq) + 2 H+ (aq) + O2 (g)
2 Br- (aq) + H2O2 (aq) + 2 H+ (aq) Br2 (l) + 2H2O (l)
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The two reactions together serve as a catalytic pathway for hydrogen peroxide decompostion.
Both of them must have significantly lower activation energies than the uncatalyzed decomposition.
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The catalyst exists in a different phase from the reactant molecules, usually as a solid in contact with either gaseous reactants or with reactants in a liquid solution.
Many industrially important reactions are catalyzed by the surfaces of the solids.
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Sulfuric acid synthesis (Contact process)
SO2 + O2, SO3 vanadium oxideshydration of SO3 gives H2SO4
Ammonia synthesis (Haber-Bosch process)
N2 + H2, NH3 iron oxides on aluminaconsumes 1% of world's industrial energy budget
Nitric acid synthesis (Ostwald process)
NH3 + O2, HNO3unsupported Pt-Rh gauze
direct routes from N2 are uneconomical
Hydrogen production by Steam reforming
CH4 + H2O, H2 + CO2 Nickel or K2OGreener routes to H2 by water splitting actively sought
Ethylene oxide synthesis
C2H4 + O2, C2H4Osilver on alumina, with many promotors
poorly applicable to other alkenes
Hydrogen cyanide synthesis (Andrussov oxidation)
NH3 + O2 + CH4, HCN Pt-RhRelated ammoxidation process converts hydrocarbons to nitriles
Olefin polymerization Ziegler-Natta polymerization
propylene, polypropylene
TiCl3 on MgCl2
many variations exist, including some homogeneous examples
Desulfurization of petroleum (hydrodesulfurization)
H2 + R2S (idealized organosulfur impurity), RH + H2S
Mo-Co on aluminaproduces low-sulfur hydrocarbons, sulfur recovered via the Claus
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http://en.wikipedia.org/wiki/Heterogeneous_catalysis
Heterogeneous catalysts are often composed of metals or metal oxides.
Initial step is usually Adsorption of reactants.
Adsorption binding of molecules to a surface, whereas absorption refers to the uptake of molecules into the interior of another substance.
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H H H H H H H H H H H H H H H H H H
H
H
HH
H
HH
H
H
H
H
H
H
H
H
H
HH
H2 absorption onpalladium hydride
H2 adsorption onpalladium
Adsorption occurs because the atoms or ions at the surface of a solid are extremely
reactive.
Example of heterogeneous catalysis is the reaction of hydrogen with ethylene:
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C2H4 + H2 C2H6 VERY SLOW!
However in the presence of finely powdered metal such as nickel or
palladium at room temperature and under <200 atm of hydrogen pressure.
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In physisorption
1. The bond is a van der Waals interaction
2. Adsorption energy is typically 5-10 kJ/mol. ( much weaker than a typical chemical bond )
3. Many layers of adsorbed molecules may be formed.
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For Chemisorption
1. The adsorption energy is comparable to the energy of a chemical bond.
2. The molecule may chemisorp intact (left) or it may dissociate (right).
3. The chemisorption energy is 30-70 kJ/mol for molecules and 100-400 kJ/mol for atoms.
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Adsorbent: surface onto which adsorption can occur.example: catalyst surface, activated carbon, alumina
Adsorbate: molecules or atoms that adsorb onto the substrate.example: nitrogen, hydrogen, carbon monoxide, water
Adsorption: the process by which a molecule or atom adsorb onto a surface of substrate.Coverage: a measure of the extent of adsorption of a species onto a surface
H H H H H H H H Hadsorbate
adsorbent
H H H H H
coverage θfraction of surface sites occupied
2NO (g) + 2N2O(g) 2N2(g) + 2NO2(g)
2 NO2(g) 2NO(g) + O2 (g)
a)What is the chemical equation for the overall equation?
b)Why is NO considered a catalyst and not an intermediate?
c) Is this an example of homogeneous or heterogeneous catalysis?
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