REACTION DYNAMICS Hilary Term 2011 1. Introduction
6 Lectures Prof M. Brouard Thermally averaged rate coefficients
The thermal rate coefficient, k(T ), is a highly averaged quantity. Understanding Look again at simple collision theory: Predicting chemical reactivity 1 • Reactions occur by collisions Controlling • Collision energy2 (E ) must exceed the barrier height (E ) t 0
At fixed relative velocity, crel (or collision energy, Et) 1. Introduction
Reaction rate = Rate of reactive collisions at velocity crel × 2. Elastic and Inelastic scattering Fraction of collisions at velocity crel, f(crel)
3. Determining the angular distribution miss hit 2 sc = p d
4. Controlling reagents and characterizing products
crel 5. Interpretation
Rate of reactive collisions = k(crel) [A] [B] 6. Probing the transition state.
1 Reactants are structureless spheres, with radii rA and rB and collision diameter d = rA + rB 2 relative motion 1 2 The collision energy is the translational energy associated with Et = 2 µcrel with mAmB v v µ = mA+mB and crel is the relative speed (crel = | B − A|).
1 k(crel) defines the reactive collision volume swept out per unit time State-resolved properties
k(crel)= crel σ(crel) , Example 1 where σ(crel) is the cross-section for the process of interest at velocity K + HCl(v) −→ KCl + H ∆H◦− = 4 kJ mol−1 crel.
−1 f(crel)dcrel is the fraction of collisions with velocities in the range crel to HCl(v = 1) has an energy of 34.5kJmol . crel + dcrel:
3/2 µ 2 −µcrel/2RT 2 f(crel) dcrel = e 4πcreldcrel Put this energy into HCl(v = 1) and rate increases by ×100. 2πkBT
Put same energy into relative translation and the rate increases by ×10. f c ()rel c s()rel Vibrational energy is ∼10 times more efficient at promoting reaction than translational energy. c rel
Example 2 Reaction rate at velocity crel d[A] OH + H (v =0, 1) −→ H O + H = − = k(c ) [A] [B] f(c ) 2 2 dt rel rel
The thermal rate constant is obtained by averaging k(crel) = crel σ(crel) Vibrational excitation of the H2 to v = 1 increases the rate constant by over the Maxwell Boltzmann distribution: over a factor of 100 (i.e. kv=1(T ) & 100 kv=0(T )).
∞ Vibrational excitation of the ‘spectator’ OH reactant has very little effect k(T )= crel σ(crel) f(crel) dcrel . Z0 on the reaction rate.
2 Example 3 Conservation laws
O + CS −→ CO(v0) + S Consider A + BC −→ AB + C
P() v’ Conservation of energy3
E ◦− tot Eavl = Et + Evib + Erot − ∆H E E’ t t
1 E 0 0 0 0 v E’ f = E + E + E . v v’ t vib rot E E avl So, for example, the fraction of r There is a population inversion in the CO product vibrational levels. reactants E’ the energy released as vibration r Populations cannot be described by Boltzmann distribution (i.e. not at would be 0 0 products thermal equilibrium). fv = Evib/Eavl .
Reactant energies influence the course of a reaction. Conservation of angular momentum
Products can be formed in a non-Boltzmann fashion. Rotational angular momentum |jBC| = J(J + 1) ~. p probe c Need to the populations over the product states.... A rel
....and control the populations in the reactant states. b For example BC
• Velocities (magnitude and direction)
Orbital angular momentum |L| = L(L + 1) ~ = µcrelb. • Vibrational and rotational (internal) energies p 0 0 Jtot = jBC + L = jAB + L . • Orientation
3It is helpful to define the total energy (with respect to the reactants): ◦− 0 0 0 The above examples suggest that reaction cross-sections can depend on Etot = Et + Evib + Erot =∆H + Et + Evib + Erot . all of these quantities.
3 Forces and potential energy surfaces Experimental requirements
Wish to select the energies and quantum states of the reactants Aim to understand forces which control interactions between atoms. and/or One dimension - a diatomic potential energy curve probe the energies and quantum state populations of the nascent prod- ucts
VR() Need to ensure collisional scrambling of the reactants and products dV (R) F (R)= − does not occur. dR R
One method is to use molecular beams
high vacuum f(c) -1