Home > Uncategorized > Introduction to Solid State ChemistryLecture 23: Reaction Rates

Introduction to Solid State ChemistryLecture 23: Reaction Rates

Today’s lecture covers reaction rates and costs 53 minutes.

N2O5 = 2NO2 + .5O2

Radioactive decay is 1st order. U238=Th234+ He4
Half Life = ln 2/K = 0.693/k

2NO2 = 2NO + O2
-dc/dt = kc^2
This is based on experiment, not stoichiometry.

Integral method uses the integrated form of the rate equation. Trial and error. Or by inspection. The differential method defines the rate.

To increase the rate of reaction, increase T, increase concentration, or add a catalyst. Catalysts reduce Ea. More molecules will have the energy to react. Catalysts need to have an affinity for the reagents, a disaffinity for the products and selectivity.

Diffusion is a rate phenonmenon – d/dt. Transport energy and matter. Energy is motion is heat transfer. The Hindenburg didn’t explode, it just burned, hydrogen transport limited it.

Dope silicon in the solid state. Silicon is single crystal. Flow B2H6 gas over it.

B2H6= 2B + 3H2

Fick’s Law
Flux (mass flow rate in x direction) = -diffusivity (dC/dx)

c8H18 is gas. CO is a product of incomplete combustion. ox = N2 O2 CO2

Pt-Pd for hydrocarbons and CO which are oxidation rxns.
Rh for NOx which are reduction rxns.
unburned hydrocarbons 200ppm will kill. Catalystis is a surface effect. A monolayer has no mechanical strength.

y=mx + b
Cuprite CU2O
Chalcocite CU2S
Chalcopyrite CuFeS2
Tenorite CuO
Hematite Fe2O3
Magnetite Fe3O4
Oxidising agents give oxygen to another substance.
Reducing agents remove oxygen from another substance.
Oxidation is loss of hydrogen.
Reduction is gain of hydrogen
MAC glass = mobility arrangement cooling rate
half life of C14 5720 years
IE13 electron acceptor, electrophile, nonmetal.

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