Introduction to Catalysis¶
What is Catalysis¶
Definition: “A substance that increases the rate (k) of a chemical reaction, without undergoing any permanent change “.
In practice, this isn;t entirely true as catalysts do break down over time, however they can partake in significantly more than a stoichiometric amount of reactions.
A catalyst doesn;t change the thermodynamics of \(A\) or \(B\), but it will change the rate in which \(A\) will become \(B\).
Philosophically speaking, the utility of the reaction is on;y present if \(B\) can be formed in your lifetime
“Our ability to devise traightforward and practical chemical syntheses is indespensible to the survival of our species”
David Lupton would suggest that our ability on its own is not enough, and that we need govrnment penalties on economy to drive the adoption, that maked the discovery meaningful.
Ryoji Noyori found a way to produce methol which is an incredibly valuable product and can be made with a massive markup.
Each of these steps is catalysed, one step in particular uses this rhodium binap TM complex.
The economic value of this process is so highly saught after that many companies have since tried to refine it, with BASF being able to synthesise it in four steps. The point being that economics drives discovery.
The vast majority of chemical manufacturing revenue comes from three primary industries; pharmaceuticals, polymers and petrochemical cracking (making specific lower MW molecules from the high MW crude material).
Methods of Catalysis¶
Catalysis generally comes in two forms:
Lowering the Energy of the Transition State¶
Using a Lower Energy TS Pathway¶
One method of biologically reducing the TS energy barrier is to develop some antibodies against the transition state that can stabilise the structure, making it easier for the reaction to occur. In the example of cocaine metabolism, below, we can see that by hydrolysing the ester, the cocaine molecule is deactivated.
If we take a closer look at the reaction we can come up with this reaction mechanism that has two transition states and one intermediate.
When we plot the energy of this reaction we can easily see that the rate determining step (RDS) is TS1.
So we can create a mimic of this structure using phosphate to generate some antibodies against.
When we introduce these antibodies into the system, they will bind to the transition state, lowering their energy, in turn reducing the activation energy for the metabolism of the cocaine.
In terms of using an alternative pathway, in the olefin metathesis (“to move about”) example above, the reactants and products are thermoneutral both the same energy, so this reaction has no real motivator to overcome the massive energy of the transition state. Instead, by making a series of lower cost reaction that are driven by entropy, this reaction has a chance of proceeding.
In this case, the entropy is increased, decreasing the Gibbs free energy, as ethylene gas is produced, but it’s also a product that can be removed, driving the equilibrium forward.
Catalysts can either be homogeneous (in the same phase as the reactants) or heterogeneous (in a different phase to the reactants).
There are some advantages/limitations to both:
|Con||Makes separation more difficult, and ensures that a purification step needs to be taken||Pro||They are good for ensuring that the products and the catalysts remain separated|
|Con||Catalysts loadings are higher, making them less effective||Con||Highly specialised usage and apparatus is required|
|Pro||They can be easily treated like any other reagent in the reaction|
|Pro||No special hardware is required|
A great example of heterogeneous catalysis is the Haber-Bosch process, as the solid catalysts will never come across in the gaseous products (the ammonia is only liquid once condensed).
Quantifying Catalytic Activity¶
We can quantify the activity of a catalyst with three main metrics; speed, robustness and stereoselectivity
We’ll use the reaction below to demonstrate this:
Turn Over Number (TON) - Robustness¶
This is a measure of how many times the catalytic process can happen before the catalyst expires.
For the reaction above, we have a 97% yield and a 0.1 mol% consumption of catalyst
First we have to calculate how many moles of product, reactant and catlayst areconsumed/produced inthe reaction
So now we can calculate the TON
Yield from TON¶
Turn Over Frequency (TOF) - Speed¶
Is how often the reaction happens
Is a measure of how much of one isomer the catalysts produces over the other. These are a few of the metrics we use
Diasteromeric excess isn’t really used as a metric.
Converting e.e. to e.r.¶
Thiese are simultaneous equations, so the second step of the e.e. of \(S\) substitutes back in to the second step of the e.e. of \(R\).