Transition Metals: Catalysts Flashcards
What kind of catalysts can transition metals and their compounds act as?
- Heterogenous catalysts
- Homogenous catalysts
Why are transition metals good catalysts?
- TMs can exist in variable oxidation states so can provide alternative pathways with lower Ea easily
What is a heterogenous catalyst?
- A heterogeneous catalyst is in a different phase from the reactants
- Reaction occurs at active sites on the surface
What does the efficiency of heterogenous catalysts depend on?
• Strength of adsorption
- How strong reactants stick to surface of TM (compound)
• Strength of desorption
- How well products unstick to surface of TM (compound)
What is a homogenous catalyst?
- A homogenous catalyst is in the same phase as the reactants
What is used to minimise the cost of heterogenous catalysts?
- Support medium
- Used to increase surface area of catalyst
What can reduce the surface area of a catalyst? How can this be tackled?
- Catalyst poisoning
- Impurities may adsorb onto surface of heterogenous catalysts and block active sites from reactants
- Purifying reactants
Which heterogenous catalysts must you know about?
- Vanadium(V) oxide( V2O5) in the Contact process
- Fe in the Haber process
Give the overall equation for the Contact Process
- SO2 (g) + ½O2 (g) → SO3 (g)
- Above → is V2O5(s) catalyst
Give all of the equations involved in the Contact Process and the changes in oxidation states of vanadium
- V2O5 + SO2 → V2O4 + SO3
- Vanadium reduced from +5 to +4
- ½O2 + V2O4 → V2O5
- Vanadium oxidised from +4 to +5
- SO2 (g) + ½O2 (g) → SO3 (g)
Give the equation for the Haber process
- N2 (g) + 3H2 (g) → 2NH3 (g)
- Above → is Fe(s)
In reactions with homogenous catalysts, what must reactions proceed through?
- Reactions must proceed through an intermediate species where the TM ion temporarily changes oxidation state
- Reactions combine with catalyst to make an intermediate species, which then reacts to form the products and reform the catalyst
Which homogenous catalysts must you know about?
- Fe2+ catalysing reaction between S2O82- (peroxydisulfate) and I-
- Mn2+ autocatalysing reaction between MnO4- and C2O42-
Give the overall reaction between S2O82- and I-
- S2O82- (aq) + 2I- (aq) → I2 (aq) + 2SO42- (aq)
Why does the reaction between S2O82- and I- occur slowly? How does iron(II) or iron (II) act as a catalyst?
- Both ions are negatively charged so repel
- Low collision frequency and high Ea
- Positively charged iron ions are attracted to the negatively charged reactants resulting in a reaction with lower Ea