Transition Metals: Catalysts Flashcards

1
Q

What kind of catalysts can transition metals and their compounds act as?

A
  • Heterogenous catalysts
  • Homogenous catalysts
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2
Q

Why are transition metals good catalysts?

A
  • TMs can exist in variable oxidation states so can provide alternative pathways with lower Ea easily
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3
Q

What is a heterogenous catalyst?

A
  • A heterogeneous catalyst is in a different phase from the reactants
  • Reaction occurs at active sites on the surface
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4
Q

What does the efficiency of heterogenous catalysts depend on?

A

• Strength of adsorption

  • How strong reactants stick to surface of TM (compound)

• Strength of desorption

  • How well products unstick to surface of TM (compound)
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5
Q

What is a homogenous catalyst?

A
  • A homogenous catalyst is in the same phase as the reactants
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6
Q

What is used to minimise the cost of heterogenous catalysts?

A
  • Support medium
  • Used to increase surface area of catalyst
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7
Q

What can reduce the surface area of a catalyst? How can this be tackled?

A
  • Catalyst poisoning
  • Impurities may adsorb onto surface of heterogenous catalysts and block active sites from reactants
  • Purifying reactants
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8
Q

Which heterogenous catalysts must you know about?

A
  • Vanadium(V) oxide( V2O5) in the Contact process
  • Fe in the Haber process
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9
Q

Give the overall equation for the Contact Process

A
  • SO2 (g) + ½O2 (g) → SO3 (g)
  • Above → is V2O5(s) catalyst
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10
Q

Give all of the equations involved in the Contact Process and the changes in oxidation states of vanadium

A
  • 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)
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11
Q

Give the equation for the Haber process

A
  • N2 (g) + 3H2 (g) → 2NH3 (g)
  • Above → is Fe(s)
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12
Q

In reactions with homogenous catalysts, what must reactions proceed through?

A
  • 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
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13
Q

Which homogenous catalysts must you know about?

A
  • Fe2+ catalysing reaction between S2O82- (peroxydisulfate) and I-
  • Mn2+ autocatalysing reaction between MnO4- and C2O42-
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14
Q

Give the overall reaction between S2O82- and I-

A
  • S2O82- (aq) + 2I- (aq) → I2 (aq) + 2SO42- (aq)
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15
Q

Why does the reaction between S2O82- and I- occur slowly? How does iron(II) or iron (II) act as a catalyst?

A
  • 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
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16
Q

Give all the equations involved in the reaction between S2O82- and I-

A
  • S2O82- (aq) + 2Fe2+ (aq) → 2Fe3+ (aq) + 2SO42- (aq)
  • 2I(aq) + 2Fe3+ (aq) → I2 (aq) + 2Fe2+ (aq)

- S2O82–(aq) + 2I(aq) → 2SO42–(aq) + I2(aq)

17
Q

What does autocatalysis mean?

A
  • When one of the products of a reaction acts as a catalyst for the reaction
18
Q

How does Mn2+ autocatalyse the reaction between MnO4- and C2O42-?

A
  • Mn2+ isn’t present at start of reaction but after it’s produced it acts as a catalyst
19
Q

Give the overall equation for the reaction between MnO4and C2O42‒

A
  • 2MnO4(aq) + 16H+(aq) + 5C2O42‒(aq) → 2Mn2+(aq) + 8H2O(l) + 10CO2(g)
20
Q

Give all the reactions involved in the reaction between MnO4and C2O42‒

A
  • MnO4(aq) + 8H+(aq) + 5e → Mn2+(aq) + 4H2O(l)
  • C2O42–(aq) → 2CO2(g) + 2e
  • 2MnO4(aq) + 16H+(aq) + 5C2O42‒(aq) → 2Mn2+(aq) + 8H2O(l) + 10CO2(g)
21
Q

Draw a concentration-time graph for the reaction between MnO4and C2O42‒ and explain its shape

A
  • Curve starts with small gradient (low rate)
  • Negative ions collide so Ea high
  • Curve gets steeper
  • Because autocatalyst (Mn2+) is formed
  • Curve levels out approaching time axis
  • Because MnO4- ions used up