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Platinum Metals Rev., 1966, 10, (1), 10

Mixed Platinum Metal Oxide Catalysts

Activity Patterns in Alloy Systems

  • By G. C. Bond, Ph.D., D.Sc.,
  • D. E. Webster, Ph.D.
  • Research Laboratories, Johnson Matthey & Co Limited
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In a previous paper (1 we demonstrated that ruthenium-platinum oxides on reduction under mild conditions yielded catalysts whose activity was superior to that of reduced platinum oxide for a number of hydrogenation reactions. We have now extended our work to examine a range of mixed platinum metal oxide systems, particularly the iridium-platinum, palladium-platinum, rhodium-platinum, rhodium-palladium and ruthenium-palladium systems, and find that the phenomenon of an activity maximum at some point is one of wide occurrence. The mixed oxides were prepared by methods similar to that described previously for ruthenium-platinum oxides; salts used were ammonium chloroplatinate, palladium chloride, ruthenium trichloride, rhodium trichloride, and ammonium chloroiridate or iridium tetrachloride.

In Fig. 1 we plot the activity (measured in ml H2 STP min−1 (10 mg)−1) of reduced ruthenium-palladium, iridium-platinum and rhodium-palladium oxides for the reduction of 6 per cent nitrobenzene in methanol at 30°C: our former results for reduced ruthenium-palladium oxides are included for comparison. We previously (1 advanced the hypothesis that the observed variations in activity are determined by the electronic constitution of the catalysts. This can be given quantitative expression in terms of the fractional number of d -electron vacancies per atom in each catalyst, assuming all to be homogeneous alloys, and we may now explore the applicability of this concept to our results. The fractions of d -electron vacancies per atom for the pure metals are taken to be (2: Pt and Pd, 0.6; Rh, 1.4; Ir, 1.7; and Ru, 2.2: values for mixtures are obtained by linear interpolation.

Fig. 1

The activity of reduced Ru-Pt, Ru-Pd, Ir-Pt and Rh-Pd oxides for the hydrogenation of 6 per cent nitrobenzene in methanol at 30°C

The activity of reduced Ru-Pt, Ru-Pd, Ir-Pt and Rh-Pd oxides for the hydrogenation of 6 per cent nitrobenzene in methanol at 30°C

In Table I we have listed the maximum rate observed with each alloy system and the composition at which this occurs (from Fig. 1). We then list the composition at which in each system there should theoretically be exactly 1.0 electron holes per atom. In two systems (Ru-Pt and Ru-Pd) this occurs precisely at the composition giving highest activity, but in the remaining systems the agreement is unsatisfactory. We have also evaluated the composition at which there should be 0.75 electron holes per atom and then find that in the Ir-Pt and Rh-Pd systems this composition tallies closely with that giving maximum activity.

Table I

Catalytic Activity for Nitrobenzene Hydrogenation and Electronic Structure of Ru-Pt, Ru-Pd, Ir-Pt and Rh-Pd Systems

SystemMaximum activity ml H2 STP min.−1 (10 mg)−1Composition at which activity is maximumComposition for 1.0 electron hole/atomComposition for 0.75 electron hole/atom
Ru-Pt17025 atom % Ru25 atom % Ru10 atom % Ru
Ru-Pd7025 atom % Ru25 atom % Ru10 atom % Ru
Ir-Pt17015 atom % Ir36 atom % Ir13.5 atom % Ir
Rh-Pd5025 atom % Rh50 atom % Rh18.5 atom % Rh

These results lead us to the following generalisations:

  • To obtain the highest activities in nitrobenzene hydrogenation, Pt must be a component of the mixture; in this sense Pd cannot replace Pt although both have nominally the same electronic structure.

  • When mixtures of metals from adjacent vertical groups are used, maximum rates of nitrobenzene hydrogenation occur when the electron hole/atom ratio is about 0.75; with metals from non-adjacent vertical groups, the optimum value of this ratio rises to about 1.0. There are clearly other factors besides the electronic structure of the component metals determining the catalytic properties of alloys.

In our previous paper (1 we showed with Ru-Pt oxides that activity maxima were shown in a number of other hydrogenations, these maxima occurring at different compositions. Table II summarises the systems in which distinct activity maxima have been observed. We have not yet examined these reactions in sufficient detail to make it worthwhile recording the compositions (or electron hole/atom ratios) at which maximum rates occur, and no generalisations have yet emerged. In several cases however maximum rates in olefin hydrogenation occur at about the same compositions at which maximum rates of nitrobenzene hydrogenation are observed. A clear illustration of the lower activity of pure metals in comparison with their mixtures or alloys is shown in Fig. 2, where rates of hydrogenation of aqueous methylethylketone are plotted against atomic composition for the Rh-Pd and Ru-Rh systems.

Table II

Reactions and Catalyst Systems Showing Activity Maxima

ReactantSolventCatalyst Systems
Maleic acidmethanolPd-Ru, Pt-lr, Pt-Ru
CyclohexenemethanolPt-lr, Pt-Ru
2-Methylbut-3-en-2-olmethanolPd-Ru, Pt-lr, Pt-Ru
Benzene, phenolmethanol, waterPd-Rh, Pt-Rh
MethylethylketonewaterRh-Ru, Pd-Rh, Pt-Ru

Fig. 2

The activity of reduced Rh-Pd, Ru-Rh and Ru-Pd oxides for the hydrogenation of aqueous methylethylketone. Open circles represent the activity of the pure metals

The activity of reduced Rh-Pd, Ru-Rh and Ru-Pd oxides for the hydrogenation of aqueous methylethylketone. Open circles represent the activity of the pure metals

However, the catalytic properties of a metal cannot be reproduced by compounding equi-atomic proportions of the metals lying to each side of it in the Periodic Classification: for example, the activity of the mixture of 50:50 Ru-Pd for hydrogenation of methylethylketone is much less than that of pure rhodium as can be clearly seen from the bottom curve of Fig. 2.

The final demonstration that the electronic structure of the catalyst is not the sole factor in deciding the positions at which activity maxima occur comes from results we have obtained with reduced Pd-Pt oxides. Since both of these metals are taken to have 0.6 electron holes/atom, no activity maxima are to be expected on electronic grounds; nevertheless they are observed. The activities shown in Fig. 3 are relative to those of palladium and platinum separately: in the cases of the hydrogenation of 1-pentene and of nitrobenzene, the activities of both metals are essentially the same. Maxima for both these reactions occur at about 15 atomic per cent platinum. Also shown in this figure are results obtained by McKee and Norton (2 for the reactions of propane hydrogenolysis and of methane-deuterium exchange at 150°C over palladium-platinum alloys obtained by reduction of mixed salt solutions by sodium borohydride. In these cases the rates are relative to the rate expected if there were a linear relation between activity and atomic composition. In the case of propane hydrogenolysis, the maximum enhancement also occurs at about 15 atomic per cent platinum, although rates of methane exchange are generally less than predicted assuming additive behaviour of the two metals, a fact not explicitly commented on by McKee and Norton. The rate of hydrogenation of 2-methylbut-3-en-2-ol is a maximum at about 20 atomic per cent platinum, and we therefore conclude that this composition possesses some properties which maximise catalytic activity.

Fig. 3

The activities of reduced Pd-Pt oxides for the hydrogenation of 1-pentene in methanol (○1;) and for the hydrogenation of nitrobenzene in methanol (+), and of Pd-Pt alloys for propane hydrogenolysis (Δ) and for methane-deuterium exchange (•)

The activities of reduced Pd-Pt oxides for the hydrogenation of 1-pentene in methanol (○1;) and for the hydrogenation of nitrobenzene in methanol (+), and of Pd-Pt alloys for propane hydrogenolysis (Δ) and for methane-deuterium exchange (•)

Although we cannot yet claim to have established a coherent body of satisfactory observations on our reduced oxide catalysts, far less to have understood their meaning fully, we nevertheless feel confident that we can, by continuing this line of investigation arrive, in due course, at some generalisations which should have considerable predictive value.

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References

  1. 1
    G. C. Bond and D. E. Webster, Platinum Metals Rev., 1965, 9, 12
  2. 2
    D. W. McKee and F. J. Norton, J. Catalysis, 1964, 3, 252

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