Rhenium(VII) sulfide

{{Chembox

| ImageFile =

| ImageSize = 250px

| IUPACName = Rhenium(VII) sulfide

| OtherNames =

|Section1={{Chembox Identifiers

| CASNo = 12038-67-4

| CASNo_Ref = {{cascite|correct|CAS}}

| UNII = K72K37878A

| UNII_Ref = {{fdacite|correct|FDA}}

| PubChem = 159414

| ChemSpiderID = 21171359

| DTXSID = DTXSID901022921

| EC_number = 234-882-5

| SMILES = S=[Re](=S)(=S)S[Re](=S)(=S)=S

| InChI = 1/2Re.7S/rRe2S7/c3-1(4,5)9-2(6,7)8

| InChIKey = CVHXCQNYOAKCMI-NEHFBHEFAV

| StdInChI = 1S/2Re.7S

| StdInChIKey = CVHXCQNYOAKCMI-UHFFFAOYSA-N

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|Section2={{Chembox Properties

| Formula = Re₂S₇

| MolarMass = 596.869 g/mol

| Appearance =

| Density =

| MeltingPt =

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|Section3={{Chembox Hazards

| GHSPictograms = {{GHS06}}{{GHS07}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|301|315|319|331|412}}

| PPhrases = {{P-phrases|261|264|270|271|273|280|301+310|302+352|304+340|305+351+338|311|321|330|332+313|337+313|362|403+233|405|501}}

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Rhenium(VII) sulfide is a chemical compound with the formula Re₂S₇. It has a complex structure, but can be synthesized from direct combination of the elements:{{cite journal |author1=Schwarz, D. E. |author2=Frenkel, A. I. |author3=Nuzzo, R. G. |author4=Rauchfuss, T. B. |author5=Vairavamurthy, A. |year=2004 |title=Electrosynthesis of {{chem|Re|S|4}}. XAS Analysis of {{chem|Re|S|2}}, {{chem|Re|2|S|7}}, and {{chem|Re|S|4}} |journal=Chemistry of Materials |volume=16 |pages=151–158 |doi=10.1021/cm034467v}} 2Re{} + 7S ->[{}\atop\Delta] Re2S7Alternatively, rhenium(VII) oxide reacts with hydrogen sulfide in 4N HCl to the same end:{{Greenwood&Earnshaw}} Re2O7{} + 7H2S ->[{}\atop\Delta] Re2S7{} + 7H2O

The compound catalyses the reduction of nitric oxide to nitrous oxide and hydrogenation of double bonds. In this regard, it unusually tolerates sulfur compounds, which poison noble metal catalysts.

Rhenium(VII) sulfide decomposes when heated. In vacuum, it generates rhenium(IV) sulfide:

:$\backslash mathrm\{Re\_2S\_7\; \backslash \; \backslash xrightarrow\{600^oC\}\backslash \; 2ReS\_2\; +\; 3S\; \}$

In air, the sulfide oxidizes to sulfur dioxide:

:$\backslash mathrm\{2Re\_2S\_7\; +\; 21O\_2\; \backslash \; \backslash xrightarrow\{\backslash Delta\}\backslash \; 2Re\_2O\_7\; +\; 14SO\_2\; \}$