\u767a\u8868\u8ad6\u6587<\/h3>\n2014\u5e74<\/h4>\n\n\n- “Bimodal Cesium hydrogen Salts of 12-Tungstosilicic Acid, Csx<\/sub>H4-x<\/sub>SiW12O40, as Highly Active Solid Acid Catalysts for Transesterification of Glycerol Tributyrate with Methanol”<\/b>
\n Yukari Iwase, Shogo Sano, Lina Mahardiani, Ryu Abe, Yuichi Kamiya
Journal of Catalysis<\/i>, 318 (2014) 34-42. DOI:10.10161\/j.jcat.2014.07.008<\/a>
Abstract<\/b>
![\"\"](\"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-content\/uploads\/2021\/05\/J_Cata.jpg\")
Bimodal Csx<\/sub>H4-x<\/sub>[SiW12<\/sub>O40<\/sub>] (Csx<\/i>-bimodal<\/b>) with mesopores interconnected with micropores were synthesized from microporous Csx<\/sub>H4-x<\/sub>[SiW12<\/sub>O40<\/sub>] (Csx<\/i>-micro<\/b>) with x = 1.0-2.5, which were prepared in advance by titrating an aqueous solution of H4<\/sub>[SiW12<\/sub>O40<\/sub>] with an aqueous solution of Cs2<\/sub>CO3<\/sub>, followed by treatment in refluxing ethanol to mainly dissolve the H4<\/sub>[SiW12<\/sub>O40<\/sub>] in the particles. Mesopore size distributions and their pore volumes changed depending on x inCsx<\/i>-micro<\/b>. MicroporousCs2.5-micro<\/b>transformed into bimodalCs2.5-bimodal<\/b>with mesopores having average diameters of 3.7 nm and large mesopore volumes. AlthoughCs2.5-bimodal<\/b>exhibited only low catalytic activity for the decomposition of isopropyl acetate, post-treatment in H2<\/sub>SO4<\/sub>enhanced the catalytic activity due to substitution of the Cs+<\/sup>ions on the surface with H+<\/sup>. H2<\/sub>SO4<\/sub>-treatedCsx<\/i>-bimodal<\/b>showed high activity toward transesterification of glyceryl tributyrate with methanol due to its strong acid strength and mesoporosity.<\/li>\n- “Combining the photocatalyst Pt\/TiO2<\/sub>and the Non-photocatalyst SnPd\/Al2<\/sub>O3<\/sub>for Effective Photocatalytic Purification of Groundwater Polluted with Nitrate”<\/b>
Jun Hirayama, Yuichi Kamiya
ACS Catalysis<\/i>, 4 (2014) 2207-2215. DOI:
\n 10.1021\/cs5003564<\/a>
Abstract<\/b>
![\"\"](\"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-content\/uploads\/2021\/05\/1.jpg\")
We investigated photocatalytic reduction of NO3<\/sub>–<\/sup>in real groundwater in the presence of the photocatalyst Pt\/TiO2<\/sub>and the nonphotocatalyst SnPd\/Al2<\/sub>O3<\/sub>, which were dispersed in the groundwater, under irradiation at \u03bb > 300 nm, with glucose as a hole scavenger. In this system, photocatalytic H2<\/sub>evolution (2H+<\/sup>+ 2e<\/i>–<\/sup>\u2192 H2<\/sub>) proceeded over Pt\/TiO2<\/sub>, and nonphotocatalytic, that is, conventional catalytic, reduction of NO3<\/sub>–<\/sup>with H2<\/sub>(NO3<\/sub>–<\/sup>+ 5\/2H2<\/sub>\u2192 1\/2N2<\/sub>+ 2H2<\/sub>O + OH–<\/sup>) occurred over SnPd\/Al2<\/sub>O3<\/sub>. NO3<\/sub>–<\/sup>(1.0 mmol dm-3<\/sup>) in the groundwater completely and selectively decomposed to N2<\/sub>(yield 83%) after 120 h with a 300 W Xe lamp (\u03bb > 300 nm) over the Pt\/TiO2<\/sub>?SnPd\/Al2<\/sub>O3<\/sub>system in combination with photooxidative pretreatment of the groundwater over Pt\/TiO2<\/sub>to decompose organic compounds. The decomposition rate of NO3<\/sub>–<\/sup>in the groundwater was still slower than that in an aqueous NO3<\/sub>–<\/sup>solution even after the pretreatment of the groundwater. The lower photocatalytic performance was due to poisoning of Pt\/TiO2<\/sub>with sulfate and silicate ions and poisoning of SnPd\/Al2<\/sub>O3<\/sub>with polymerized silicate ions. On the other hand, cations, including Na+<\/sup>, K+<\/sup>, Mg2+<\/sup>, and Ca2+<\/sup>, in the groundwater did not affect the photocatalytic and catalytic performances of the system. Sulfate ions adsorbed on the Pt sites on Pt\/TiO2<\/sub>, where H2<\/sub>evolution occurs, and silicate ions deactivated the oxidation sites on TiO2<\/sub>by reacting with the surface hydroxyl groups, leading to a decline in the photocatalytic performance of Pt\/TiO2<\/sub>.\n <\/li>\n- “Catalytic oxidation of ammonium ion in water with ozone over metal oxide catalysts”<\/b>
Sho-ichi Ichikawa, Lina Mahardiani, Yuichi Kamiya
Catal. Today.<\/i>, 232 (2014) 192-197. DOI:10.1016\/j.cattod.2013.09.039<\/a>
Abstract<\/b>
![\"\"](\"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-content\/uploads\/2021\/05\/Cata_today.jpg\")
Oxidative decomposition of NH4<\/sub>+<\/sup>(10 mmol L-1<\/sup>) with O3<\/sub>in water was studied at 333 K over a variety of metal oxide catalysts without pH control of the solution. Although MgO and NiO had the highest catalytic activities, large amounts of undesired NO3<\/sub>–<\/sup>formed due to low selectivity to gaseous products as well as high activity. Co3<\/sub>O4<\/sub>, which was slightly less active than MgO and NiO, was the best catalyst in terms of activity, selectivity to gaseous products, and dissolution degree among the metal oxide catalysts studied. Over Co3<\/sub>O4<\/sub>, NH4<\/sub>+<\/sup>was selectively oxidized to N2<\/sub>with 88% selectivity in water, and the dissolution degree of Co3<\/sub>O4<\/sub>was less than 1%. Fe2<\/sub>O3<\/sub>, SnO2<\/sub>, Mn3<\/sub>O4<\/sub>, CuO, MgO, and Al2<\/sub>O3<\/sub>were less selective to gaseous products or much less active for the reaction. The selectivities to gaseous products were strongly related to the standard enthalpy changes of formation per mol of oxygen atom (\u0394H<\/i>0<\/sup>1<\/sub>) of the metal oxides. The metal oxide catalysts with low \u0394H<\/i>0<\/sup>1<\/sub>, like Co3<\/sub>O4<\/sub>, showed high selectivity to gaseous products probably due to the low surface density of the active oxygen formed from O3<\/sub>on the catalysts. Chloride ions (Cl–<\/sup>) present in the reaction solution significantly accelerated the reaction rate for NH4<\/sub>+<\/sup>decomposition with O3<\/sub>in the presence of Co3<\/sub>O4<\/sub>. This was due to the involvement of Cl–<\/sup>in the catalytic cycle. For instance, ClO–<\/sup>, which may form by the reaction of Cl–<\/sup>with O3<\/sub>over Co3<\/sub>O4<\/sub>, could further oxidize NH4<\/sub>+<\/sup>.<\/li>\n- “Combinational effect of Pt\/SrTiO3<\/sub>:Rh photocatalyst and SnPd\/Al2<\/sub>O3<\/sub>non-photocatalyst for photocatalytic reduction of nitrate to nitrogen in water under visible light irradiation”<\/b>
Jun Hirayama, Ryu Abe, Yuichi Kamiya
Appl. Catal. B.<\/i>, 144 (2014) 721-729. DOI:10.1016\/j.apcatb.2013.08.005<\/a>
Abstract<\/b>
![\"\"](\"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-content\/uploads\/2021\/05\/App_Cata.jpg\")
Photocatalytic reduction of nitrate in water in the co-presence of Pt\/SrTiO3<\/sub>:Rh and SnPd\/Al2<\/sub>O3<\/sub>under visible light irradiation (\u03bb > 420 nm) was investigated. This reaction system efficiently and selectively promoted the photocatalytic reduction of nitrate to nitrogen, whereas Pt\/SrTiO3<\/sub>:Rh or SnPd\/Al2<\/sub>O3<\/sub>alone showed little activity under the reaction conditions. The selectivity to N2 was 94% under the optimum reaction conditions, where the amounts of Pt\/SrTiO3<\/sub>:Rh and SnPd\/Al2<\/sub>O3<\/sub>loaded in the reaction system were 500 mg and 150 mg, respectively. This reaction system showed a superior nitrate decomposition rate and superior selectivity to nitrogen compared with SrTiO3<\/sub>:Rh directly modified with SnPd bimetal. From analysis of the reaction mechanism, hydrogen formed by photoreduction of water over Pt\/SrTiO3<\/sub>:Rh acted as the reductant for a non-photocatalytic nitrate conversion reaction over SnPd\/Al2<\/sub>O3<\/sub>. Moreover, the products, including formaldehyde and formic acid, formed by photo-oxidation of methanol over Pt\/SrTiO3<\/sub>:Rh acted as reductants for nitrate over SnPd\/Al2<\/sub>O3<\/sub>.<\/li>\n<\/ul>\n<\/div>\n\u5b66\u4f1a\u767a\u8868<\/h3>\n2014\u5e74\u5ea6<\/h4>\n\n\n- \u7b2c115\u56de\u89e6\u5a92\u8a0e\u8ad6\u4f1a\uff083\u670823\u65e5\uff5e24\u65e5\u3001\u6771\u4eac\uff09<\/b>
\n \uff08\u30dd\u30b9\u30bf\u30fc\u767a\u8868\uff09\u795e\u8c37\u3000\u201c\u6c34\u4e2dNH4<\/sub>+<\/sup>\u306e\u9178\u5316\u5206\u89e3\u53cd\u5fdc\u3078\u306e\u9178\u5316\u30b3\u30d0\u30eb\u30c8\u89e6\u5a92\u306e\u53cd\u5fa9\u4f7f\u7528\u306b\u3088\u308b\u6d3b\u6027\u5411\u4e0a\u52b9\u679c\u201d<\/li>\n- \u5316\u5b66\u7cfb\u5b66\u5354\u4f1a\u5317\u6d77\u9053\u652f\u90e82015\u5e74\u51ac\u5b63\u7814\u7a76\u767a\u8868\u4f1a\uff081\u670827\u65e5\uff5e28\u65e5\u3001\u672d\u5e4c\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u5c71\u672c\u3000\u201c\u6c34\u4e2d\u785d\u9178\u30a4\u30aa\u30f3\u5149\u9084\u5143\u5206\u89e3\u306b\u5bfe\u3059\u308bSn-Pd\/SrTiO3<\/sub>:Rh\u306e\u6027\u80fd\u652f\u914d\u56e0\u5b50\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u91ce\u5cf6\u3000\u201c\u5730\u4e0b\u6c34\u6d44\u5316\u306e\u305f\u3081\u306e\u62c5\u6301\u30cb\u30c3\u30b1\u30eb\u89e6\u5a92\u306b\u3088\u308b\u6c34\u4e2d\u785d\u9178\u30a4\u30aa\u30f3\u9084\u5143\u5206\u89e3\u201d<\/li>\n- \u7b2c45\u56de\u4e2d\u90e8\u5316\u5b66\u95a2\u4fc2\u5b66\u5354\u4f1a\u652f\u90e8\u9023\u5408\u79cb\u5b63\u5927\u4f1a(11\u670829\u65e5\uff5e30\u65e5\u3001\u6625\u65e5\u4e95\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u5b89\u7530\u3000\u201c\u62c5\u6301\u91d1\u5c5e\u9178\u5316\u7269\u89e6\u5a92\u306b\u3088\u308b\u9178\u7d20\u5171\u5b58\u4e0b\u3067\u306e\u6c34\u4e2d\u4e9c\u785d\u9178\u30a4\u30aa\u30f3\u306e\u9078\u629e\u9084\u5143\u5206\u89e3\u201d<\/li>\n- \u7b2c44\u56de\u77f3\u6cb9\u30fb\u77f3\u6cb9\u5316\u5b66\u8a0e\u8ad6\u4f1a(10\u670816\u65e5\uff5e17\u65e5\u3001\u65ed\u5ddd\uff09<\/b>
\n \uff08\u62db\u5f85\u8b1b\u6f14\uff09\u795e\u8c37\u3000\u201cSelective conversion of butenes over silica-supported 12-tungstosilicic acid catalyst\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09Lina\u3000\u201cIncrease in catalytic activity of cobalt oxide by repeated use for oxidative decomposition of ammonia with ozone in water\u201d<\/li>\n- \u7b2c114\u56de\u89e6\u5a92\u8a0e\u8ad6\u4f1a(9\u670825\u65e5\uff5e27\u65e5\u3001\u6771\u5e83\u5cf6\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u798f\u897f\u3000\u201c\u91d1\u5c5e\u9178\u5316\u7269\u89e6\u5a92\u306b\u3088\u308b\u6c34\u4e2d\u30a2\u30cb\u30ea\u30f3\u306e\u30aa\u30be\u30f3\u9178\u5316\u5206\u89e3\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u4fdd\u7530\u3000\u201c12-\u30e2\u30ea\u30d6\u30c9\u30ea\u30f3\u9178\u89e6\u5a92\u4e0a\u3067\u306e\u30e1\u30bf\u30af\u30ed\u30ec\u30a4\u30f3\u9078\u629e\u9178\u5316\u53cd\u5fdc\u306b\u304a\u3051\u308b\u6c34\u84b8\u6c17\u306e\u6dfb\u52a0\u52b9\u679c\u201d<\/li>\n- \u77f3\u6cb9\u5b66\u4f1a\u7b2c57\u56de\u5e74\u4f1a(5\u670827\u65e5\uff5e28\u65e5\u3001\u6771\u4eac\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u795e\u8c37\u3000\u201cTiO2<\/sub>\u304a\u3088\u3073Al2<\/sub>O3<\/sub>\u306b\u52a0\u6301\u3057\u305fH4<\/sub>SiW12<\/sub>O40<\/sub>\u306e\u9178\u6027\u8cea\u201d<\/li>\n- Seminar of Chemistry and Chemical Education \u2165(6\u670821\u65e5\u3001Solo\u3001\u30a4\u30f3\u30c9\u30cd\u30b7\u30a2\uff09<\/b>
\n \uff08\u62db\u5f85\u8b1b\u6f14\uff09\u795e\u8c37\u3000\u201cWater Purification by Catalytic and Photocatalytic Reactions : Nitrate-Polluted Groundwater as an Example\u201d<\/li>\n<\/ul>\n<\/div>\n","protected":false},"excerpt":{"rendered":"\u7814\u7a76\u696d\u7e3e \u7814\u7a76\u696d\u7e3e\u4e00\u89a7\u3078 \u767a\u8868\u8ad6\u6587 2014\u5e74 “Bimodal Cesium hydrogen Salts of 12-Tungstosilici … <\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-282","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/comments?post=282"}],"version-history":[{"count":9,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282\/revisions"}],"predecessor-version":[{"id":3274,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282\/revisions\/3274"}],"wp:attachment":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/media?parent=282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n
- \n
- “Bimodal Cesium hydrogen Salts of 12-Tungstosilicic Acid, Csx<\/sub>H4-x<\/sub>SiW12O40, as Highly Active Solid Acid Catalysts for Transesterification of Glycerol Tributyrate with Methanol”<\/b>
\n Yukari Iwase, Shogo Sano, Lina Mahardiani, Ryu Abe, Yuichi Kamiya
Journal of Catalysis<\/i>, 318 (2014) 34-42. DOI:10.10161\/j.jcat.2014.07.008<\/a>
Abstract<\/b>
Bimodal Csx<\/sub>H4-x<\/sub>[SiW12<\/sub>O40<\/sub>] (Csx<\/i>-bimodal<\/b>) with mesopores interconnected with micropores were synthesized from microporous Csx<\/sub>H4-x<\/sub>[SiW12<\/sub>O40<\/sub>] (Csx<\/i>-micro<\/b>) with x = 1.0-2.5, which were prepared in advance by titrating an aqueous solution of H4<\/sub>[SiW12<\/sub>O40<\/sub>] with an aqueous solution of Cs2<\/sub>CO3<\/sub>, followed by treatment in refluxing ethanol to mainly dissolve the H4<\/sub>[SiW12<\/sub>O40<\/sub>] in the particles. Mesopore size distributions and their pore volumes changed depending on x inCsx<\/i>-micro<\/b>. MicroporousCs2.5-micro<\/b>transformed into bimodalCs2.5-bimodal<\/b>with mesopores having average diameters of 3.7 nm and large mesopore volumes. AlthoughCs2.5-bimodal<\/b>exhibited only low catalytic activity for the decomposition of isopropyl acetate, post-treatment in H2<\/sub>SO4<\/sub>enhanced the catalytic activity due to substitution of the Cs+<\/sup>ions on the surface with H+<\/sup>. H2<\/sub>SO4<\/sub>-treatedCsx<\/i>-bimodal<\/b>showed high activity toward transesterification of glyceryl tributyrate with methanol due to its strong acid strength and mesoporosity.<\/li>\n- “Combining the photocatalyst Pt\/TiO2<\/sub>and the Non-photocatalyst SnPd\/Al2<\/sub>O3<\/sub>for Effective Photocatalytic Purification of Groundwater Polluted with Nitrate”<\/b>
Jun Hirayama, Yuichi Kamiya
ACS Catalysis<\/i>, 4 (2014) 2207-2215. DOI:
\n 10.1021\/cs5003564<\/a>
Abstract<\/b>
We investigated photocatalytic reduction of NO3<\/sub>–<\/sup>in real groundwater in the presence of the photocatalyst Pt\/TiO2<\/sub>and the nonphotocatalyst SnPd\/Al2<\/sub>O3<\/sub>, which were dispersed in the groundwater, under irradiation at \u03bb > 300 nm, with glucose as a hole scavenger. In this system, photocatalytic H2<\/sub>evolution (2H+<\/sup>+ 2e<\/i>–<\/sup>\u2192 H2<\/sub>) proceeded over Pt\/TiO2<\/sub>, and nonphotocatalytic, that is, conventional catalytic, reduction of NO3<\/sub>–<\/sup>with H2<\/sub>(NO3<\/sub>–<\/sup>+ 5\/2H2<\/sub>\u2192 1\/2N2<\/sub>+ 2H2<\/sub>O + OH–<\/sup>) occurred over SnPd\/Al2<\/sub>O3<\/sub>. NO3<\/sub>–<\/sup>(1.0 mmol dm-3<\/sup>) in the groundwater completely and selectively decomposed to N2<\/sub>(yield 83%) after 120 h with a 300 W Xe lamp (\u03bb > 300 nm) over the Pt\/TiO2<\/sub>?SnPd\/Al2<\/sub>O3<\/sub>system in combination with photooxidative pretreatment of the groundwater over Pt\/TiO2<\/sub>to decompose organic compounds. The decomposition rate of NO3<\/sub>–<\/sup>in the groundwater was still slower than that in an aqueous NO3<\/sub>–<\/sup>solution even after the pretreatment of the groundwater. The lower photocatalytic performance was due to poisoning of Pt\/TiO2<\/sub>with sulfate and silicate ions and poisoning of SnPd\/Al2<\/sub>O3<\/sub>with polymerized silicate ions. On the other hand, cations, including Na+<\/sup>, K+<\/sup>, Mg2+<\/sup>, and Ca2+<\/sup>, in the groundwater did not affect the photocatalytic and catalytic performances of the system. Sulfate ions adsorbed on the Pt sites on Pt\/TiO2<\/sub>, where H2<\/sub>evolution occurs, and silicate ions deactivated the oxidation sites on TiO2<\/sub>by reacting with the surface hydroxyl groups, leading to a decline in the photocatalytic performance of Pt\/TiO2<\/sub>.\n <\/li>\n- “Catalytic oxidation of ammonium ion in water with ozone over metal oxide catalysts”<\/b>
Sho-ichi Ichikawa, Lina Mahardiani, Yuichi Kamiya
Catal. Today.<\/i>, 232 (2014) 192-197. DOI:10.1016\/j.cattod.2013.09.039<\/a>
Abstract<\/b>
Oxidative decomposition of NH4<\/sub>+<\/sup>(10 mmol L-1<\/sup>) with O3<\/sub>in water was studied at 333 K over a variety of metal oxide catalysts without pH control of the solution. Although MgO and NiO had the highest catalytic activities, large amounts of undesired NO3<\/sub>–<\/sup>formed due to low selectivity to gaseous products as well as high activity. Co3<\/sub>O4<\/sub>, which was slightly less active than MgO and NiO, was the best catalyst in terms of activity, selectivity to gaseous products, and dissolution degree among the metal oxide catalysts studied. Over Co3<\/sub>O4<\/sub>, NH4<\/sub>+<\/sup>was selectively oxidized to N2<\/sub>with 88% selectivity in water, and the dissolution degree of Co3<\/sub>O4<\/sub>was less than 1%. Fe2<\/sub>O3<\/sub>, SnO2<\/sub>, Mn3<\/sub>O4<\/sub>, CuO, MgO, and Al2<\/sub>O3<\/sub>were less selective to gaseous products or much less active for the reaction. The selectivities to gaseous products were strongly related to the standard enthalpy changes of formation per mol of oxygen atom (\u0394H<\/i>0<\/sup>1<\/sub>) of the metal oxides. The metal oxide catalysts with low \u0394H<\/i>0<\/sup>1<\/sub>, like Co3<\/sub>O4<\/sub>, showed high selectivity to gaseous products probably due to the low surface density of the active oxygen formed from O3<\/sub>on the catalysts. Chloride ions (Cl–<\/sup>) present in the reaction solution significantly accelerated the reaction rate for NH4<\/sub>+<\/sup>decomposition with O3<\/sub>in the presence of Co3<\/sub>O4<\/sub>. This was due to the involvement of Cl–<\/sup>in the catalytic cycle. For instance, ClO–<\/sup>, which may form by the reaction of Cl–<\/sup>with O3<\/sub>over Co3<\/sub>O4<\/sub>, could further oxidize NH4<\/sub>+<\/sup>.<\/li>\n- “Combinational effect of Pt\/SrTiO3<\/sub>:Rh photocatalyst and SnPd\/Al2<\/sub>O3<\/sub>non-photocatalyst for photocatalytic reduction of nitrate to nitrogen in water under visible light irradiation”<\/b>
Jun Hirayama, Ryu Abe, Yuichi Kamiya
Appl. Catal. B.<\/i>, 144 (2014) 721-729. DOI:10.1016\/j.apcatb.2013.08.005<\/a>
Abstract<\/b>
Photocatalytic reduction of nitrate in water in the co-presence of Pt\/SrTiO3<\/sub>:Rh and SnPd\/Al2<\/sub>O3<\/sub>under visible light irradiation (\u03bb > 420 nm) was investigated. This reaction system efficiently and selectively promoted the photocatalytic reduction of nitrate to nitrogen, whereas Pt\/SrTiO3<\/sub>:Rh or SnPd\/Al2<\/sub>O3<\/sub>alone showed little activity under the reaction conditions. The selectivity to N2 was 94% under the optimum reaction conditions, where the amounts of Pt\/SrTiO3<\/sub>:Rh and SnPd\/Al2<\/sub>O3<\/sub>loaded in the reaction system were 500 mg and 150 mg, respectively. This reaction system showed a superior nitrate decomposition rate and superior selectivity to nitrogen compared with SrTiO3<\/sub>:Rh directly modified with SnPd bimetal. From analysis of the reaction mechanism, hydrogen formed by photoreduction of water over Pt\/SrTiO3<\/sub>:Rh acted as the reductant for a non-photocatalytic nitrate conversion reaction over SnPd\/Al2<\/sub>O3<\/sub>. Moreover, the products, including formaldehyde and formic acid, formed by photo-oxidation of methanol over Pt\/SrTiO3<\/sub>:Rh acted as reductants for nitrate over SnPd\/Al2<\/sub>O3<\/sub>.<\/li>\n<\/ul>\n<\/div>\n\u5b66\u4f1a\u767a\u8868<\/h3>\n
2014\u5e74\u5ea6<\/h4>\n
\n- \n
- \u7b2c115\u56de\u89e6\u5a92\u8a0e\u8ad6\u4f1a\uff083\u670823\u65e5\uff5e24\u65e5\u3001\u6771\u4eac\uff09<\/b>
\n \uff08\u30dd\u30b9\u30bf\u30fc\u767a\u8868\uff09\u795e\u8c37\u3000\u201c\u6c34\u4e2dNH4<\/sub>+<\/sup>\u306e\u9178\u5316\u5206\u89e3\u53cd\u5fdc\u3078\u306e\u9178\u5316\u30b3\u30d0\u30eb\u30c8\u89e6\u5a92\u306e\u53cd\u5fa9\u4f7f\u7528\u306b\u3088\u308b\u6d3b\u6027\u5411\u4e0a\u52b9\u679c\u201d<\/li>\n- \u5316\u5b66\u7cfb\u5b66\u5354\u4f1a\u5317\u6d77\u9053\u652f\u90e82015\u5e74\u51ac\u5b63\u7814\u7a76\u767a\u8868\u4f1a\uff081\u670827\u65e5\uff5e28\u65e5\u3001\u672d\u5e4c\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u5c71\u672c\u3000\u201c\u6c34\u4e2d\u785d\u9178\u30a4\u30aa\u30f3\u5149\u9084\u5143\u5206\u89e3\u306b\u5bfe\u3059\u308bSn-Pd\/SrTiO3<\/sub>:Rh\u306e\u6027\u80fd\u652f\u914d\u56e0\u5b50\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u91ce\u5cf6\u3000\u201c\u5730\u4e0b\u6c34\u6d44\u5316\u306e\u305f\u3081\u306e\u62c5\u6301\u30cb\u30c3\u30b1\u30eb\u89e6\u5a92\u306b\u3088\u308b\u6c34\u4e2d\u785d\u9178\u30a4\u30aa\u30f3\u9084\u5143\u5206\u89e3\u201d<\/li>\n- \u7b2c45\u56de\u4e2d\u90e8\u5316\u5b66\u95a2\u4fc2\u5b66\u5354\u4f1a\u652f\u90e8\u9023\u5408\u79cb\u5b63\u5927\u4f1a(11\u670829\u65e5\uff5e30\u65e5\u3001\u6625\u65e5\u4e95\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u5b89\u7530\u3000\u201c\u62c5\u6301\u91d1\u5c5e\u9178\u5316\u7269\u89e6\u5a92\u306b\u3088\u308b\u9178\u7d20\u5171\u5b58\u4e0b\u3067\u306e\u6c34\u4e2d\u4e9c\u785d\u9178\u30a4\u30aa\u30f3\u306e\u9078\u629e\u9084\u5143\u5206\u89e3\u201d<\/li>\n- \u7b2c44\u56de\u77f3\u6cb9\u30fb\u77f3\u6cb9\u5316\u5b66\u8a0e\u8ad6\u4f1a(10\u670816\u65e5\uff5e17\u65e5\u3001\u65ed\u5ddd\uff09<\/b>
\n \uff08\u62db\u5f85\u8b1b\u6f14\uff09\u795e\u8c37\u3000\u201cSelective conversion of butenes over silica-supported 12-tungstosilicic acid catalyst\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09Lina\u3000\u201cIncrease in catalytic activity of cobalt oxide by repeated use for oxidative decomposition of ammonia with ozone in water\u201d<\/li>\n- \u7b2c114\u56de\u89e6\u5a92\u8a0e\u8ad6\u4f1a(9\u670825\u65e5\uff5e27\u65e5\u3001\u6771\u5e83\u5cf6\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u798f\u897f\u3000\u201c\u91d1\u5c5e\u9178\u5316\u7269\u89e6\u5a92\u306b\u3088\u308b\u6c34\u4e2d\u30a2\u30cb\u30ea\u30f3\u306e\u30aa\u30be\u30f3\u9178\u5316\u5206\u89e3\u201d
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u4fdd\u7530\u3000\u201c12-\u30e2\u30ea\u30d6\u30c9\u30ea\u30f3\u9178\u89e6\u5a92\u4e0a\u3067\u306e\u30e1\u30bf\u30af\u30ed\u30ec\u30a4\u30f3\u9078\u629e\u9178\u5316\u53cd\u5fdc\u306b\u304a\u3051\u308b\u6c34\u84b8\u6c17\u306e\u6dfb\u52a0\u52b9\u679c\u201d<\/li>\n- \u77f3\u6cb9\u5b66\u4f1a\u7b2c57\u56de\u5e74\u4f1a(5\u670827\u65e5\uff5e28\u65e5\u3001\u6771\u4eac\uff09<\/b>
\n \uff08\u53e3\u982d\u767a\u8868\uff09\u795e\u8c37\u3000\u201cTiO2<\/sub>\u304a\u3088\u3073Al2<\/sub>O3<\/sub>\u306b\u52a0\u6301\u3057\u305fH4<\/sub>SiW12<\/sub>O40<\/sub>\u306e\u9178\u6027\u8cea\u201d<\/li>\n- Seminar of Chemistry and Chemical Education \u2165(6\u670821\u65e5\u3001Solo\u3001\u30a4\u30f3\u30c9\u30cd\u30b7\u30a2\uff09<\/b>
\n \uff08\u62db\u5f85\u8b1b\u6f14\uff09\u795e\u8c37\u3000\u201cWater Purification by Catalytic and Photocatalytic Reactions : Nitrate-Polluted Groundwater as an Example\u201d<\/li>\n<\/ul>\n<\/div>\n","protected":false},"excerpt":{"rendered":"\u7814\u7a76\u696d\u7e3e \u7814\u7a76\u696d\u7e3e\u4e00\u89a7\u3078 \u767a\u8868\u8ad6\u6587 2014\u5e74 “Bimodal Cesium hydrogen Salts of 12-Tungstosilici … <\/p>\n","protected":false},"author":1,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-282","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/comments?post=282"}],"version-history":[{"count":9,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282\/revisions"}],"predecessor-version":[{"id":3274,"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/pages\/282\/revisions\/3274"}],"wp:attachment":[{"href":"https:\/\/www.ees.hokudai.ac.jp\/ems\/staff\/kamiya\/wp-json\/wp\/v2\/media?parent=282"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- \u5316\u5b66\u7cfb\u5b66\u5354\u4f1a\u5317\u6d77\u9053\u652f\u90e82015\u5e74\u51ac\u5b63\u7814\u7a76\u767a\u8868\u4f1a\uff081\u670827\u65e5\uff5e28\u65e5\u3001\u672d\u5e4c\uff09<\/b>
- “Combining the photocatalyst Pt\/TiO2<\/sub>and the Non-photocatalyst SnPd\/Al2<\/sub>O3<\/sub>for Effective Photocatalytic Purification of Groundwater Polluted with Nitrate”<\/b>