. . . . . . . . . . . . . . . . . . . "\u062A\u062D\u0644\u064A\u0644 \u0643\u0647\u0631\u0628\u0627\u0626\u064A \u0644\u0644\u0645\u0627\u0621"@ar . . "1123948581"^^ . . . . . . . . . . . . . . . . . . . . "Electrolysis of water"@en . . "La primera electr\u00F3lisis del agua se llev\u00F3 a cabo el 1 de mayo de 1800 por dos qu\u00EDmicos brit\u00E1nicos William Nicholson (1753-1815) y sir Anthony Carlisle (1768-1840), un par de semanas despu\u00E9s de la invenci\u00F3n por Alessandro Volta de la primera bater\u00EDa el\u00E9ctrica, la pila voltaica (publicaci\u00F3n presentada el 20 de marzo de 1800). Once a\u00F1os antes J. R. Deiman y A. Paets van Troostwijk ya hab\u00EDan logrado una electr\u00F3lisis del agua por medio de una y una botella de Leyden, pero sin ser capaces de interpretar la reacci\u00F3n observada."@es . . . . . "Wasserelektrolyse"@de . "\u6C34\u96FB\u89E3\u662F\u6307\u4EE5\u96FB\u6D41\u901A\u904E\u6C34\u4EE5\u88FD\u9020\u6C2B\u6C23\u8207\u6C27\u6C23\u3002\u6B64\u96FB\u89E3\u7684\u6700\u4F4E\u96FB\u58D3\u9650\u5236\u70BA1.23\u4F0F\u7279\u3002 \u9019\u500B\u5DE5\u5E8F\u53EF\u88FD\u4F5C\u6C2B\u71C3\u6599\u548C\uFF0C\u4F46\u7531\u65BC\u6210\u672C\u554F\u984C\uFF0C\u5927\u90E8\u5206\u4EBA\u5747\u4EE5\u5929\u7136\u6C23\u88FD\u4F5C\u6C2B\u6C23\uFF0C\u4E26\u5F9E\u7A7A\u6C23\u4E2D\u63D0\u53D6\u6C27\u6C23\u3002"@zh . . "L'elettrolisi dell'acqua \u00E8 un processo elettrolitico nel quale il passaggio di corrente elettrica causa la scomposizione dell'acqua in ossigeno ed idrogeno gassoso. Dal punto di vista etimologico, il termine elettrolisi \u00E8 composto dal prefisso elettro- (elettricit\u00E0) e da lisi (separazione). L'etimologia del termine \u00E8 connessa con il meccanismo del processo di elettrolisi dell'acqua, che consiste appunto nel \"rompere\" la molecola di acqua nei suoi elementi costituenti (idrogeno e ossigeno)."@it . . . "L'electr\u00F2lisi de l'aigua \u00E9s la descomposici\u00F3 de l'aigua (H\u2082O) en oxigen (O\u2082) i hidrogen (H\u2082) deguda al pas d'un corrent el\u00E8ctric a trav\u00E9s de l'aigua. Aquest proc\u00E9s electrol\u00EDtic es fa servir en algunes aplicacions industrials quan es necessita obtenir hidrogen. L'electr\u00F2lisi en aigua \"pura\" (destil\u00B7lada) \u00E9s molt baixa, i nom\u00E9s pot succeir degut a l'autoionitzaci\u00F3 de l'aigua. L'aigua destil\u00B7lada t\u00E9 una conductivitat el\u00E8ctrica d'una part per mili\u00F3 respecte de l'aigua de mar. Aquesta conductivitat augmenta molt\u00EDssim quan s'hi afegeix un electr\u00F2lit (com una sal, un \u00E0cid o una base)."@ca . "A Eletr\u00F3lise da \u00E1gua \u00E9 a decomposi\u00E7\u00E3o qu\u00EDmica da \u00E1gua (H2O) em oxig\u00EAnio (O2) e hidrog\u00EAnio (H2) por efeito da passagem de uma corrente el\u00E9ctrica pela \u00E1gua (ver: Separa\u00E7\u00E3o da \u00E1gua). No entanto, este processo eletrol\u00EDtico raramente \u00E9 usado em aplica\u00E7\u00F5es industriais uma vez que o hidrog\u00EAnio pode ser produzido mais acessivelmente atrav\u00E9s de combust\u00EDveis f\u00F3sseis.Uma fonte de energia el\u00E9ctrica est\u00E1 ligada a dois el\u00E9ctrodos (geralmente feitos a partir de alguns metais inertes como a platina ou o a\u00E7o inoxid\u00E1vel, no caso da imagem 1, \u00E9 usada a grafite) que est\u00E3o colocados na \u00E1gua. Se tudo estiver corretamente montado, origina-se hidrog\u00EAnio no c\u00E1todo (o el\u00E9ctrodo ligado ao terminal negativo da fonte de energia) e oxig\u00EAnio no \u00E2nodo (o el\u00E9ctrodo ligado ao terminal positivo da fonte de energia)."@pt . . . . . . . . . "L'\u00E9lectrolyse de l'eau est un proc\u00E9d\u00E9 \u00E9lectrolytique qui d\u00E9compose l'eau (H2O) en dioxyg\u00E8ne et dihydrog\u00E8ne gazeux gr\u00E2ce \u00E0 un courant \u00E9lectrique. La cellule \u00E9lectrolytique est constitu\u00E9e de deux \u00E9lectrodes \u2014 habituellement en m\u00E9tal inerte dans la zone de potentiel et de pH consid\u00E9r\u00E9e, typiquement du groupe du platine \u2014 immerg\u00E9es dans un \u00E9lectrolyte (ici l'eau elle-m\u00EAme) et connect\u00E9es aux p\u00F4les oppos\u00E9s de la source de courant continu."@fr . "59922"^^ . "\u6C34\u96FB\u89E3"@zh . "Electrolysis of water, also known as electrochemical water splitting, is the process of using electricity to decompose water into oxygen and hydrogen gas by electrolysis. Hydrogen gas released in this way can be used as hydrogen fuel, or remixed with the oxygen to create oxyhydrogen gas, which is used in welding and other applications. Electrolysis of water requires a minimum potential difference of 1.23 volts, though at that voltage external heat is required from the environment."@en . . "Elektrolisis air adalah peristiwa penguraian senyawa air (H2O) menjadi oksigen (O2) dan hidrogen gas (H2) dengan menggunakan arus listrik yang melalui air tersebut.Pada katoda, dua molekul air bereaksi dengan menangkap dua elektron, tereduksi menjadi gas H2 dan ion hidrokida (OH-). Sementara itu pada anoda, dua molekul air lain terurai menjadi gas oksigen (O2), melepaskan 4 ion H+ serta mengalirkan elektron ke katode. Ion H+ dan OH- mengalami netralisasi sehingga terbentuk kembali beberapa molekul air. Reaksi keseluruhan yang setara dari elektrolisis air dapat dituliskan sebagai berikut. Gas hidrogen dan oksigen yang dihasilkan dari reaksi ini membentuk gelembung pada elektroda dan dapat dikumpulkan."@in . . . . . . . . . . . "Electr\u00F3lisis del agua"@es . "Unter Wasserelektrolyse versteht man die Zerlegung von Wasser in Wasserstoff und Sauerstoff mit Hilfe eines elektrischen Stromes. Die wichtigste Anwendung dieser Elektrolyse ist die Gewinnung von Wasserstoff. Bisher ist die Wasserstoffgewinnung aus fossilen Energietr\u00E4gern wirtschaftlicher als die Herstellung von Wasserstoff mittels Wasserelektrolyse. Die Wasserelektrolyse wird daher noch selten angewandt."@de . . . . . . "\u0627\u0644\u062A\u062D\u0644\u064A\u0644\u064F \u0627\u0644\u0643\u0647\u0631\u0628\u0627\u0626\u064A\u064F\u0651 \u0644\u0644\u0645\u0627\u0621 \u0647\u0648 \u0639\u0645\u0644\u064A\u0629 \u0625\u062C\u0631\u0627\u0621 \u062A\u062D\u0644\u064A\u0644 \u0643\u0647\u0631\u0628\u0627\u0626\u064A \u0644\u062C\u0632\u064A\u0626\u0627\u062A \u0627\u0644\u0645\u0627\u0621 H2O \u0628\u0641\u0635\u0644\u0647 \u0625\u0644\u0649 \u0645\u0643\u0648\u0646\u0627\u062A\u0647 \u0648\u0647\u064A \u0627\u0644\u0623\u0643\u0633\u062C\u064A\u0646 O2 \u0648\u0627\u0644\u0647\u064A\u062F\u0631\u0648\u062C\u064A\u0646 \u0648\u0630\u0644\u0643 \u0639\u0646 \u0637\u0631\u064A\u0642 \u062A\u0645\u0631\u064A\u0631 \u062A\u064A\u0627\u0631 \u0643\u0647\u0631\u0628\u0627\u0626\u064A \u0641\u064A \u0627\u0644\u0648\u0633\u0637 \u0627\u0644\u0645\u0627\u0626\u064A. \u0648\u062A\u0643\u0648\u0646 \u0627\u0644\u0645\u0639\u0627\u062F\u0644\u0629 \u0643\u0627\u0644\u062A\u0627\u0644\u064A: 2H2O(l)\u27F62H2(g)+O2g"@ar . . . . . . . . . . . . . . . . . . . "\u6C34\u96FB\u89E3\u662F\u6307\u4EE5\u96FB\u6D41\u901A\u904E\u6C34\u4EE5\u88FD\u9020\u6C2B\u6C23\u8207\u6C27\u6C23\u3002\u6B64\u96FB\u89E3\u7684\u6700\u4F4E\u96FB\u58D3\u9650\u5236\u70BA1.23\u4F0F\u7279\u3002 \u9019\u500B\u5DE5\u5E8F\u53EF\u88FD\u4F5C\u6C2B\u71C3\u6599\u548C\uFF0C\u4F46\u7531\u65BC\u6210\u672C\u554F\u984C\uFF0C\u5927\u90E8\u5206\u4EBA\u5747\u4EE5\u5929\u7136\u6C23\u88FD\u4F5C\u6C2B\u6C23\uFF0C\u4E26\u5F9E\u7A7A\u6C23\u4E2D\u63D0\u53D6\u6C27\u6C23\u3002"@zh . . . . . . . "Elektrolisis air adalah peristiwa penguraian senyawa air (H2O) menjadi oksigen (O2) dan hidrogen gas (H2) dengan menggunakan arus listrik yang melalui air tersebut.Pada katoda, dua molekul air bereaksi dengan menangkap dua elektron, tereduksi menjadi gas H2 dan ion hidrokida (OH-). Sementara itu pada anoda, dua molekul air lain terurai menjadi gas oksigen (O2), melepaskan 4 ion H+ serta mengalirkan elektron ke katode. Ion H+ dan OH- mengalami netralisasi sehingga terbentuk kembali beberapa molekul air. Reaksi keseluruhan yang setara dari elektrolisis air dapat dituliskan sebagai berikut."@in . . . . . . . . . . . . . . . . . . . . . . . . . . . "Elettrolisi dell'acqua"@it . . . . . "L'elettrolisi dell'acqua \u00E8 un processo elettrolitico nel quale il passaggio di corrente elettrica causa la scomposizione dell'acqua in ossigeno ed idrogeno gassoso. Dal punto di vista etimologico, il termine elettrolisi \u00E8 composto dal prefisso elettro- (elettricit\u00E0) e da lisi (separazione). L'etimologia del termine \u00E8 connessa con il meccanismo del processo di elettrolisi dell'acqua, che consiste appunto nel \"rompere\" la molecola di acqua nei suoi elementi costituenti (idrogeno e ossigeno)."@it . "3206764"^^ . . . . . . . . . . . "A Eletr\u00F3lise da \u00E1gua \u00E9 a decomposi\u00E7\u00E3o qu\u00EDmica da \u00E1gua (H2O) em oxig\u00EAnio (O2) e hidrog\u00EAnio (H2) por efeito da passagem de uma corrente el\u00E9ctrica pela \u00E1gua (ver: Separa\u00E7\u00E3o da \u00E1gua). No entanto, este processo eletrol\u00EDtico raramente \u00E9 usado em aplica\u00E7\u00F5es industriais uma vez que o hidrog\u00EAnio pode ser produzido mais acessivelmente atrav\u00E9s de combust\u00EDveis f\u00F3sseis.Uma fonte de energia el\u00E9ctrica est\u00E1 ligada a dois el\u00E9ctrodos (geralmente feitos a partir de alguns metais inertes como a platina ou o a\u00E7o inoxid\u00E1vel, no caso da imagem 1, \u00E9 usada a grafite) que est\u00E3o colocados na \u00E1gua. Se tudo estiver corretamente montado, origina-se hidrog\u00EAnio no c\u00E1todo (o el\u00E9ctrodo ligado ao terminal negativo da fonte de energia) e oxig\u00EAnio no \u00E2nodo (o el\u00E9ctrodo ligado ao terminal positivo da fonte de energia). \u00C9 necess\u00E1ria uma enorme quantidade de energia para fazer a electr\u00F3lise da \u00E1gua pura uma vez que esta n\u00E3o \u00E9 boa condutora el\u00E9ctrica. Sem o excesso de energia a electr\u00F3lise da \u00E1gua pura ocorre muito lentamente. Isto deve-se \u00E1 limitada auto-ioniza\u00E7\u00E3o da \u00E1gua: a cada 555 milh\u00F5es de mol\u00E9culas, somente uma se ioniza. A condutividade el\u00E9ctrica da \u00E1gua pura \u00E9 cerca de um milh\u00E3o de vezes menor que a da \u00E1gua do mar. A efic\u00E1cia da electr\u00F3lise da \u00E1gua pode ser aumentada adicionando um electr\u00F3lito (como sal, um \u00E1cido ou uma base) e/ou utilizando eletro catalisadores.Equa\u00E7\u00E3o Qu\u00EDmica:2H2O = 2H2 + O2"@pt . . . . . . . . . . . . . . . . . . . "Elektrolisis air"@in . . . . . . . . . . . . "Electr\u00F2lisi de l'aigua"@ca . . . . "\u00C9lectrolyse de l'eau"@fr . . . . . "Electrolysis of water, also known as electrochemical water splitting, is the process of using electricity to decompose water into oxygen and hydrogen gas by electrolysis. Hydrogen gas released in this way can be used as hydrogen fuel, or remixed with the oxygen to create oxyhydrogen gas, which is used in welding and other applications. Electrolysis of water requires a minimum potential difference of 1.23 volts, though at that voltage external heat is required from the environment."@en . . . . . . . . . . . . . . . . . . . . . "Unter Wasserelektrolyse versteht man die Zerlegung von Wasser in Wasserstoff und Sauerstoff mit Hilfe eines elektrischen Stromes. Die wichtigste Anwendung dieser Elektrolyse ist die Gewinnung von Wasserstoff. Bisher ist die Wasserstoffgewinnung aus fossilen Energietr\u00E4gern wirtschaftlicher als die Herstellung von Wasserstoff mittels Wasserelektrolyse. Die Wasserelektrolyse wird daher noch selten angewandt. Durch den starken Ausbau der Nutzung von erneuerbaren Energien wird davon ausgegangen, dass die Wasserelektrolyse als Bestandteil von Power-to-Gas-Anlagen mittel- bis langfristig eine gro\u00DFe Bedeutung zur Herstellung von Synthesegas erreichen wird. Mit Wasserstoff als Energiespeicher wird die Verstetigung der Stromerzeugung aus erneuerbaren Energien, insbesondere bei Windkraft und Photovoltaik, gef\u00F6rdert, indem \u00DCbersch\u00FCsse von Wind- und Solarstrom chemisch zwischengespeichert werden k\u00F6nnen. Der erzeugte Wasserstoff kann f\u00FCr chemische Prozesse genutzt oder direkt oder nach anschlie\u00DFender Methanisierung als Methan dem Erdgasnetz zugef\u00FChrt werden. Anschlie\u00DFend steht er f\u00FCr verschiedene Anwendungszwecke wie z. B. als Rohstoff f\u00FCr die chemische Industrie (Power-to-Chemicals), als Antriebsenergie von Fahrzeugen, Schiffen und Flugzeugen (Power-to-Fuel) oder f\u00FCr die R\u00FCckverstromung in Gaskraftwerken oder Brennstoffzellen zur Verf\u00FCgung. Die Wasserelektrolyse ist auch als Demonstrationsversuch bedeutsam; dabei wird oft der Hofmannsche Wasserzersetzungsapparat genutzt. Eine weitere Anwendung der Wasserelektrolyse ist die Anreicherung von Deuterium. Ferner ist die Wasserelektrolyse die wichtigste Nebenreaktion vieler technischer Elektrolysen, z. B. der Chloralkali-Elektrolyse."@de . . "L'\u00E9lectrolyse de l'eau est un proc\u00E9d\u00E9 \u00E9lectrolytique qui d\u00E9compose l'eau (H2O) en dioxyg\u00E8ne et dihydrog\u00E8ne gazeux gr\u00E2ce \u00E0 un courant \u00E9lectrique. La cellule \u00E9lectrolytique est constitu\u00E9e de deux \u00E9lectrodes \u2014 habituellement en m\u00E9tal inerte dans la zone de potentiel et de pH consid\u00E9r\u00E9e, typiquement du groupe du platine \u2014 immerg\u00E9es dans un \u00E9lectrolyte (ici l'eau elle-m\u00EAme) et connect\u00E9es aux p\u00F4les oppos\u00E9s de la source de courant continu."@fr . . . . "\u0627\u0644\u062A\u062D\u0644\u064A\u0644\u064F \u0627\u0644\u0643\u0647\u0631\u0628\u0627\u0626\u064A\u064F\u0651 \u0644\u0644\u0645\u0627\u0621 \u0647\u0648 \u0639\u0645\u0644\u064A\u0629 \u0625\u062C\u0631\u0627\u0621 \u062A\u062D\u0644\u064A\u0644 \u0643\u0647\u0631\u0628\u0627\u0626\u064A \u0644\u062C\u0632\u064A\u0626\u0627\u062A \u0627\u0644\u0645\u0627\u0621 H2O \u0628\u0641\u0635\u0644\u0647 \u0625\u0644\u0649 \u0645\u0643\u0648\u0646\u0627\u062A\u0647 \u0648\u0647\u064A \u0627\u0644\u0623\u0643\u0633\u062C\u064A\u0646 O2 \u0648\u0627\u0644\u0647\u064A\u062F\u0631\u0648\u062C\u064A\u0646 \u0648\u0630\u0644\u0643 \u0639\u0646 \u0637\u0631\u064A\u0642 \u062A\u0645\u0631\u064A\u0631 \u062A\u064A\u0627\u0631 \u0643\u0647\u0631\u0628\u0627\u0626\u064A \u0641\u064A \u0627\u0644\u0648\u0633\u0637 \u0627\u0644\u0645\u0627\u0626\u064A. \u0648\u062A\u0643\u0648\u0646 \u0627\u0644\u0645\u0639\u0627\u062F\u0644\u0629 \u0643\u0627\u0644\u062A\u0627\u0644\u064A: 2H2O(l)\u27F62H2(g)+O2g"@ar . . "L'electr\u00F2lisi de l'aigua \u00E9s la descomposici\u00F3 de l'aigua (H\u2082O) en oxigen (O\u2082) i hidrogen (H\u2082) deguda al pas d'un corrent el\u00E8ctric a trav\u00E9s de l'aigua. Aquest proc\u00E9s electrol\u00EDtic es fa servir en algunes aplicacions industrials quan es necessita obtenir hidrogen. L'electr\u00F2lisi en aigua \"pura\" (destil\u00B7lada) \u00E9s molt baixa, i nom\u00E9s pot succeir degut a l'autoionitzaci\u00F3 de l'aigua. L'aigua destil\u00B7lada t\u00E9 una conductivitat el\u00E8ctrica d'una part per mili\u00F3 respecte de l'aigua de mar. Aquesta conductivitat augmenta molt\u00EDssim quan s'hi afegeix un electr\u00F2lit (com una sal, un \u00E0cid o una base)."@ca . . . . . . . . . . . . . . . "La primera electr\u00F3lisis del agua se llev\u00F3 a cabo el 1 de mayo de 1800 por dos qu\u00EDmicos brit\u00E1nicos William Nicholson (1753-1815) y sir Anthony Carlisle (1768-1840), un par de semanas despu\u00E9s de la invenci\u00F3n por Alessandro Volta de la primera bater\u00EDa el\u00E9ctrica, la pila voltaica (publicaci\u00F3n presentada el 20 de marzo de 1800). Once a\u00F1os antes J. R. Deiman y A. Paets van Troostwijk ya hab\u00EDan logrado una electr\u00F3lisis del agua por medio de una y una botella de Leyden, pero sin ser capaces de interpretar la reacci\u00F3n observada."@es . "Eletr\u00F3lise da \u00E1gua"@pt . . . . . . . . . . . . . . . . . . . . . . .