Zhi-qiang Tang, Ling-wen Liao, Yong-li Zheng, Jing Kang, Yan-xia Chen. Temperature Effect on Hydrogen Evolution Reaction at Au Electrode[J]. Chinese Journal of Chemical Physics , 2012, 25(4): 469-474. doi: 10.1088/1674-0068/25/04/469-474
Citation: Zhi-qiang Tang, Ling-wen Liao, Yong-li Zheng, Jing Kang, Yan-xia Chen. Temperature Effect on Hydrogen Evolution Reaction at Au Electrode[J]. Chinese Journal of Chemical Physics , 2012, 25(4): 469-474. doi: 10.1088/1674-0068/25/04/469-474

Temperature Effect on Hydrogen Evolution Reaction at Au Electrode

doi: 10.1088/1674-0068/25/04/469-474
Funds:  This work was supported by one Hundred Tal-ents' Program of the Chinese Academy of Science, the National Natural Science Foundation of China (No.21073176), and 973 Program from the Ministry ofScience and Technology of China (No.2010CB923302).
  • Received Date: 2012-05-08
  • The temperature dependence of hydrogen evolution reaction (HER) at a quasi-single crys-talline gold electrode in both 0.1 mol/L HClO4 and 0.1 mol/L KOH solutions was investigated by cyclic voltammetry. HER current displays a clear increase with reaction overpotential (η) and temperature from 278~333 K. In 0.1 mol/L HClO4 the Tafel slopes are found to increases slightly with temperature from 118 mV/dec to 146 mV/dec, while in 0.1 mol/L KOH it is ca. 153±15 mV/dec without clear temperature-dependent trend. The apparent activation energy (Ea) for HER at equilibrium potential is ca. 48 and 34 kJ/mol in 0.1 mol/L HClO4 and 0.1 mol/L KOH, respectively. In acid solution, Ea decreases with increase in η, from Ea=37 kJ/mol (η=0.2 V) to 30 kJ/mol (η=0.35 V). In contrast, in 0.1 mol/L KOH, Ea does not show obvious change with η. The pre-exponential factor (A) in 0.1 mol/L HClO4 is ca. 1 order higher than that in 0.1 mol/L KOH. Toward more negative potential, in 0.1 mol/L HClO4 A changes little with potential, while in 0.1 mol/L KOH it displays a monotonic increase with η. The change trends of the potential-dependent kinetic parameters for HER at Au electrode in 0.1 mol/L HClO4 and that in 0.1 mol/L KOH are discussed.
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Temperature Effect on Hydrogen Evolution Reaction at Au Electrode

doi: 10.1088/1674-0068/25/04/469-474
Funds:  This work was supported by one Hundred Tal-ents' Program of the Chinese Academy of Science, the National Natural Science Foundation of China (No.21073176), and 973 Program from the Ministry ofScience and Technology of China (No.2010CB923302).

Abstract: The temperature dependence of hydrogen evolution reaction (HER) at a quasi-single crys-talline gold electrode in both 0.1 mol/L HClO4 and 0.1 mol/L KOH solutions was investigated by cyclic voltammetry. HER current displays a clear increase with reaction overpotential (η) and temperature from 278~333 K. In 0.1 mol/L HClO4 the Tafel slopes are found to increases slightly with temperature from 118 mV/dec to 146 mV/dec, while in 0.1 mol/L KOH it is ca. 153±15 mV/dec without clear temperature-dependent trend. The apparent activation energy (Ea) for HER at equilibrium potential is ca. 48 and 34 kJ/mol in 0.1 mol/L HClO4 and 0.1 mol/L KOH, respectively. In acid solution, Ea decreases with increase in η, from Ea=37 kJ/mol (η=0.2 V) to 30 kJ/mol (η=0.35 V). In contrast, in 0.1 mol/L KOH, Ea does not show obvious change with η. The pre-exponential factor (A) in 0.1 mol/L HClO4 is ca. 1 order higher than that in 0.1 mol/L KOH. Toward more negative potential, in 0.1 mol/L HClO4 A changes little with potential, while in 0.1 mol/L KOH it displays a monotonic increase with η. The change trends of the potential-dependent kinetic parameters for HER at Au electrode in 0.1 mol/L HClO4 and that in 0.1 mol/L KOH are discussed.

Zhi-qiang Tang, Ling-wen Liao, Yong-li Zheng, Jing Kang, Yan-xia Chen. Temperature Effect on Hydrogen Evolution Reaction at Au Electrode[J]. Chinese Journal of Chemical Physics , 2012, 25(4): 469-474. doi: 10.1088/1674-0068/25/04/469-474
Citation: Zhi-qiang Tang, Ling-wen Liao, Yong-li Zheng, Jing Kang, Yan-xia Chen. Temperature Effect on Hydrogen Evolution Reaction at Au Electrode[J]. Chinese Journal of Chemical Physics , 2012, 25(4): 469-474. doi: 10.1088/1674-0068/25/04/469-474

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