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GF-TiO2 20 30 40 50 60 70 80 20 30 40 50 60 70 80 a (Å): b (Å): c (Å): Alpha (°): Beta (°): Gamma (°): 4,5890 4,5890 2,9540 90,0000 90,0000 90,0000 2 theta (degrees) 20 30 40 50 60 70 80 2 theta (degrees) 2 theta (degrees) Figure 6.3. – X-ray diffraction spectra of GF electrode and as-prepared GF@TiO2. 6.1.1.1.1 Electrochemical characterization Besides, the electrochemical characterization in a three electrode cell,of the GF-TiO2 samples expose an inhibition of the hydrogen evolution reaction (HER) (6.1), as it can be seen in Figure 6.4b. The maximum current value for an electrode potential at -0.9 V vs. NHE following the trend [A/g]: GF-HT [-5.8]> GF-P [-4.7]> GF-TiO2 (SNRs) [-3.3]> GF-TiO2 (NPs) [-2.0]> GF-TiO2 (MNRs) [-1.2]. First, focusing on the fact that HER increases from the pristine graphite felt to the plasma treated one it is because an increase on the active surface area, which will favor kinetically HER reaction onto the carbonaceous surface. Next, there is a HER decrease when the amount of TiO2 covering the surface increases which follows the trend: SNRs < NPs < MNRs. It is due to a large bounding energy of atomic hydrogen to rutile TiO2 phase182,195–197, which inhibits a posterior hydrogen formation. Additionally, in case it is only considered the reduction standard potential for the reaction (2.17) (E0 (V2+/V3+) = -0.26 V vs. NHE) all the samples that have titanium dioxide on its surface posses a neglected tendency towards the reaction of hydrogen evolution. GF Crystallographic parameters Crystal system: Space group: Space group number: Tetragonal P42/mnm 136 TiO2 (rutile) pattern Calculated density (g/cm^3): 4,26 Volume of cell (10^6 pm^3): 62,21 Z: 2,00 RIR: 3,45 86 (101) (101) (211) (211) (110) (110)PDF Image | Redox Flow Batteries Vanadium to Earth Quinones
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