The threat of global warming is high due to the extensive use of fossil fuels.Using non-renewable resources is a viable solution. Sunlight can be converted in two ways - into electrical energy and into chemical energy. Water splitting and CO2 are two important methods which can be used in solar cells.
2. Introduction
The threat of global warming is high due to the extensive use of fossil fuels.
Using non-renewable resources is a viable solution.
Sunlight can be converted in two ways - into electrical energy and into chemical
energy
Water splitting and CO2 are two important methods which can be used in solar cells.
3. Artificial Photosynthesis
The basic process can be split into four steps:
Generation of charge carriers (electron–hole pairs) upon absorption of photons with
suitable energy from light irradiation
Charge carrier separation and transportation
Adsorption of chemical species on the surface of the photocatalyst
Chemical reactions between adsorbed species and charge carriers
4. Pictorial representation of Artificial
photosynthesis
Courtesy of Toshisba Corporate Research & Development Center
Fig 1: Mechanism of Artificial photosynthesis
5. Photocatalysis
A good photocatalytic material should be able to-
Separate electron - hole pairs generated and prevent recombination.
Transfer electrons to the surface for chemical reaction
Provide catalytic surface for the chemical reaction to take place.
Materials which generate catalytic activity when exposed to light are
called photocatalysts.
6. Possible Redox reactions
Chem. Commun., 2016, 52, 35; DOI: 10.1039/c5cc07613g
Table 1: Some possible reactions related to photocatalytic conversion of CO2 with H2O
7. Drawbacks
Mismatch between the absorption ability of semiconductor and the solar spectrum
Charge recombination or poor charge carrier separation
Low solubility of CO2 in water (approximately 33 µmol in 1 ml of water at 100 KPa and room
temperature)
Problem of back reactions during CO2 reduction
Water reduction to hydrogen is a competing reaction
8. TiO2 as Photocatalyst
High efficiency in UV irradiation.
Wide availability
Lack of Toxicity
Durability and Stability
Easy to synthesize at nanoscale (TiO2 nanotubes)
The PROBLEM?
Lack of Photo-response under visible light irradiation
Avelino Corma , Hermenegildo Garcia; Photocatalytic reduction of CO2 for fuel production: Possibilities and Challenges; Journal of Catalysis 308 (2013) 168–175
9. TiO2 - Modifications
• Retarding fast charge recombination
• Reducing the band gap: improving
photoresponse
Doping
&
Creating Heterojunction
• Selectivity towards a single product
• Increasing the recombination time:
Permanent effect
• Solution to photocorrosion
Loading a
Co-catalyst
Eg: Au/Ag NPs on TiO2
10. 1. Doping
Metallic Non-Metallic
Replacing Ti4+ by Fe3+, Pt4+ or Pd2+
Photocorrosion- Leaching and deactivation
Replacing Oxygen/Oxygen vacancies by C, N
or S
More stable TiO2 photocatalysts
Reproducibility problems due to variation in dopant concentrations and its location.
1) A. Fujishima, X. Zhang, D.A. Tryk, Surf. Sci. Rep. 63 (2008) 515–582.
2) C. Burda, Y.B. Lou, X.B. Chen, A.C.S. Samia, J. Stout, J.L. Gole, Nano Lett. 3 (2003) 1049–1051.
11. 2. Forming a Heterojunction
Fig 2: Schematic Representation of ‘surface
heterojunction’ effect in TiO2 , {001} and {101} facets
Improve light absorption and charge separation
Autonomous effect: due to the field generated
Semiconducting QDs can be used to create
heterojunctions
Results in better visible light response
J. Yu, J. Low, W. Xiao, P. Zhou and M. Jaroniec, J. Am. Chem. Soc., 2014, 136, 8839–8842.
12. 3. Loading a Co- Catalyst
Fig 3: Proposed mechanism for the photocatalytic hydrogen generation assisted by
Au NPs on the TiO2 surface
Surface plasmon band characteristic: Absorption of visible light
Supplying e- s to the CB of TiO2
State of charge separation
Reproducibility X Water oxidation X Redundant reactions Product Selectivity
Avelino Corma , Hermenegildo Garcia; Photocatalytic reduction of CO2 for fuel production: Possibilities and Challenges; Journal of Catalysis 308 (2013) 168–175
13. Desirable properties
Int. J. Mol. Sci. 2014, 15, 5246-5262; doi:10.3390/ijms15045246
How to accomplish the property Property Effect
Small particle size High surface area High adsorption
Crystalline material Single site structure Homogeneity
Engineering the band gap Light absorption Higher efficiency
Preferential migration along
certain direction
Efficient charge separation Low recombination
Presence of co-catalysts Long lifetime of charge separation Possibility of chemical reactions
High crystallinity High mobility of charge carriers More efficient charge separation
Adequate co-catalysts Selectivity towards single product Efficient chemical process
Table 2: Compendium of all the desired properties and necessary modifications for efficient photocatalysis.
14. TiO2 nanotubes via anodization
Titanium foils - degreased using acetone, methanol, rinsed with DI water and blow
dried
Ethylene glycol + Ammonium fluoride is used as electrolyte, Pt as counter electrode
Electrochemical anodization carried out at 50V for 3 hours
Annealed at around 450℃ for 2 hours for obtaining the crystalline phase
Free standing nanotubes can also be obtained by methanol evaporation
Chem. Mater. 2008, 20, 1257–1261
15. Biomaterials and Biotechnology Schemes Utilizing TiO2 Nanotube Arrays, By Karla S. Brammer, Seunghan Oh, Christine J. Frandsen and
Sungho Jin ISBN 978-953-307-609-6, Published: September 15, 2011
Anodization mechanism
Fig 4: Schematic illustration of TiO2 nanotube formation
16. Fig 5: Schematic of experimental setup
Nanoscale, 2014, 6, 14305; DOI: 10.1039/c4nr05371k
CO2 photoreduction experiment
17. CO2 Photoreduction experiment
Before the start of the experiment the steel chamber is heated to 80℃ to remove
the desorbed gases
Photocatalyst is kept inside a steel chamber along with water droplets covered with
an optical grade Quartz window
The chamber is vacuumed and desired pressure of CO2 is filled
The solar simulator is switched on to irradiate the sample for a period of time
After the experiment is over, the output valve can be connected to Mass
Spectrometer to analyse the reaction products
Nanoscale, 2014, 6, 14305; DOI: 10.1039/c4nr05371k
18. Conclusion and further work
The efficiency of artificial photocatalysis is generally lower than in natural
photosynthesis
Alcohols/amines can be used in place of water to generate H+ ions
Need for optimal catalyst for CO2 reduction to be applied commercially
Lack of a single measure of efficiency which would allow for an unequivocal
comparison of heterogeneous photocatalytic systems
In-situ spectroscopic techniques for understanding elementary steps
Developing efficient co-catalysts for activation and selective reduction of CO2
Hinweis der Redaktion
One of the reasons for this low efficiency associated with the use of TiO2 could be the low reduction potential of electrons in its conduction band (-0.1 V) that ismuch lower than the theoretical thermodynamics requirements for one electron reduction of CO2
Band gap engineering has to be done
Surface heterojunction: concept is proposed on the basis of the DFT calculations to explain the difference in the photocatalytic
activity of anatase TiO2 with coexposed {001} and {101} facets.
Bi-crystalline TiO2 : Brookite and Anatase show improved photocatalytic activity.
>Some metal NPs, such as gold, silver and copper, when of appropriate size and morphology, exhibit absorption bands in the visible region as a consequence of the collective oscillation of electrons on the surface of the NPs (“surface plasmon band”). In particular, the surface plasmon band absorption of Au NPs appears as a very broad band at λ max around 560 nm expanding from 400 to 700 nm
>To reduce CO2 into carbon monoxide or hydrocarbons, electrons in the semiconductor are required to have more negative chemical potential and for water oxidation, holes need to have more positive potential
Glycerol (6% ethylene glycol, 5% NH4F) + 15% DI water
N atoms were doped into TiO2NTs by a facile hydrothermal method. The hydrothermal process was subsequently conducted at 120 °C for 12 h and then the autoclave was cooled to room temperature naturally
An appropriate amount of H2PtCl6·6H2O solution based on Pt content in the sample (0.05, 0.1 and 0.2 wt.%) was mixed with TO-NP in distilled flask. The resulting slurry was stirred in the rotary dryer at 333 K for 2 h and maintained at 363 K for 30 min to evaporate the water completely. The solid residue is further dried at 383 K for 12 h and calcined in air at 773 K for 2 h.
Anodic Reaction: Ti + 2H2O TiO2 + 4H+ + 4e-
Chemical dissolution: TiO2 + 4H+ + 6F- TiF62- + 2H2O
Before anodization, a nano scale TiO2 passivation layer is on the Ti surface.
When constant voltage is applied, a pit is formed on the TiO2 layer.
As anodization time increases, the pit grows longer and larger, and then it becomes a nanopore.
Nanopores and small pits undergo continuous barrier layer formation. (e) After specific anodization time, completely developed nanotubes are formed on the Ti surface.
In general, the mechanism of TiO2 nanotube formation in fluorine-ion based electrolytes is said to occur as a result of three simultaneous processes: the field assisted oxidation of Ti metal to form titanium dioxide, the field assisted dissolution of Ti metal ions in the electrolyte, and the chemical dissolution of Ti and TiO2 due to etching by fluoride ions, which is enhanced by the presence of H+ions (Shankar et al. 2007). TiO2 nanotubes are not formed on the pure Ti surface but on the thin TiO2oxide layer naturally present on the Ti surface. Therefore, the mechanism of TiO2 nanotubes formation is related to oxidation and dissolution kinetics. Schematic diagram of the formation of TiO2nanotubes by anodization process is shown in Figure 1. For a description of the process displayed inFigure 1, the anodization mechanism for creating the nanotube structure is as follows:
The in situ monitoring of the surface reaction intermediates, the investigation of the rate
limiting step and the process dynamics of adsorption and desorption of these species finally
should lead to the synthesis of new photocatalysts with higher efficiency, selectivity, long-term
stability and economic competitiveness
more effort should be put into the design of
co-catalysts that are able to enhance the chemisorption of CO2
from the mixture of CO2 and H2O, to activate CO2 molecules
preferentially and to catalyze the product formation with controllable selectivity.
The lack of a single measure of efficiency which wouldallow for an unequivocal comparison of heterogeneousphotocatalytic systems has to be considered as a seriousimpediment to advancing the field. The situation could bepartially ameliorated by standardizing the experimentalconditions as well as by publishing at least two of the popularmeasures, one related to the amount of the catalyst (e.g.formation rate) and one related to the strength of theillumination (e.g. photonic efficiency). An alternative wouldbe to devise a new measure that encompasses both relationships. Both approaches would be valuable steps forward fora consistent assessment of the efficiency of any system withrespect to others and thereby enable identification of the bestperforming ones and paths for further improvement.