# Photocatalytic Oxidation of Triiodide in UVA-Exposed Dye-Sensitized Solar Cells

Authors: Matthew Carnie; Daniel Bryant; Trystan Watson; David Worsley
Journal: International Journal of Photoenergy
 (2012)

---

## Abstract

UVA irradiation of glass mounted dye-sensitized solar cells without UV filtration causes failure within 400 hours of light exposure. The failure mode is shown to relate to consumption ofI3-, which is directly related to TiO2 photo-catalysis.  The onset of failure is easily determined from electrochemical impedance data where the recombination resistance of the TiO2/electrolyte back reaction drops markedly prior to the onset of degradation. At the point of complete cell failure this impedance value then dramatically increases as there is no longer an interfacial reaction possible between the TiO2 and the I3- depleted electrolyte. Device failure is most rapid for cells under electrical load indicating that the degradation of the electrolyte is related to photogenerated hole production by excitation of the TiO2. Once depleted by UV exposure, the I3- can be regenerated by simple application of a reverse bias which can restore severely UV degraded devices to near original working conditions.


---

## Body

## 1. Introduction

As an alternative to conventional silicon solar cells, dye-sensitized solar cells (DSCs) have been studied for some 20 years [1–3]. The photoelectrode most often used in DSCs is a nanoporous layer of TiO2 sintered onto a conductive glass or metal substrate. The photocatalytic properties of TiO2 are well documented [4–6], and photocatalytic reactions may proceed via several steps [7], the most important of which is the production of electron-hole pairs by direct excitation of the TiO2 with UV light. This results in a redox process, creating radicals which can ultimately result in degradative attack on organic molecules in the vicinity of the TiO2 [8]. Since both the DSC dye and the electrolyte have organic components, both are potentially susceptible to photocatalytic attack. It has been shown, however, that modification of the crystal structure and polarity of the TiO2 surface can impart photocatalytic selectivity leading to the possibility that one component could be degraded more favourably over the other [9, 10].Some notable works have been published on DSC stability [11–19] as well as a comprehensive review published in 2010 [20]. The degradation of cells exposed to UV irradiation has been noted many times, as has a corresponding depletion in I3- from the electrolyte. Depletion of I3- has been observed in DSC cells subjected to outdoor testing as evidenced by an increase in the Nernst diffusion impedance and changes to the cell’s Raman spectra [16], and it has been shown that in extreme cases decreased I3- concentration can cause a reduction in JSC by diffusion limitation [21]. The mechanism of I3- depletion has been suggested as either the sublimation of iodine [11] or perhaps the formation of iodate by reactions with water or other impurities in the electrolyte [22]. It appears, however, that I3- depletion could be as a result of a photoreactions as Sommeling et al. demonstrated that electrolyte bleaching occurred rapidly in illuminated cells held at 85° but did not occur in cells held at 85° and kept in the dark [13]. In DSCs, the photogenerated hole in the TiO2 valence band is said to be quenched by the iodide ion in the electrolyte [14]. However, DSC modules can degrade quickly under UV illumination [23], and the fact that filtering at λ<384 nm improves the stability of a DSC cell [24] suggests that the photocatalytic properties of the TiO2 contribute at least in part to the degradation of the DSC.A number of trends have been reported during long-term and accelerated tests. These include an increase inJSC and a decrease in VOC  [18]. Electrochemical impedance spectroscopy (EIS) has also been used to monitor degradation, and it has been shown that the modelled resistance of the TiO2/electrolyte back reaction decreases concurrently with the decrease in VOC and that the drop in VOC is due to a positive shift in the TiO2 conduction band [25]. This can also explain the increase in JSC, as a positive shift of the conduction band should increase electron injection efficiency [24]. The Nernst diffusion impedance of I3- has been shown to increase as a result of the change of the components of the electrolyte during long-term outdoor testing [16]. It was our primary aim with this work to examine the electrochemical and cell efficiency changes that occur in the early stages of DSCs exposed to UV light in order to determine whether failure was related to electrolyte or dye degradation and whether this resulted from photocatalysis. A key secondary goal was to determine if irradiation of cells under load or at open circuit had an effect since, in many cases, longevity testing is conducted in the latter condition. In order to achieve these aims, we have developed some rapid testing methods building on the electrochemical methods proposed by others [13, 14, 18, 25] and using a spectrophotometric method to determine degradation rates of dye and electrolyte in situ without the need for destruction of the cells. We have then used these systems to examine the effectiveness of some UV filtration and in terms of a potential method to revive cells that have been partially photodegraded.


## 2. Experimental

### 2.1. Cell Preparation

The photoanode was prepared by the doctor blading of a commercial TiO2 paste (DSL 18NRT (Dyesol)) onto Solaronix TCO22-15 fluorine-doped SnO2 glass followed by sintering at 500°C for 30 minutes giving a 7 μm dry film thickness. The counter electrodes were prepared by the deposition of 5 mM chloroplatinic acid and heat-treated at 400°C for 30 minutes. N719 dye was prepared at 0.3 mM in a 1 : 1 acetonitrile/T-butanol solution. Adsorption of the dye to the TiO2 was achieved by immersion of the electrode in the dye solution over a period of 16–20 hours. 50 μm Surlyn gaskets were used to separate the electrodes and an electrolyte solution (0.8 M 1-propyl-3-methylimidazolium iodide (PMII), 0.3 M benzimidazole, 0.1 M I2, and 0.05 M guanidinium thiocyanate dissolved in N-methoxy propionitrile) was then introduced to the cell by vacuum injection. All test cells were made with a working electrode area of 1 cm2 except those cells used for UV-Vis measurements which had a working electrode area of 6.25 cm2, and the larger cells were needed in order to completely cover the sample aperture of the spectrophotometer.


### 2.2. Measurements

Photovoltaic characterisation was carried out using an Oriel Sol3A (94023A) utilizing a xenon arc lamp, an AM 1.5 filter, and a Keithley 2400 source meter. A reference measurement was provided using a monocrystalline silicon reference cell traceable to the National Renewable Energy Laboratory (NREL) that enabled adjustment of the solar simulator to the standard light intensity of one sun that is, 100 mW/cm2.Impedance spectroscopy measurements were carried out on a Solartron SI 1280 Electrochemical Measurement Unit using ZPlot software. Cells were measured in a two-electrode setup in the dark. All cell measurements in this study were conducted with a bias potential of −0.68 V, and the corresponding resistance values were averaged for the cell sets in question. AC amplitude was ±10 mV with a frequency range of 20 kHz to 0.1 Hz.UV exposure was conducted using a custom-made bank of 6 × 8 W UVA lamps held 5 cm above the test cells. Measured intensity of the UV lamps was 0.64 Wm−2 at a λmax of 354 nm. This is of comparable UV intensity to ASTM G173−03 (2008) which is given as 0.61 Wm−2 at 354 nm [26].


## 2.1. Cell Preparation

The photoanode was prepared by the doctor blading of a commercial TiO2 paste (DSL 18NRT (Dyesol)) onto Solaronix TCO22-15 fluorine-doped SnO2 glass followed by sintering at 500°C for 30 minutes giving a 7 μm dry film thickness. The counter electrodes were prepared by the deposition of 5 mM chloroplatinic acid and heat-treated at 400°C for 30 minutes. N719 dye was prepared at 0.3 mM in a 1 : 1 acetonitrile/T-butanol solution. Adsorption of the dye to the TiO2 was achieved by immersion of the electrode in the dye solution over a period of 16–20 hours. 50 μm Surlyn gaskets were used to separate the electrodes and an electrolyte solution (0.8 M 1-propyl-3-methylimidazolium iodide (PMII), 0.3 M benzimidazole, 0.1 M I2, and 0.05 M guanidinium thiocyanate dissolved in N-methoxy propionitrile) was then introduced to the cell by vacuum injection. All test cells were made with a working electrode area of 1 cm2 except those cells used for UV-Vis measurements which had a working electrode area of 6.25 cm2, and the larger cells were needed in order to completely cover the sample aperture of the spectrophotometer.


## 2.2. Measurements

Photovoltaic characterisation was carried out using an Oriel Sol3A (94023A) utilizing a xenon arc lamp, an AM 1.5 filter, and a Keithley 2400 source meter. A reference measurement was provided using a monocrystalline silicon reference cell traceable to the National Renewable Energy Laboratory (NREL) that enabled adjustment of the solar simulator to the standard light intensity of one sun that is, 100 mW/cm2.Impedance spectroscopy measurements were carried out on a Solartron SI 1280 Electrochemical Measurement Unit using ZPlot software. Cells were measured in a two-electrode setup in the dark. All cell measurements in this study were conducted with a bias potential of −0.68 V, and the corresponding resistance values were averaged for the cell sets in question. AC amplitude was ±10 mV with a frequency range of 20 kHz to 0.1 Hz.UV exposure was conducted using a custom-made bank of 6 × 8 W UVA lamps held 5 cm above the test cells. Measured intensity of the UV lamps was 0.64 Wm−2 at a λmax of 354 nm. This is of comparable UV intensity to ASTM G173−03 (2008) which is given as 0.61 Wm−2 at 354 nm [26].


## 3. Results and Discussion

### 3.1. Effect of UV Exposure upon Cell Efficiency

Exposure of unprotected DSCs to UV light induces failure which is illustrated in Figure1 for identical cells forward illuminated and kept in the dark. After around 400 hours of exposure, the efficiency of the UV-exposed cells falls off dramatically whilst, in the dark, it is relatively constant. The change in efficiency, however, follows on from measurable electrochemical changes in the cell that occur well before the failure of the device as determined by its overall cell efficiency.Figure 1
The effect of UV exposure on the %η of DSC test cells compared to that of cells kept in the dark (unexposed).


### 3.2. IV Measurements at 120-Hour Exposure

Figure2 shows the typical I-V curves of a cell at 0-hour and 120-hour UV exposures for the cells illustrated in Figure 1. After just 120-hour exposure, well before detectable changes in efficiency, it can be seen that VOC decreases whilst JSC increases. The change in VOC has been attributed to UV exposure causing a positive shift in the TiO2 conduction band. This would explain the drop in VOC as this is given by the energy difference of the TiO2 quasi-Fermi level and that of the redox potential of the electrolyte [27]. The increase in JSC due to UV illumination has been reported previously and has also been attributed to the positive shift in the conduction band [28].Figure 2
I-V curves of a typical cell at 0-hour and 120-hour UV exposures. It can be seen that VOC has decreased, whilst JSC has increased; however, as can be seen in Figure 1, there is no observable significant changes to cell efficiency.


### 3.3. EIS Measurements at 120-Hour Exposure

Figure3 shows illustrative EIS Nyquist and Bode phase angle plots of the same cell type, again at 0-hour and 120-hour exposures. The larger semicircle of the Nyquist plot (Figure 3(a)) represents the impedance of the TiO2/electrolyte back reaction (RBR). It is clear from the Nyquist plot that the cell experiences a large decrease in RBR whilst the decrease in the phase angle at lower frequencies shown in the Bode phase plot (Figure 3(b)) suggests that electron lifetimes in the TiO2 are reduced. Both of these results can be explained by an increase in the rate of the back reaction (1) [25]. This could arise from an initial exposure of the TiO2 surface, possibly by detachment of dye ligands or by the initial removal of adsorbed organic species from the electrolyte(1)e-[TiO2]+1/2I3-⟶3/2I-.Nyquist plot (a) and Bode phase diagram (b) of the same cell as in Figure2. These results are typical of all the cells exposed during this experiment.
(a)(b)


### 3.4. Longer-Term Testing of Cells Irradiated in Reverse and under Load

Following these initial tests on forward illuminated cells, a more systematic study was performed on a wider range of conditions. Batches of 4 cells were irradiated from the WE (Forward) side, and, from the CE (Reverse) side, in addition, some were irradiated under a load provided by 100 Ω resistor. These are compared to cells that were kept in the dark at 40°C as this was the measured temperature under the UV lamps. Figure4 shows the mean efficiencies and the VOC of the cells subjected to UV irradiation over the time period shown. In Figure 4, it is clear that there is a pattern in the relative rates of degradation of the cells tested. First to fail are the cells irradiated under load followed by cells irradiated from the WE side and then cells irradiated from the CE side. Cells kept in the dark at 40°C show comparatively little sign of degradation, despite a gradual decline in efficiency. This pattern is repeated when looking at the drop in VOC values but, in this case, the drop in VOC manifests itself much more quickly than the decline in efficiency. This data illustrates some important points. Firstly, the reverse illumination where photons travel through the electrolyte reduces photodegradation considerably as the electrolyte is acting as a filter. It does not, however, reduce the rate to zero. Secondly, the cells under load fail more quickly which suggests that the photogenerated electrons from the dye activation have a role to play in reducing the rate of failure when the cells are at open circuit.Change in (a) %η and in (b) VOC over the UV-exposure period. There is a clear order of cell degradation whereby cells under load and illuminated from the WE side fail before those under opencircuit (also illuminated from the WE side) which fail faster than those under opencircuit and illuminated from the CE side. Data is also shown for cells under opencircuit and kept in the dark for the exposure period.
(a)(b)Figure5 shows the change in JSC and the change in RBR  over the exposure period. The value of RBR  falls off quite quickly for all the cells suggesting that there is an increasing area of TiO2 in contact with the electrolyte after the initial UV exposure. Cells that are continually exposed to UV irradiation suffer a collapse in photocurrent and simultaneously a large increase in RBR. The onset of photodegradation also coincides with a loss of colour from the electrolyte which is measured by UV-Vis and is noticeable to the eye at the point of failure. This along with the collapse in JSC and the large increase in RBR  strongly suggests that the cell degradation reaches a point where the I3- has been consumed until there are not enough charge carriers available to give the cell a viable photocurrent.Change inJSC (a) and change in RBR (b) over the UV-exposure period, showing the collapse in photocurrent at the point of cell failure coinciding with a large increase in RBR. The order of cell failure is the same as in Figure 4.
(a)(b)


### 3.5. Triiodide Depletion Measured with UV-Vis

UV-Vis spectroscopy is a useful method for analysing which of the components in the DSC is failing since both the dye and the electrolyte have absorbances which can be analysed simultaneously and in situ without taking the cells apart. The changing UV visible absorbance spectra for the forward illuminated cells are shown in Figure6. It can be seen that the absorbance related to the adsorbed N719 dye (at ca 530 nm) remains relatively constant and the main colour shift is at much lower wavelengths where the electrolyte is absorbing. This adds weight to the suggestion that it is the failure of the electrolyte that is responsible for the failure of the cells, despite the fact that it is the dye that is adsorbed on the TiO2.Figure 6
UV-Vis spectra of a typical cell over the exposure period shown.This is more clearly illustrated in Figure7 where the absorbance of the cell at 531 nm (the λmax of the dye) and 450 nm (a representation of the electrolyte absorbance) is plotted as a function of time. 450 nm was chosen to represent dye colouration as the λmax  of the I−/I3-  redox couple is hidden by the large absorbance of the TiO2. Figure 7 shows that the electrolyte is clearly being degraded whilst dye absorbance remains constant.Figure 7
The changing absorbance of the cell at 531 nm (representing dye colouration) and at 450 nm (representing electrolyte colouration) of cells over the exposure period.Having observed that the electrolyte was being degraded it was desirable to work out the origin of the failure. It could be that the electrolyte is directly attacked or that it is related to TiO2 photoreactions. Figure 8 illustrates the changes in electrolyte absorbance at 450 nm as a function of UV exposure time for two model cells. The first model cell was assembled from two counter electrodes (to examine whether UV alone caused the failure). The second cell type was essentially a full DSC assembly but without any dying step.Figure 8
Change in absorbance of model cells. The undyed cell is essentially a complete DSC. The CE-CE cell consists of two counter electrodes and the electrolyte. This clearly shows that TiO2 is required for electrolyte degradation under UV illumination.It can be seen from the data in Figure8 below that the UV exposure alone does not cause failure but that having a TiO2 electrode causes very rapid failure. There is almost no colour change in the CE-CE cell, and it could be argued that the Pt is absorbing some of the UV light. Whilst this is true, it has been shown in Figure 5 that cells exposed via the CE side still degrade meaning that there is enough UV light reaching the TiO2 to initiate consumption of the I3-. If TiO2 was not involved in I3- consumption, then it would be expected that there might be a colour change in the CE-CE cell despite the UV absorbing properties of the Pt layer.Comparing the data in Figure8 with that from Figure 7 where the dye is included on the TiO2, the presence of the dye dramatically slows the rate of cell failure. We believe this is for two reasons. Firstly, the dye will have taken up sites on the TiO2, and, secondly, it seems that at open circuit the dye is able to inject electrons into the TiO2 (as evidenced by the accelerated failure under load). Hence, it appears that it is the TiO2 and photooxidation by photogenerated holes that are the primary reason for attack on the electrolyte. Since it appears that photocatalytic oxidation could be responsible for the discoloration, the question remains what is the oxidised iodine containing species. At this stage, we have not been able to establish via chemical testing. One possibility for oxidation would be the reverse of (1), but this would of course give rise to a darker electrolyte. Since discolouration is observed, it therefore seems likely that the oxidation yields iodate as suggested in previous work [22]. Further work is in progress to assess; it is potentially the case that by drying and removing oxygen this pathway could be reduced although the TiO2 surface will still have a large quantity of surface bound hydroxyl groups that could lead to this.


### 3.6. UV Filtering

To investigate this further, a series of cells was irradiated with UV in the presence and absence of filters with certain wavelength cutoffs. The data shown earlier shows thatVOC changes are an early indicator of the onset of cell degradation; for this reason, the change in VOC was chosen as an indicator of the effectiveness of UV filters. VOC data for these cells is shown in Figure 9. The initial increase in the VOC of all the filtered cells is typical of cells kept in the dark. It can be seen that the introduction of a 385 nm filter causes an initial increase in VOC, but, after some time, the VOC begins to decline indicating, albeit delayed, the onset of photodegradation. Using higher wavelength cut-off filters of 400 and 420 nm appears to stop this photooxidation completely (within our exposure times at least). This data again points to the potential for TiO2 photocatalysis to contribute to degradation since the TiO2 bandgap for direct excitation is in the range 360–380 nm. The removal of this range of photons clearly prevents cell failure occurring rapidly.Figure 9
VOC data for cells filtered at 385 nm, 400 nm, and 420 nm over the exposure period compared to cells exposed without a UV filter.


### 3.7. Triiodide Regeneration by Application of a Reverse Bias

During the course of these investigations, it was found that UV-degraded and thereforeI3- depleted cells can be regenerated by application of a reverse bias of around +1.3 V. Figure 10 shows the IV curves of the same cell before UV exposure, after UV exposure, and after electrolyte regeneration treatment. It can be seen that the cell, having undergone regeneration treatment, after a period of UV exposure, shows no significant recovery in VOC but a partial recovery in JSC, with increase being attributed to the regeneration of I3- charge carriers in the electrolyte. The production of I3- via application of reverse bias has been noted before by Hauch and Georg [21], but it is not believed to have been reported in connection with the regeneration of UV-degraded DSCs. It was also found during these investigations that the less severely UV degraded the cell, the more effective the regeneration treatment is at recovering the cell to its original properties. It may be possible that by refining this treatment (in terms of the polarisation time, magnitude, and its frequency of application) the regeneration of the devices could be more effectively controlled. This is an attractive solution to restoring device performance since it could be periodically applied (e.g., at night) to maintain cell longevity.Figure 10
I-Vcurves of a typical photodegraded DSC cell before UV exposure, after UV exposure, and after electrolyte regeneration treatment.


## 3.1. Effect of UV Exposure upon Cell Efficiency

Exposure of unprotected DSCs to UV light induces failure which is illustrated in Figure1 for identical cells forward illuminated and kept in the dark. After around 400 hours of exposure, the efficiency of the UV-exposed cells falls off dramatically whilst, in the dark, it is relatively constant. The change in efficiency, however, follows on from measurable electrochemical changes in the cell that occur well before the failure of the device as determined by its overall cell efficiency.Figure 1
The effect of UV exposure on the %η of DSC test cells compared to that of cells kept in the dark (unexposed).


## 3.2. IV Measurements at 120-Hour Exposure

Figure2 shows the typical I-V curves of a cell at 0-hour and 120-hour UV exposures for the cells illustrated in Figure 1. After just 120-hour exposure, well before detectable changes in efficiency, it can be seen that VOC decreases whilst JSC increases. The change in VOC has been attributed to UV exposure causing a positive shift in the TiO2 conduction band. This would explain the drop in VOC as this is given by the energy difference of the TiO2 quasi-Fermi level and that of the redox potential of the electrolyte [27]. The increase in JSC due to UV illumination has been reported previously and has also been attributed to the positive shift in the conduction band [28].Figure 2
I-V curves of a typical cell at 0-hour and 120-hour UV exposures. It can be seen that VOC has decreased, whilst JSC has increased; however, as can be seen in Figure 1, there is no observable significant changes to cell efficiency.


## 3.3. EIS Measurements at 120-Hour Exposure

Figure3 shows illustrative EIS Nyquist and Bode phase angle plots of the same cell type, again at 0-hour and 120-hour exposures. The larger semicircle of the Nyquist plot (Figure 3(a)) represents the impedance of the TiO2/electrolyte back reaction (RBR). It is clear from the Nyquist plot that the cell experiences a large decrease in RBR whilst the decrease in the phase angle at lower frequencies shown in the Bode phase plot (Figure 3(b)) suggests that electron lifetimes in the TiO2 are reduced. Both of these results can be explained by an increase in the rate of the back reaction (1) [25]. This could arise from an initial exposure of the TiO2 surface, possibly by detachment of dye ligands or by the initial removal of adsorbed organic species from the electrolyte(1)e-[TiO2]+1/2I3-⟶3/2I-.Nyquist plot (a) and Bode phase diagram (b) of the same cell as in Figure2. These results are typical of all the cells exposed during this experiment.
(a)(b)


## 3.4. Longer-Term Testing of Cells Irradiated in Reverse and under Load

Following these initial tests on forward illuminated cells, a more systematic study was performed on a wider range of conditions. Batches of 4 cells were irradiated from the WE (Forward) side, and, from the CE (Reverse) side, in addition, some were irradiated under a load provided by 100 Ω resistor. These are compared to cells that were kept in the dark at 40°C as this was the measured temperature under the UV lamps. Figure4 shows the mean efficiencies and the VOC of the cells subjected to UV irradiation over the time period shown. In Figure 4, it is clear that there is a pattern in the relative rates of degradation of the cells tested. First to fail are the cells irradiated under load followed by cells irradiated from the WE side and then cells irradiated from the CE side. Cells kept in the dark at 40°C show comparatively little sign of degradation, despite a gradual decline in efficiency. This pattern is repeated when looking at the drop in VOC values but, in this case, the drop in VOC manifests itself much more quickly than the decline in efficiency. This data illustrates some important points. Firstly, the reverse illumination where photons travel through the electrolyte reduces photodegradation considerably as the electrolyte is acting as a filter. It does not, however, reduce the rate to zero. Secondly, the cells under load fail more quickly which suggests that the photogenerated electrons from the dye activation have a role to play in reducing the rate of failure when the cells are at open circuit.Change in (a) %η and in (b) VOC over the UV-exposure period. There is a clear order of cell degradation whereby cells under load and illuminated from the WE side fail before those under opencircuit (also illuminated from the WE side) which fail faster than those under opencircuit and illuminated from the CE side. Data is also shown for cells under opencircuit and kept in the dark for the exposure period.
(a)(b)Figure5 shows the change in JSC and the change in RBR  over the exposure period. The value of RBR  falls off quite quickly for all the cells suggesting that there is an increasing area of TiO2 in contact with the electrolyte after the initial UV exposure. Cells that are continually exposed to UV irradiation suffer a collapse in photocurrent and simultaneously a large increase in RBR. The onset of photodegradation also coincides with a loss of colour from the electrolyte which is measured by UV-Vis and is noticeable to the eye at the point of failure. This along with the collapse in JSC and the large increase in RBR  strongly suggests that the cell degradation reaches a point where the I3- has been consumed until there are not enough charge carriers available to give the cell a viable photocurrent.Change inJSC (a) and change in RBR (b) over the UV-exposure period, showing the collapse in photocurrent at the point of cell failure coinciding with a large increase in RBR. The order of cell failure is the same as in Figure 4.
(a)(b)


## 3.5. Triiodide Depletion Measured with UV-Vis

UV-Vis spectroscopy is a useful method for analysing which of the components in the DSC is failing since both the dye and the electrolyte have absorbances which can be analysed simultaneously and in situ without taking the cells apart. The changing UV visible absorbance spectra for the forward illuminated cells are shown in Figure6. It can be seen that the absorbance related to the adsorbed N719 dye (at ca 530 nm) remains relatively constant and the main colour shift is at much lower wavelengths where the electrolyte is absorbing. This adds weight to the suggestion that it is the failure of the electrolyte that is responsible for the failure of the cells, despite the fact that it is the dye that is adsorbed on the TiO2.Figure 6
UV-Vis spectra of a typical cell over the exposure period shown.This is more clearly illustrated in Figure7 where the absorbance of the cell at 531 nm (the λmax of the dye) and 450 nm (a representation of the electrolyte absorbance) is plotted as a function of time. 450 nm was chosen to represent dye colouration as the λmax  of the I−/I3-  redox couple is hidden by the large absorbance of the TiO2. Figure 7 shows that the electrolyte is clearly being degraded whilst dye absorbance remains constant.Figure 7
The changing absorbance of the cell at 531 nm (representing dye colouration) and at 450 nm (representing electrolyte colouration) of cells over the exposure period.Having observed that the electrolyte was being degraded it was desirable to work out the origin of the failure. It could be that the electrolyte is directly attacked or that it is related to TiO2 photoreactions. Figure 8 illustrates the changes in electrolyte absorbance at 450 nm as a function of UV exposure time for two model cells. The first model cell was assembled from two counter electrodes (to examine whether UV alone caused the failure). The second cell type was essentially a full DSC assembly but without any dying step.Figure 8
Change in absorbance of model cells. The undyed cell is essentially a complete DSC. The CE-CE cell consists of two counter electrodes and the electrolyte. This clearly shows that TiO2 is required for electrolyte degradation under UV illumination.It can be seen from the data in Figure8 below that the UV exposure alone does not cause failure but that having a TiO2 electrode causes very rapid failure. There is almost no colour change in the CE-CE cell, and it could be argued that the Pt is absorbing some of the UV light. Whilst this is true, it has been shown in Figure 5 that cells exposed via the CE side still degrade meaning that there is enough UV light reaching the TiO2 to initiate consumption of the I3-. If TiO2 was not involved in I3- consumption, then it would be expected that there might be a colour change in the CE-CE cell despite the UV absorbing properties of the Pt layer.Comparing the data in Figure8 with that from Figure 7 where the dye is included on the TiO2, the presence of the dye dramatically slows the rate of cell failure. We believe this is for two reasons. Firstly, the dye will have taken up sites on the TiO2, and, secondly, it seems that at open circuit the dye is able to inject electrons into the TiO2 (as evidenced by the accelerated failure under load). Hence, it appears that it is the TiO2 and photooxidation by photogenerated holes that are the primary reason for attack on the electrolyte. Since it appears that photocatalytic oxidation could be responsible for the discoloration, the question remains what is the oxidised iodine containing species. At this stage, we have not been able to establish via chemical testing. One possibility for oxidation would be the reverse of (1), but this would of course give rise to a darker electrolyte. Since discolouration is observed, it therefore seems likely that the oxidation yields iodate as suggested in previous work [22]. Further work is in progress to assess; it is potentially the case that by drying and removing oxygen this pathway could be reduced although the TiO2 surface will still have a large quantity of surface bound hydroxyl groups that could lead to this.


## 3.6. UV Filtering

To investigate this further, a series of cells was irradiated with UV in the presence and absence of filters with certain wavelength cutoffs. The data shown earlier shows thatVOC changes are an early indicator of the onset of cell degradation; for this reason, the change in VOC was chosen as an indicator of the effectiveness of UV filters. VOC data for these cells is shown in Figure 9. The initial increase in the VOC of all the filtered cells is typical of cells kept in the dark. It can be seen that the introduction of a 385 nm filter causes an initial increase in VOC, but, after some time, the VOC begins to decline indicating, albeit delayed, the onset of photodegradation. Using higher wavelength cut-off filters of 400 and 420 nm appears to stop this photooxidation completely (within our exposure times at least). This data again points to the potential for TiO2 photocatalysis to contribute to degradation since the TiO2 bandgap for direct excitation is in the range 360–380 nm. The removal of this range of photons clearly prevents cell failure occurring rapidly.Figure 9
VOC data for cells filtered at 385 nm, 400 nm, and 420 nm over the exposure period compared to cells exposed without a UV filter.


## 3.7. Triiodide Regeneration by Application of a Reverse Bias

During the course of these investigations, it was found that UV-degraded and thereforeI3- depleted cells can be regenerated by application of a reverse bias of around +1.3 V. Figure 10 shows the IV curves of the same cell before UV exposure, after UV exposure, and after electrolyte regeneration treatment. It can be seen that the cell, having undergone regeneration treatment, after a period of UV exposure, shows no significant recovery in VOC but a partial recovery in JSC, with increase being attributed to the regeneration of I3- charge carriers in the electrolyte. The production of I3- via application of reverse bias has been noted before by Hauch and Georg [21], but it is not believed to have been reported in connection with the regeneration of UV-degraded DSCs. It was also found during these investigations that the less severely UV degraded the cell, the more effective the regeneration treatment is at recovering the cell to its original properties. It may be possible that by refining this treatment (in terms of the polarisation time, magnitude, and its frequency of application) the regeneration of the devices could be more effectively controlled. This is an attractive solution to restoring device performance since it could be periodically applied (e.g., at night) to maintain cell longevity.Figure 10
I-Vcurves of a typical photodegraded DSC cell before UV exposure, after UV exposure, and after electrolyte regeneration treatment.


## 4. Conclusion

Photocatalytic reactions instigated by UV irradiation are detrimental to dye-sensitized solar cell performance, and this study shows there are subtle changes that occur within a few days of exposure that manifest themselves before changes in cell efficiency are detected. The open circuit voltage, short circuit current, and back reaction resistance (VOC, JSC, and RBR) all change relatively rapidly, and these are therefore potentially important indicators of cell degradation which can be to quickly evaluate UV protection measures, such as spectral cut-off filters. In addition, spectrophotometry is an important and simple tool for evaluating which component of the cell (dye or electrolyte) is under attack and enable kinetics of the processes to be simultaneously evaluated.The focus for degradation in cell performance in our tests seems to be through TiO2 photocatalysed attack on the electrolyte leading to consumption of the triiodide in the electrolyte. This seems to come from an initial exposure of TiO2 surfaces which is evidenced by a reduction in RBR. The fall in RBR coincides with the onset of discolouration of the electrolyte and is far more rapid in cells under load. This indicates that, at open circuit, electrons injected into the TiO2 by the dye are able to quench photogenerated holes as there is no external transport mechanism. When an external circuit is present, fewer TiO2 electron-hole pair recombinations occur, leading to an increase in hole concentration and an increase in the rate of I3- consumption and therefore cell degradation. In addition, removal of bandgap photons in the range <400 nm stops the degradation of the electrolyte from occurring. One reaction that could occur from the oxidative hole is the conversion of I− to I3- resulting in increased triiodide production and therefore an increase absorbance at 450 nm. Since this is not the case, then it could be possible that the triiodide is oxidised to iodate. Work is continuing in order to determine whether or not this is the case and to establish if iodate is the reaction product and the nature of the oxygen source (water or oxygen in the electrolyte or directly from OH moieties on the TiO2 surface).It seems that in the timescale of our irradiations, at least the dye is not subject to degradation. Since it is the TiO2 photocatalysed oxidation that dominates, DSC stability can be improved as would be expected by including appropriate filters into the device to remove photons in the range of the bandgap of the TiO2. In addition, application of a reverse bias appears to regenerate depleted triiodide and restore cell performance of UV-photodegraded DSCs. Work is also continuing to establish whether a periodically applied reverse bias to DSCs under UV and visible light soaking conditions is an effective means of maintaining cell performance.



---

*Source: 524590-2012-02-01.xml*