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Electronic Supplementary Material (ESI) for ChemComm.
This journal is © The Royal Society of Chemistry 2014
Platinum nanoparticles strongly associated with graphitic carbon nitride
as efficient co-catalysts for photocatalytic hydrogen evolution
under visible light
Yasuhiro Shiraishi,*,a Yusuke Kofuji,a Shunsuke Kanazawa,a Hirokatsu Sakamoto,a
Satoshi Ichikawa,b Shunsuke Tanaka,c and Takayuki Hiraia
a
Research Center for Solar Energy Chemistry, and Division of Chemical Engineering, Graduate
School of Engineering Science, Osaka University, Toyonaka 560-8531, Japan
b
Institute for NanoScience Design, Osaka University, Toyonaka 560-8531, Japan
c
Department of Chemical, Energy and Environmental Engineering, Kansai University, Suita
564-8680, Japan
E-mail: shiraish@cheng.es.osaka-u.ac.jp
Electronic Supplementary Information (ESI†)
Catalyst preparation
g-C3N4: this was synthesized according to literature procedure,[1] as follows: melamine (9.0 g)
was added to a porcelain cup and calcined at 823 K for 4 h, with the heating rate being 2.3 K
min−1. Grinding of the resultant affords yellow powders of g-C3N4.
Pt0.3/g-C3N4 (photoreduction method): this was synthesized according to literature
procedure,[2,3] as follows: g-C3N4 (0.1 g) and H2PtCl6・6H2O (0.8 mg) were added to a 10 %
TEOA solution (30 mL) in a borosilicate glass bottle (φ 35 mm; capacity, 50 mL). The bottle
was sealed with a rubber septum cap and purged with Ar by the gas bubbling. The bottle was
photoirradiated at λ >420 nm using a 2 kW Xe lamp (USHIO Inc.)[4] with magnetic stirring at
298 K for 6 h. The resultant was recovered by centrifugation, washed with water, and dried in
vacuo at room temperature for 12 h, affording dark yellow powders of Pt0.3/g-C3N4.
Annealing of Pt0.3/g-C3N4 was carried out under N2 or H2 flow. The heating rate was 10 K
min–1, and the temperature was kept for 2 h at 673 K.
Ptx/g-C3N4 (H2 reduction method): the catalysts [x (wt%) = 0.05, 0.1 0.2, 0.3, 0.4, 0.5, 0.8,
and 1.0] were prepared as follows:[5] g-C3N4 (1.0 g) and different amount of H2PtCl6・6H2O
(1.3, 2.7, 5.3, 8.0, 10.7, 13.3, 21.4, or 26.8 mg) were added to water (30 mL) in a borosilicate
glass bottle and evaporated with vigorous stirring at 373 K for 12 h. The obtained powders
were reduced under H2 flow (0.1 mL min–1). The heating rate was 10 K min–1, and the
temperature was kept for 2 h at designated temperature (473, 573, 673, 773 and 873 K).
Photoreaction
Each respective catalyst (20 mg) was added to a 10% TEOA solution (5 mL) within a Pyrex
glass tube (capacity, 20 mL). The tube was sealed with a rubber septum cap. The catalyst was
dispersed well by ultrasonication for 5 min, and Ar gas was bubbled through the solution for
1
15 min. The bottle was immersed in a temperature-controlled water bath and photoirradiated
at λ >420 nm using a 2 kW Xe lamp (USHIO Inc.) with magnetic stirring at 298 K.[6] After
the reaction, the amount of H2 formed was determined by GC-TCD (Shimadzu; GC-8A).
Determination of apparent quantum efficiency
Photoreaction was performed with a 10% MeOH solution (30 mL) containing each respective
catalyst (100 mg) within a borosilicate glass bottle (capacity, 50 mL), sealed with a rubber
septum cap. The catalyst was dispersed by ultrasonication for 5 min, and Ar was bubbled
through the solution for 15 min. The solution was photoirradiated with 2 kW Xe lamp
(USHIO Inc.), where the incident light was monochromated by a band-pass glass filter (λ =
440 nm, Asahi Techno Glass Co.). The full-width at half-maximum (FWHM) of the light was
11 nm. The temperature of solution during irradiation was kept at 298 K with a
temperature-controlled water bath. The photon number entered into the reaction vessel was
determined with a spectroradiometer USR-40 (USHIO Inc.). The apparent quantum efficiency
(ΦAQE) for H2 evolution was calculated using the equation:[7] ΦAQE (%) = {[H2 evolved
(µmol)] × 2} / [photon number entered into the reaction vessel] × 100.
Analysis
XPS anaysis was performed using a JEOL JPS-9000MX spectrometer using Mg Kα radiation
as the energy source. TEM observations were performed using an FEI Tecnai G2 20ST
analytical electron microscope operated at 200 kV.[8] XRD patterns were measured on a
Philips X′Pert-MPD spectrometer. Total Pt amounts on the catalysts were determined by an
X-ray ﬂuorescence spectrometer (Seiko Instruments, Inc.; SEA2110). Diffuse-reflectance
UV-vis spectra were measured on an UV-vis spectrophotometer (JASCO Corp.; V-550)
equipped with Integrated Sphere Apparatus ISV-469, using BaSO4 as a reference.
References
[1] S. Yan, Z. Li and Z. Zou, Langmuir, 2009, 25, 10397–10401.
[2] K. Bernhard and A. J. Bard, J. Am. Chem. Soc., 1978, 100, 4317–4318.
[3] Y. Shiraishi, Y. Sugano, S. Tanaka and T. Hirai, Angew. Chem. Int. Ed., 2010, 49,
1656–1660.
[4] Y. Sugano, Y. Shiraishi, D. Tsukamoto, S. Ichikawa, S. Tanaka and T. Hirai, Angew. Chem.
Int. Ed., 2013, 52, 5295–5299.
[5] Y. Shiraishi, H. Sakamoto, Y. Sugano, S. Ichikawa and T. Hirai, ACS Nano, 2013, 7,
9287–9297.
[6] D. Tsukamoto, Y. Shiraishi, Y. Sugano, S. Ichikawa, S. Tanaka and T. Hirai, J. Am. Chem.
Soc., 2012, 134, 6309–6315.
[7] X. Wang, K. Maeda, A. Thomas, K. Takanabe, G. Xin, J. Carlsson, K. Domen and M.
Antonietti, Nat. Mater., 2009, 8, 76–80.
[8] Y. Shiraishi, K. Tanaka, E. Shirakawa, Y. Sugano, S. Ichikawa, S. Tanaka and T. Hirai,
Angew. Chem. Int. Ed., 2013, 52, 8304–8308.
2
3
g-C3N4
F(R∞)
2
Pt0.3/g-C3N4
Photoreduction@298 K
1
Pt0.3/g-C3N4
H2 reduction@673 K
0
400
600
800
Wavelength / nm
2.55 eV
(H2 reduction@673 K)
(hνF (R∞）)2
3
2
1
2.58 eV (photoreduction@298 K)
2.62 eV (g-C3N4)
0
2
3
4
hν / eV
Fig. S1 (top) Diffuse reflectance UV-vis spectra of respective g-C3N4 and Pt0.3/g-C3N4
catalysts. (bottom) Results of band gap determination.
3
(002)
27.4
(100)
12.7
g-C3N4
Pt0.3/g-C3N4
Photoreduction
@298 K
H2 reduction
@473 K
@573 K
@673 K
@773 K
@873 K
10
20
30
40
2θ / degree
Fig. S2 XRD patterns for respective g-C3N4 and Pt0.3/g-C3N4 catalysts.
4
284.6
287.5
285.5
g-C3N4
289.0
Pt0.3/g-C3N4
Photoreduction
@298 K
289.1
285.7
285.8
H2 reduction
@473 K
285.6
289.3
@673 K
289.1
@873 K
294
292
288
286
290
Binding energy / eV
284
282
398.1
399.3
g-C3N4
399.4
Pt0.3/g-C3N4
Photoreduction
@298 K
399.5
H2 reduction
@473 K
399.4
@673 K
@873 K
404
402
398
400
Binding energy / eV
396
394
Fig. S3 XPS chart for (top) C1s and (bottom) N1s levels of g-C3N4 and Pt0.3/g-C3N4.
5
Pt0.3/g-C3N4 (photoreduction@
(photoreduction@298 K + N2 annealing@673 K)
dPt = 31.4 ± 9.7 nm
Count
10
5
0
0
10 20 30 40 50 60
Size / nm
Pt0.3/g-C3N4 (photoreduction@298 K + H2 annealing@673 K)
dPt = 26.4 ± 6.2
.2 nm
Count
20
10
0
0 10 20 30 40 50 60
Size / nm
Pt0.3/g-C3N4 (H2 reduction@473
473 K)
50
dPt = 1.5 ± 0.5 nm
Count
40
30
20
10
0
0
2
4
6
8
10
Size / nm
6
Pt0.3/g-C3N4 (H2 reduction@873
873 K)
15
dPt = 6.6 ± 2.3 nm
Count
10
5
0
0
2
4
6
8
10
Size / nm
673 K)
Pt0.1/g-C3N4 (H2 reduction@673
40
dPt = 3.4 ± 0.9 nm
Count
30
20
10
0
0
2
4
6
8
10
Size / nm
Pt1.0/g-C3N4 (H2 reduction@673
673 K)
dPt = 3.6 ± 1.3 nm
40
Count
30
20
10
0
0
2
4
6
8
10
Size / nm
Fig. S4 Typical TEM images of Ptx/g-C3N4 catalysts and size distributions of Pt particles.
7