DEVELOPMENT OF HIGH TEMPERATURE PROTON EXCHANGE MEMBRANE WATER ELECTROLYSER FOR GENERATION OF PURE
HYDROGEN AND OXYGEN
VARAGUNAPANDIYAN N
DEPARTMENT OF CHEMICAL ENGINEERING INDIAN INSTITUTE OF TECHNOLOGY DELHI
NEW DELHI - 110016
MARCH 2015
© Indian Institute of Technology Delhi (IITD), New Delhi, 2015
DEVELOPMENT OF HIGH TEMPERATURE PROTON EXCHANGE MEMBRANE WATER ELECTROLYSER FOR GENERATION OF PURE
HYDROGEN AND OXYGEN
by
VARAGUNAPANDIYAN N Department of Chemical Engineering
Submitted
in fulfillment of the requirements of the degree of Doctor of Philosophy
to the
INDIAN INSTITUTE OF TECHNOLOGY DELHI
MARCH 2015
Dedicated to my family
i
CERTIFICATE
This is to certify that thesis entitled “Development of high temperature proton exchange
membrane water electrolyser for generation of pure hydrogen and oxygen” submitted by Mr. Varagunapandiyan N to the Department of Chemical Engineering, Indian Institute of Technology Delhi, New Delhi, for fulfillment of the requirements for the award of Doctor of Philosophy in Chemical Engineering is a record of bonafide work carried out by him. He has worked under my guidance and supervision and has fulfilled the requirements, which to my knowledge, has reached the requisite standard for the submission of the thesis.
The research report and results presented in this thesis have not been submitted, in part or full, to any other university or institute for the award of any degree or diploma.
Suddhasatwa Basu Professor and Head Department of Chemical Engineering Indian Institute of Technology Delhi New Delhi 110016, India
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ACKNOWLEDGEMENTS
First of all, I would like to express my sincere gratitude and heartiest thanks to my guide and mentor Prof. Suddhasatwa Basu for his sincere guidance, keen interest and continuous encouragement. He has always shown immense patience and dedicated interest for rectifying my mistakes and improving my skills through discussions by devoting his invaluable time. I am fortunate enough to work under his supervision. He has influenced me both in academic and personal front.
I wish to thank my committee members, Dr. Anupam Shukla, Prof. A. N. Bhaskarwar and Prof. A. Ramanan, for their valuable suggestion and requisite guidance on technical issues during the research work. Encouragement and constant support from Dr. Anupam Shukla throughout my research work is greatly acknowledged. I am also grateful to all the faculty members for their help and cooperation whenever needed.
I wish to thank Council of Scientific and Industrial Research organization (CSIR) for financial support during the execution of research work. I thank all the non teaching staff of Chemical Engineering Department for their help and support, Centre for Polymer Science and Engineering for providing me SEM and EDX facilities and Department of Physics and Chemistry for TEM and XRD facilities.
It was great pleasure to work in fuel cell laboratory. I am thankful to Dr Debika Basu, Dr.
Anand Singh, Dr. Amit Kumar Gupta, Dr. Rajalekhmi Chockalingam, Mr. Pankaj Kumar Tiwari, Dr. Gurpreet Kaur, Mr. Shaneeth M., Mrs Jyoti Goel, Mr. Amandeep Jindal, Mr.
Harikrishnan N., Dr. Merajul Islam, Mrs. Neetu Kumari, Ms. Ieeba Khan, Mr. Nimai Bhandary, Ms. Garima, Ms. Anu, Mr. Amol, Ms. Criti Mahajan, Mr. Assem Sharma, Mr. Sarthak Nigam,
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Mr. Deepak and all other lab members. I would like to thanks Mr. Sunder Singh for his kind support during entire period.
I wish to express my heartfelt thanks to Mr. Vishesh Kumar for allowing me to use Design Lab and furnaces during my research work. I wish to thank all the laboratory and office staff of Chemical Engineering Department especially Mr. Ashish and Mr. Chandan Singh for their encouragement, help and assistance.
I must express my heartiest thanks to my parents Mr. R. Natarajan and Mrs. Ganambal for their well wishes. I sincerely thank my elder brother Mr. N. Annadurai and his wife Mrs. B.
Meenakshi. I should not forget my in-laws Mr. V. Sadhasivam and Mrs. R. Siraivani and brother-in-law Mr. S. Stalin who supported me in these years and help me to take challenges through devotion and hard work.
The research would not have been possible without the support of my wife S. Ezhilarasi. I will always be thankful to her for tremendous patience and encouragement to generate positive thoughts and strength inside me to accomplish the ultimate goal.
Varagunapandiyan N
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ABSTRACT
Proton exchange membrane water electrolyser (PEMWE) splits water into oxygen and pure hydrogen by oxygen evolution reaction (OER) at anode and hydrogen evolution reaction (HER) at cathode. Water splitting may be more efficient in high temperature PEMWE because of the higher kinetics of electrocatalyst and conductivity of membrane. Although the work on high temperature PEM fuel cell is reported in literature, the same is not true for high temperature PEMWE. To reduce energy consumption in PEMWE, RuO2 and RuO2-Ta2O5
electrocatalysts are tried as anode electrocatalyst in high temperature PEMWE. The anode electrocatalysts are prepared by sol-gel procedure with different compositions and at different calcination temperatures for oxygen evolution reaction. The catalysts are characterized by physical and electrochemical characterization techniques. Physical characterizations are carried out to study the thermal stability, oxygen-metal bond formation, crystalline phase and size, particle size, surface morphology, elemental analysis and elemental mapping by thermogravimetry analysis (TGA), fourier transform infrared spectroscopy (FTIR), X-ray diffraction (XRD) pattern, transmission electron microscope (TEM), scanning electron microscope (SEM) and energy dispersive X-ray (EDX), respectively. Electrochemical characterization is carried out to study the OER on prepared electrocatalyst by cyclic voltammetry (CV), chronoamperometry (CA) in 1.0 M H3PO4 and 0.5 M H2SO4 electrolyte.
Additionally, the effect of electrolyte temperature (25-90 °C) on oxygen evolution reaction is studied and apparent activation energy is estimated from chronoamperogram. The maximum current density (17.27 mA cm-2) at 1.2 V is achieved for 90%RuO2-10%Ta2O5 anode electrocatalyst calcined at 500 °C in CV experiment using 1.0 M H3PO4 electrolyte at 90 °C.
LSV is carried out to understand the OER electron pathway mechanism using rotating ring disk electrode (RRDE) with different rotations (800 to 2000 rpm). LSV of RuO2 and 90%RuO2-10%Ta2O5 electrocatalyst calcined at 500 oC follows 3.8 and 2.68 electron
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pathway mechanism for OER. Since proton exchange membrane, Nafion 117, dry up at high temperature (>100 oC) leading to severe loss in ionic conductivity, phosphoric acid doped polybenzimidazole (PBI) membrane is used as electrolyte in the present work. The measured conductivity of 14 M H3PO4 acid doped PBI membrane is 0.012 S/cm at 150 oC. RuO2 and RuO2-Ta2O5 electrocatalysts are tested in PEMWE for splitting of water using 14 M H3PO4
acid doped PBI membrane as proton exchange electrolyte and Pt black as cathode catalyst.
Gold plated titanium mesh is used as current collector and gold plated titanium monopolar plate (TMP) is used as an end plate and water vapour delivery system at the anode. PEMWE showed best performance for 90%RuO2-10%Ta2O5 electrocatalyst calcined at 500 °C and operating at 150 °C with current density of 1.1 A cm-2 at 1.8 V. However, RuO2 used as anode electrocatalyst in PEMWE (at 80 °C) gave lower current density of 0.875 A cm-2 at 1.8 V and its performance dipped after 2.8 h. The stability of PEMWE is improved by the addition of tantalum oxide to ruthenium oxide as 90%RuO2-10%Ta2O5 anode electrocatalyst showed the stable current density of 1.1 A cm-2 at 1.8 V up to 5.3 h. The product analysis are carried out in gas chromatography using molecular sieve 5A and Propak Q column, which confirms the presence of hydrogen and oxygen with purity of 99.68% and 95.5% respectively The energy efficiency of PEMWE is estimated as 35.31%. Moreover 90%RuO2-10%Ta2O5
anode catalyst found to be more stable compared to RuO2 in 5 h operation of PEMWE at 150
°C and, further, PEMWE anolyte, membrane electrode assembly after PEMWE operation are investigated by FTIR and X-ray photoelectron spectroscopies (XPS) to evaluate degradation.
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CONTENTS
Page No.
Certificate i
Acknowledgements ii-iii
Abstract iv-v
Contents vi
List of Figures x
List of Tables xvii
Nomenclature xix
Chapter 1 Introduction 1-14
1.1 Background 1
1.2
Principle of proton exchange membrane water electrolyser
(PEMWE) 4
1.3 Thermodynamics of water splitting 5
1.4 PEMWE energy efficiency calculation 8
1.5 Thesis organization 10
References 13
Chapter 2 Literature Review 15-40
2.1 Oxygen evolution reaction (OER) catalysts 15
2.1.1 Dimensionally stable electrodes 16
2.1.2 Anode electrocatalysts for OER in PEMWE 17 2.2 Physical and electrochemical characterization techniques 25
2.3 Motivation and objectives of thesis work 26
References 29
vii
Chapter 3 Experimental 41-58
3.1 Materials 41
3.2 Catalyst preparation 43
3.3 Physical characterization techniques 45
3.4 Electrochemical analysis 47
3.5 Membrane conductivity measurement 49
3.6 PEMWE testing 51
3.6.1 Gold coating of titanium mono-polar (TMP) plate and titanium
mesh 51
3.6.2 Fabrication of membrane electrode assembly (MEA) 53
3.6.3 PEMWE setup and operation 54
References 58
Chapter 4 Results and Discussion on Performance of RuO2 Anode
Electrocatalyst for High Temperature PEMWE 59-80
4.1 Physical characterization techniques 59
4.1.1 X-ray diffraction (XRD) pattern of RuO2 59
4.1.2 FTIR of RuO2 60
4.1.3 TEM of RuO2 62
4.1.4 EDX and SEM of RuO2 62
4.2 Electrochemical analysis 64
4.2.1 Rotating ring disk electrode (RRDE) 69
4.3 Performance of RuO2 in PEMWE 72
4.3.1 Low temperature PEMWE 72
4.3.2 High temperature PEMWE 73
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4.4 PEMWE stability test 76
References 79
Chapter 5 Results and Discussion on Performance of Ruthenium oxide- Tantalum Oxide Anode Electrocatalyst for High
Temperature PEMWE 81-124
5.1 Physical characterization techniques 82
5.1.1 X-ray diffraction (XRD) pattern of RuO2-Ta2O5 82
5.1.2 FTIR of RuO2-Ta2O5 84
5.1.3 TEM of RuO2-Ta2O5 87
5.1.4 EDX and SEM of RuO2-Ta2O5 88
5.2 Electrochemical Analysis 93
5.2.1 Effect of compositions of RuO2-Ta2O5 93 5.2.2 Effect of calcination and electrolyte temperature on RuO2-Ta2O5 97
5.2.3 Chronoamperometry of RuO2-Ta2O5 101
5.2.4 Rotating ring disk electrode (RRDE) 104
5.3 Performance of RuO2-Ta2O5 in PEMWE 109
5.3.1 Effect of different compositions of RuO2-Ta2O5 in PEMWE 109 5.3.2 Effect of operating temperature in PEMWE 111
5.4 PEMWE stability test 114
5.5 Degradation analysis 115
5.6 Product analysis and energy efficiency calculation 120
References 122
Chapter 6 Conclusions and Summary 125-130
6.1 Scope of future work 128
ix
Appendices 131-138
A Synthesis and characterization of RuO2 and IrO2 by polyol method
131
B Stability test for 90%RuO2-10%Ta2O5 calcined at different temperatures
136 C Synthesis of composite membranes and testing in PEMWE 137
List of Publications 139
About the Author 141
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LIST OF FIGURES
Figure No. Title Page
No.
Fig. 1.1 Schematic diagram showing working principle of PEMWE 5
Fig. 1.2 Polarization curve of PEMWE 7
Fig. 3.1 TGA/DTA curve of RuCl3.xH2O and RuO2 calcined at 400 °C 44 Fig. 3.2 Schematic diagram of three electrode cell assembly connected to
potentiostat-galvanostat 47
Fig. 3.3 Schematic diagram of rotating ring disk electrode 48
Fig. 3.4 Structure of phosphoric acid doped PBI 49
Fig. 3.5 PBI membrane conductivity measurement setup 49 Fig. 3.6 Apparent activation energy of PBI membrane 50 Fig. 3.7 Schematic representation of gold coating (a) TMP flow channel (b)
Titanium mesh 51
Fig. 3.8 Photograph of gold coating setup for TMP flow channel 52 Fig. 3.9 Photograph of gold coated (a) TMP flow channel (b)Titanium mesh 52 Fig. 3.10 Schematic representation of fabrication of membrane electrode
assembly (MEA) for PEMWE 53
Fig. 3.11 Photograph of (a) RuO2 coated on PBI membrane (b) Pt black coated on carbon
54
Fig. 3.12 (a) Schematic diagram of PEMWE 55
Fig. 3.12 (b) Schematic diagram of high temperature PEMWE experimental setup 55 Fig. 3.12 (c) Photograph of high temperature PEMWE experimental setup 56
xi
Fig. 4.1 XRD of RuO2 calcined at three temperatures (a) 400 °C, (b) 500 °C
and (c) 600 °C 60
Fig. 4.2 FTIR of RuO2 calcined at three temperatures (a) 400 °C, (b) 500 °C
and (c) 600 °C 61
Fig. 4.3 TEM of RuO2 calcined at three temperatures (a) 400 °C, (b) 500 °C
and (c) 600 °C 62
Fig. 4.4 EDX of RuO2 calcined at three temperatures (a) 400 °C, (b) 500 °C
and (c) 600 °C 63
Fig. 4.5 SEM of RuO2 calcined at three temperatures (a) 400 °C, (b) 500 °C
and (c) 600 °C 64
Fig. 4.6 Cyclic voltammetry at different temperatures of electrolyte for RuO2
calcined at 400 °C, 500 °C, 600 °C (a) 1.0 H3PO4 (b) H2SO4 66 Fig. 4.7 Chronoampertometry of RuO2 calcined at 500 °C at different
electrolyte (1.0 H3PO4) temperatures 66
Fig. 4.8 Apparent activation energy plot for RuO2 calcined at 400 °C, 500 °C,
and 600 °C (a) 1.0 M H3PO4 (b) 0.5 M H2SO4 68 Fig. 4.9 Linear sweep voltammetry using rotating ring disk electrode for
RuO2 catalyst calcined at 500 °C in 1.0 M H3PO4 electrolyte at 50 °C
with different rotation speeds 69
Fig. 4.10 Linear sweep voltammetry using rotating ring disk electrode for RuO2 catalyst calcined at 500 °C in 1.0 H3PO4 electrolyte at 90 °C
with different rotation speeds 70
Fig. 4.11 Koutecky-Levich plot for RuO2 catalyst calcined at 500 °C 71 Fig. 4.12 i-V curve of PEMWE with RuO2 and IrO2 as anode catalyst for
PEMWE with different operating temperatures
73
xii
Fig. 4.13 Performance of PEMWE with Pt black as anode and cathode catalyst 74 Fig. 4.14 Performance of PEMWE with RuO2 as anode catalyst calcined at 400
°C and Pt black as cathode catalyst 74
Fig. 4.15 Performance of PEMWE with RuO2 as anode catalyst calcined at 500
°C and Pt black as cathode catalyst 75
Fig. 4.16 Performance of PEMWE with RuO2 as anode catalyst calcined at 600
°C and Pt black as cathode catalyst 75
Fig. 4.17 Stability test of RuO2 in PEMWE operated at 150 °C 77 Fig. 5.1 XRD of RuO2-Ta2O5 with different compositions calcined at 400 °C 83 Fig. 5.2 XRD of RuO2-Ta2O5 with different compositions calcined at 500 °C 83 Fig. 5.3 XRD of RuO2-Ta2O5 with different compositions calcined at 600 °C 84 Fig. 5.4 FTIR of RuO2-Ta2O5 with different compositions calcined at 400 °C 85 Fig. 5.5 FTIR of RuO2-Ta2O5 with different compositions calcined at 500 °C 86 Fig. 5.6 FTIR of RuO2-Ta2O5 with different compositions calcined at 600 °C 86 Fig. 5.7 TEM of RuO2-Ta2O5 with different compositions calcined at 400 °C
(a) 90% RuO2-10%Ta2O5 (b) 80% RuO2-20%Ta2O5 (c) 70% RuO2-
30%Ta2O5 87
Fig. 5.8 TEM of RuO2-Ta2O5 with different compositions calcined at 500 °C (a) 90% RuO2-10%Ta2O5 (b) 80% RuO2-20%Ta2O5 (c) 70% RuO2-
30%Ta2O5 87
Fig. 5.9 TEM of RuO2-Ta2O5 with different compositions calcined at 600 °C
(a) 90% RuO2-10%Ta2O5 (b) 80% RuO2-20%Ta2O5 88 Fig. 5.10 EDX of RuO2-Ta2O5 with different compositions calcined 400 °C (a)
90%RuO2-10%Ta2O5 (b) 80%RuO2-20%Ta2O5 (c) 70%RuO2-
30%Ta2O5 (d) 60%RuO2-40%Ta2O5 89
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Fig. 5.11(a) Elemental mapping of 90%RuO2-10%Ta2O5 calcined at 400 °C 89 Fig. 5.11(b) Elemental mapping of 80%RuO2-20%Ta2O5 calcined at 400 °C 90 Fig. 5.11(c) Elemental mapping of 70%RuO2-30%Ta2O5 calcined at 400 °C 90 Fig. 5.11(d) Elemental mapping of 60%RuO2-40%Ta2O5 calcined at 400 °C 91 Fig. 5.12 SEM of RuO2-Ta2O5 with different compositions calcined at 400 °C
(a) 90%RuO2-10%Ta2O5 (b) 80%RuO2-20%Ta2O5 (c) 70%RuO2-
30%Ta2O5 (d) 60%RuO2-40%Ta2O5 91
Fig. 5.13 SEM of RuO2-Ta2O5 with different compositions calcined at 500 °C (a) 90%RuO2-10%Ta2O5 (b) 80%RuO2-20%Ta2O5 (c) 70%RuO2-
30%Ta2O5 (d) 60%RuO2-40%Ta2O5 92
Fig. 5.14 SEM of RuO2-Ta2O5 with different compositions calcined at 600 °C (a) 90%RuO2-10%Ta2O5 (b) 80%RuO2-20%Ta2O5 (c) 70%RuO2-
30%Ta2O5 (d) 60%RuO2-40%Ta2O5 92
Fig. 5.15 Cyclic voltammetry of RuO2-Ta2O5 calcined at 400 °C with different
compositions in 1.0 M H3PO4 with 20 mV s-1 at 50 °C 93 Fig. 5.16 Cyclic voltammetry of RuO2-Ta2O5 calcined at 500 °C with different
compositions in 1.0 M H3PO4 with 20 mV s-1 at 50 °C 94 Fig. 5.17 Cyclic voltammetry of RuO2-Ta2O5 calcined at 600 °C with different
compositions in 1.0 M H3PO4 with 20 mV s-1 at 50 °C 95 Fig. 5.18 Cyclic voltammetry of 90%RuO2-10%Ta2O5 calcined at different
calcination temperatures and electrolyte (1.0 M H3PO4) temperatures
with 20 mV s-1 98
Fig. 5.19 Cyclic voltammetry of 80%RuO2-20%Ta2O5 calcined at different calcination temperatures and electrolyte (1.0 M H3PO4) temperatures
with 20 mV s-1 99
xiv
Fig. 5.20 Cyclic voltammetry of 70%RuO2-30%Ta2O5 calcined at different calcination temperatures and electrolyte (1.0 M H3PO4) temperatures
with 20 mV s-1 99
Fig. 5.21 In-situ FTIR of 90%RuO2-10%Ta2O5 anode catalyst at different
voltages in 1.0 M H3PO4 electrolyte at 25 °C 101 Fig. 5.22 Chronoamperometry of 90%RuO2-10%Ta2O5 calcined at different
calcination temperatures and electrolyte (1.0 M H3PO4) temperatures 102 Fig. 5.23 Chroamperometry of 80%RuO2-20%Ta2O5 calcined at different
calcination temperatures and electrolyte (1.0 M H3PO4) temperatures 103 Fig. 5.24 Chronoamperometry of 70%RuO2-30%Ta2O5 calcined at different
calcination temperatures and electrolyte (1.0 M H3PO4) temperatures 103 Fig. 5.25 Linear sweep voltammetry using rotating ring disk electrode for
90%RuO2-10%Ta2O5 catalyst calcined at 500 °C in 1.0 M H3PO4
electrolyte at 90 °C with different rotation speeds 105 Fig. 5.26 Linear sweep voltammetry using rotating ring disk electrode for
80%RuO2-20%Ta2O5 catalyst calcined at 500 °C in 1.0 M H3PO4
electrolyte at 90 °C with different rotation speeds 106 Fig. 5.27 Koutecky-Levich plot at different voltages for 90%RuO2-10%Ta2O5
catalyst calcined at 500 °C 107
Fig. 5.28 Linear sweep voltammetry using rotating ring disk electrode for 90%RuO2-10%Ta2O5 catalyst calcined at 500 °C at different
electrolyte (1.0 M H3PO4) temperatures at 2000 rpm 108 Fig. 5.29 i-V curve of PEMWE with different compositions of RuO2-Ta2O5 as
anode catalyst calcined at 400 °C 110
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Fig. 5.30 i-V curve of PEMWE with different compositions of RuO2-Ta2O5 as
anode catalyst calcined at 500 °C 110
Fig. 5.31 i-V curve of PEMWE with different compositions of RuO2-Ta2O5 as
anode catalyst calcined at 600 °C 111
Fig. 5.32 i-V curve of PEMWE of 90%RuO2-10%Ta2O5 as anode catalyst calcined at 500 °C using Celazole PBI membrane with different
operating temperatures 112
Fig. 5.33 i-V curve of PEMWE of 90%RuO2-10%Ta2O5 as anode catalyst calcined at 500 °Cusing NCL PBI membrane with different
operating temperatures 112
Fig. 5.34 Stability of different anode catalysts in high temperature PEMWE 114 Fig. 5.35 FTIR of 90%RuO2-10%Ta2O5 electrocatalyst before and after
PEMWE operation 115
Fig. 5.36 Core level peaks for 90%RuO2-10%Ta2O5 before and after PEMWE
operation (a) Ru 3d (b) Ta 4f and (c) O 1s 117 Fig. 5.37 FTIR of H3PO4 doped PBI membrane before and after experiment 118 Fig. 5.38 SEM of catalyst coated PBI membrane (a) before (b) after PEMWE
operation 119
Fig. 5.39 EDX of catalyst coated PBI membrane (a) before (b) after PEMWE
operation 119
Fig. 5.40 PEMWE anolyte analysis using UV spectrometry 120 Fig. A.1 Flow chart for electrocatalyst synthesis by polyol method 131 Fig. A.2 XRD pattern of RuO2 and IrO2 catalyst prepared by polyol method 132
xvi
Fig. A.3(a) Cyclic voltammetry of RuO2 with different electrolyte (0.5 M H2SO4)
temperature with scan rate of 20 mV sec-1 133 Fig. A.3(b) Cyclic voltammetry of RuO2 with different electrolyte (1.0 M H3PO4)
temperature with scan rate of 20 mV sec-1 133
Fig. A.4(a) Cyclic voltammetry of IrO2 with different electrolyte (0.5 M H2SO4)
temperature with scan rate of 20 mV sec-1 135
Fig. A.4(b) Cyclic voltammetry of IrO2 with different electrolyte (1.0 M H3PO4)
temperature with scan rate of 20 mV sec-1 135
Fig. B.1 Stability of 90%RuO2-10%Ta2O5 electrocatalyst in different
electrolyte (1.0 M H3PO4) temperatures and calcination temperatures 136 Fig. C.1 Apparent activation energy for Nafion composite membranes 137 Fig. C.2 i-V curve of PEMWE with different composite membranes operating
at 70 °C and 80 °C
138
xvii
LIST OF TABLES
Table No. Title Page No.
Table 1.1 Classification of electrolyser and its features 2 Table 1.2 Application areas for hydrogen energy 3 Table 2.1 Literature review on anode catalyst for PEMWE and its
performance
22
Table 3.1 Composition and properties of Nafion® dispersion 42
Table 3.2 Properties of carbon paper 42
Table 3.3 Properties of PBI electrolyte membrane 43 Table 4.1 Apparent activation energy of RuO2 at different calcination
temperature 67
Table 5.1 Onset potential and current density at 1.2 V for OER on RuO2-Ta2O5 catalyst with different compositions calcined at 400 °C
95
Table 5.2 Onset potential and current density at 1.2 V for OER on RuO2-Ta2O5 catalyst with different compositions calcined at 500 °C
95
Table 5.3 Onset potential and current density at 1.2 V for OER on RuO2-Ta2O5 catalyst with different compositions calcined at 600 °C
96
Table 5.4 Anodic peak charge density (qF) of RuO2-Ta2O5 96 Table 5.5 Capacitive charge density (qdl) of RuO2-Ta2O5 97
xviii
Table 5.6 Onset potential and current density at 1.2 V with different electrolyte temperature for OER on 90%RuO2-10%Ta2O5
calcined at 400 °C, 500 °C and 600 °C 100
Table 5.7 Onset potential and current density at 1.2 V with different electrolyte temperature for OER on 80%RuO2-20%Ta2O5
calcined at 400 °C, 500 °C and 600 °C 100
Table 5.8 Onset potential and current density at 1.2 V with different electrolyte temperature for OER on 70%RuO2-30%Ta2O5
calcined at 400 °C, 500 °C and 600 °C 100
Table 5.9 Apparent activation energy of RuO2-Ta2O5 anode
electrocatalyst 104
Table 5.10 Performance of RuO2-Ta2O5 with different compositions
and calcination temperatures at 1.8 V 113 Table 5.11 Energy efficiency of PEMWE operated at 150 °C with
90%RuO2-10%Ta2O5 anode catalyst calcined at 500 °C 121
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NOMENCLATURE
Symbol
Meaning
IC Internal combustion
PEMWE Proton exchange membrane water electrolyser
PEM Proton exchange membrane
OER Oxygen evolution reaction
HER Hydrogen evolution reaction
MEA Membrane electrode assembly
HHV High heating value of hydrogen = 3.55 kWh/Nm3 RRDE Rotating ring disk electrode
EC Energy consumption (Wh/Nm3)
En Nernst potential (V)
H2
P Partial pressure of hydrogen
O2
P Partial pressure of oxygen
H O2
P Partial pressure of water
Go
' Free energy change for the reaction (kJ mol-1) Volume of hydrogen measured (m3) Volume of hydrogen theoretically calculated (m3) R Universal gas constant (8.314 J/mol K)
I Current (A)
T Temperature (K)
t Time (s)
F Faraday’s constant (96485 C/mol)
p Pressure (Pa)
n Number of electrons
H mea2
V
H theo2
V
xx
ηf Faraday efficiency (%)
V Voltage (V)
Hydrogen production rate (Nm3/h),
Q Total charge (C)
ηE Energy efficiency (%)
Etn Thermoneutral voltage (V)
R Universal rate constant (8.314 J/ mol K) RH
2