Storage of electricity within an electrochemical cell
Simplified view of a double-layer with specifically adsorbed ions which have submitted their charge to the electrode to explain the faradaic charge-transfer of the pseudocapacitance.
Pseudocapacitance is the
) since only a charge-transfer takes place.
Faradaic pseudocapacitance only occurs together with static double-layer capacitance . Pseudocapacitance and double-layer capacitance both contribute inseparably to the total capacitance value.
The amount of pseudocapacitance depends on the surface area, material and structure of the electrodes. Pseudocapacitance may contribute more capacitance than double-layer capacitance for the same surface area by 100x.[1]
The amount of electric charge stored in a pseudocapacitance is linearly proportional to the applied voltage . The unit of pseudocapacitance is farad .
History
Redox reactions
Differences
Rechargeable batteries
Redox reactions in batteries with faradaic charge-transfer between an electrolyte and the surface of an electrode were characterized decades ago. These chemical processes are associated with chemical reactions of the electrode materials usually with attendant phase changes . Although these chemical processes are relatively reversible, battery charge/discharge cycles often irreversibly produce unreversed chemical reaction products of the reagents. Accordingly, the cycle-life of rechargeable batteries is usually limited. Further, the reaction products lower power density . Additionally, the chemical processes are relatively slow, extending charge/discharge times.
Electro-chemical capacitors
Schematic representation of a double layer on an electrode (BMD) model. 1. Inner Helmholtz plane, (IHP), 2. Outer Helmholtz plane (OHP), 3. Diffuse layer, 4. Solvated electrolyte ions (cations) 5. Specifically adsorbed ions (redox ion, which contributes to the pseudocapacitance), 6. Molecules of the solvent
A fundamental difference between redox reactions in batteries and in electrochemical capacitors (supercapacitors) is that in the latter, the reactions are a very fast sequence of reversible processes with electron transfer without any phase changes of the electrode molecules. They do not involve making or breaking chemical bonds . The de-solvated atoms or ions contributing the pseudocapacitance simply cling[4] to the atomic structure of the electrode and charges are distributed on surfaces by physical adsorption processes. Compared with batteries, supercapacitor faradaic processes are much faster and more stable over time, because they leave only traces of reaction products. Despite the reduced amount of these products, they cause capacitance degradation. This behavior is the essence of pseudocapacitance.
Pseudocapacitive processes lead to a charge-dependent, linear capacitive behavior, as well as the accomplishment of non-faradaic double-layer capacitance in contrast to batteries, which have a nearly charge-independent behavior. The amount of pseudocapacitance depends on the surface area, material and structure of the electrodes. The pseudocapacitance may exceed the value of double-layer capacitance for the same surface area by 100x.[1]
Capacitance functionality
Intercalated metal atoms between planar graphite layers
adsorbed by the electrode's surface atoms. They are specifically adsorbed and deliver their charge to the electrode. In other words, the ions in the electrolyte within the Helmholtz double-layer also act as
electron donors and transfer electrons to the electrode atoms, resulting in a
faradaic current . This faradaic
charge transfer , originated by a fast sequence of reversible
redox reactions,
electrosorptions or
intercalation processes between electrolyte and the electrode surface is called pseudocapacitance.
[5]
Depending on the electrode's structure or surface material, pseudocapacitance can originate when specifically adsorbed ions pervade the double-layer, proceeding in several one-electron stages. The electrons involved in the faradaic processes are transferred to or from the electrode's valence-electron states (orbitals ) and flow through the external circuit to the opposite electrode where a second double-layer with an equal number of opposite-charged ions forms. The electrons remain in the strongly ionized and electrode surface's "electron hungry" transition-metal ions and are not transferred to the adsorbed ions. This kind of pseudocapacitance has a linear function within narrow limits and is determined by the potential-dependent degree of surface coverage of the adsorbed anions. The storage capacity of the pseudocapacitance is limited by the finite quantity of reagent or of available surface.
Systems that give rise to pseudocapacitance:[5]
Redox system: Ox + ze‾ ⇌ Red
Intercalation system: Li+ in "Ma2 "
Electrosorption , underpotential deposition of metal adatoms or H: M+ + ze‾ + S ⇌ SM or H+ + e‾ + S ⇌ SH (S = surface lattice sites)
All three types of electrochemical processes have appeared in supercapacitors.[5]
When discharging pseudocapacitance, the charge transfer is reversed and the ions or atoms leave the double-layer and spread throughout the electrolyte.
Materials
Electrodes' ability to produce pseudocapacitance strongly depends on the electrode materials' chemical affinity to the ions adsorbed on the electrode surface as well as on the electrode pore structure and dimension. Materials exhibiting redox behavior for use as pseudocapacitor electrodes are
transition-metal oxides inserted by doping in the conductive electrode material such as active carbon, as well as conducting polymers such as
polyaniline or derivatives of
polythiophene covering the electrode material.
Transition metal oxides/sulfides
These materials provide high pseudocapacitance and were thoroughly studied by Conway.[1] [7] Many oxides of transition metals like ruthenium (RuO2 ), iridium (IrO2 ), iron (Fe3 O4 ), manganese (MnO2 ) or sulfides such as titanium sulfide (TiS2 ) or their combinations generate faradaic electron–transferring reactions with low conducting resistance.[citation needed ]
valence orbitals
. The electron transfer reaction is very fast and can be accompanied with high currents.
The electron transfer reaction takes place according to:
R
u
O
2
+
x
H
+
+
x
e
−
↔
R
u
O
2
−
x
(
O
H
)
x
{\displaystyle \mathrm {RuO_{2}+xH^{+}+xe^{-}\leftrightarrow RuO_{2-x}(OH)_{x}} }
where
0
≤
x
≤
2
{\displaystyle 0\leq x\leq 2}
[8]
During charge and discharge, H+ (protons ) are incorporated into or removed from the RuO2 crystal lattice , which generates storage of electrical energy without chemical transformation. The OH groups are deposited as a molecular layer on the electrode surface and remain in the region of the Helmholtz layer. Since the measurable voltage from the redox reaction is proportional to the charged state, the reaction behaves like a capacitor rather than a battery, whose voltage is largely independent of the state of charge.
Conducting polymers
Another type of material with a high amount of pseudocapacitance is electron-conducting polymers. Conductive polymer such as polyaniline , polythiophene , polypyrrole and polyacetylene have a lower reversibility of the redox processes involving faradaic charge transfer than transition metal oxides, and suffer from a limited stability during cycling.[citation needed ] Such electrodes employ electrochemical doping or dedoping of the polymers with anions and cations. Highest capacitance and power density are achieved with a n/p-type polymer configuration, with one negatively charged (n-doped) and one positively charged (p-doped) electrode.
Structure
Pseudocapacitance may originate from the electrode structure, especially from the material pore size. The use of
nanoporous materials have diameters in the range of <2 nm that can be referred to as intercalated pores. Solvated ions in the electrolyte are unable to enter these small pores, but de-solvated ions that have reduced their ion dimensions are able to enter, resulting in larger ionic packing density and increased charge storage. The tailored sizes of pores in nano-structured carbon electrodes can maximize ion confinement, increasing specific capacitance by faradaic
H2 adsorption treatment. Occupation of these pores by de-solvated ions from the electrolyte solution occurs according to (faradaic) intercalation.
[9] [10] [11]
Verification
A cyclic voltammogram shows the fundamental difference of the current curves between static capacitors and pseudocapacitors
Pseudocapacitance properties can be expressed in a cyclic voltammogram . For an ideal double-layer capacitor, the current flow is reversed immediately upon reversing the potential yielding a rectangular-shaped voltammogram, with a current independent of the electrode potential. For double-layer capacitors with resistive losses, the shape changes to a parallelogram . In faradaic electrodes the electrical charge stored in the capacitor is strongly dependent on the potential, therefore, the voltammetry characteristics deviate from the parallelogram due to a delay while reversing the potential, ultimately coming from kinetic charging processes.[12] [13]
Applications
Pseudocapacitance is an important property in supercapacitors .
Literature
Héctor D. Abruña ; Yasuyuki Kiya; Jay C. Henderson (2008), "Batteries and electrochemical capacitors" (PDF) , Physics Today , no. 12, pp. 43–47
Béguin, Francois; Raymundo-Piñero, E.; .
Müller, Klaus; Bockris, J. O'M.; Devanathan, M. A. V. (1965). "On the Structure of Charged Interfaces" . Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences . 274 (1356): 55–79. .
B. E. Conway (1999), Electrochemical Supercapacitors: Scientific Fundamentals and Technological Applications (in German), Berlin: Springer,
Leitner, K. W.; Winter, M.; Besenhard, J. O. (December 2003). "Composite supercapacitor electrodes". Journal of Solid State Electrochemistry . 8 (1): 15–16. .
Yu M., Volfkovich; Serdyuk, T. M. (September 2002). "Electrochemical Capacitors". Russian Journal of Electrochemistry . 38 (9): 935–959. .
Aiping Yu; Aaron Davies; Zhongwei Chen (2011). "8 - Electrochemical Supercapacitors" . In Jiujun Zhang; Lei Zhang; Hansan Liu; Andy Sun; Ru-Shi Liu (eds.). Electrochemical Technologies for Energy Storage and Conversion, Band 1 . Weinheim: Wiley-VCH. pp. 317–376. .
References
^
^ Marin S. Halper, James C. Ellenbogen (March 2006). Supercapacitors: A Brief Overview (PDF) (Technical report). MITRE Nanosystems Group. Archived from the original (PDF) on 2014-02-01. Retrieved 2014-01-20 .
.
^ a b Garthwaite, Josie (12 July 2011). "How ultracapacitors work (and why they fall short)" . Earth2Tech . GigaOM Network. Archived from the original on 22 November 2012. Retrieved 23 April 2013 .
^ a b c B.E. Conway, W.G. Pell, Double-layer and pseudocapacitance types of electrochemical capacitors and their applications to the development of hybrid components
.
^ P. Simon, Y.Gogotsi, Materials for electrochemical capacitors, nature materials , VOL 7, NOVEMBER 2008
^ A.G. Pandolfo, A.F. Hollenkamp, Carbon properties and their role in supercapacitors Archived 2014-01-02 at the Wayback Machine , Journal of Power Sources 157 (2006) 11–27
^ B.P. Bakhmatyuk, B.Ya. Venhryn, I.I. Grygorchak, M.M. Micov and S.I. Mudry, INTERCALATION PSEUDO-CAPACITANCE IN CARBON SYSTEMS OF ENERGY STORAGE
^ P. Simon, A. Burke, Nanostructured carbons: Double-Layer capacitance and more Archived 2018-12-14 at the Wayback Machine
^ Elżbieta Frąckowiak , Francois Beguin, PERGAMON, Carbon 39 (2001) 937–950, Carbon materials for the electrochemical storage of energy in Capacitors
^ Why does an ideal capacitor give rise to a rectangular cyclic voltammogram