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Avogadro constant

The Avogadro constant, denoted N_A, is a fundamental physical constant that serves as the proportionality factor relating the number of elementary entities (such as atoms, molecules, ions, or subatomic particles) in a substance to the amount of substance in moles.^[1] It defines the mole, the SI unit for amount of substance, such that one mole contains exactly N_A entities.^[2] Since the 2019 revision of the International System of Units (SI), N_A has been fixed at the exact value $6.02214076 \times 10^{23} mol^{-1}, making it one of the seven defining constants of the SI alongside the speed of light, Planck's constant, and others.^[1] This precise value enables the mole to be defined independently of the kilogram, linking microscopic particle counts directly to macroscopic measurements of mass and quantity.^[3] Named in honor of Italian chemist Amedeo Avogadro (1776–1856), who in 1811 proposed the hypothesis that equal volumes of different gases at the same temperature and pressure contain the same number of molecules, the constant itself was not determined during his lifetime.^[4] Experimental determinations began in the late 19th century with estimates from electrolysis and gas kinetics, but a reliable value emerged in 1908–1909 through the work of French physicist Jean Perrin, who used observations of Brownian motion to calculate N_A as approximately $6.0 \times 10^{23} mol^{-1} and popularized the term "Avogadro's constant."^[5] Perrin's measurements, which earned him the 1926 Nobel Prize in Physics, confirmed the atomic theory and bridged the gap between statistical mechanics and observable phenomena.^[2] Over the 20th century, refinements came from methods like X-ray crystallography, the oil drop experiment, and the International Avogadro Project's silicon sphere measurements, reducing uncertainty to parts per billion by the 2010s.^[3] In modern chemistry and physics, N_A is indispensable for stoichiometry, quantifying reaction yields, and scaling properties from atomic to bulk levels, such as converting molar mass to atomic mass units.^[6] Its adoption as an exact constant in 2019 eliminated dependencies on experimental artifacts like the international prototype kilogram, ensuring long-term stability for metrology and advancing fields from materials science to environmental modeling.^[3]

Definition and Value

Conceptual Basis

The Avogadro constant, denoted N_A, is defined as the proportionality factor between the amount of substance, measured in moles, and the number of specified elementary entities, such as atoms, molecules, ions, electrons, or other particles, in that substance.^[1] This constant establishes a direct link between the discrete, microscopic realm of individual particles—too numerous to count directly—and the continuous, macroscopic quantities observable in laboratory settings, like mass or volume.^[2] By providing a standardized scaling factor, N_A enables chemists and physicists to translate between these scales, making quantitative predictions about material properties feasible without enumerating each particle.^[7] The mole, the International System of Units (SI) base unit for amount of substance, is formally the quantity of substance containing exactly N_A elementary entities of a specified type.^[8] Prior to the 2019 SI revision, the mole was operationally tied to the mass of 12 grams of the carbon-12 isotope, which implicitly defined N_A through that reference; the modern definition fixes N_A exactly, rendering the mole independent of any particular substance while preserving its role in stoichiometric calculations.^[7] This conceptual framework underscores the mole's purpose: not as a measure of mass or volume, but as a count of entities scaled to practical proportions. The mathematical relation expressing this proportionality is

n = \frac{N}{N_A},

where n represents the amount of substance in moles, N is the total number of elementary entities, and N_A has units of inverse moles (mol⁻¹).^[1] Unlike particle number density, which varies with spatial arrangement and is expressed as entities per unit volume (a local, condition-dependent property), N_A is a dimensionless universal constant in its numerical value, invariant across all substances and physical states.^[8] This fixed nature ensures consistency in defining chemical equivalents and reaction extents, distinguishing N_A as a cornerstone of metrology rather than a tunable parameter.^[9]

Numerical Value and Units

Following the 2019 revision of the International System of Units (SI), the Avogadro constant N_A is defined to have the exact value $6.02214076 \times 10^{23} mol^{-1}.^[10] This fixed numerical value establishes the mole as the amount of substance containing exactly this number of elementary entities, such as atoms, molecules, or ions, thereby defining the mole independently of any mass-based standards like the kilogram or carbon-12.^[10]^[2] The dimension of the Avogadro constant is mol^{-1}, representing a pure number of entities per mole, with no other physical dimensions involved.^[10] This unit structure directly influences derived quantities, such as the unified atomic mass unit (u), defined as u = 1 g mol^{-1} / N_A, which equals approximately $1.66053906660 \times 10^{-24} g or $1.66053906660 \times 10^{-27} kg.^[10] Prior to the 2019 redefinition, the Avogadro constant was a measured quantity subject to uncertainty; the CODATA 2014 recommended value was $6.022140857(74) \times 10^{23} mol^{-1}, where the uncertainty reflects the standard deviation in the last two digits.^[11] By fixing N_A exactly, the redefinition eliminates propagation of measurement uncertainties into calculations involving molar masses and amount of substance, ensuring higher precision and consistency in applications across metrology, chemistry, and physics.^[10]^[2]

Historical Development

Avogadro's Hypothesis and Early Ideas

In 1811, Amedeo Avogadro proposed a fundamental hypothesis in chemical theory, stating that equal volumes of different gases, at the same temperature and pressure, contain an equal number of molecules.^[12] This idea sought to explain discrepancies in gas volumes during chemical reactions, distinguishing between atoms and molecules and implying a universal constant relating the number of molecules to macroscopic quantities like volume.^[13] Avogadro's work built on John Dalton's atomic theory but addressed its limitations in predicting reaction stoichiometries for gases, such as the formation of water from hydrogen and oxygen.^[14] A similar hypothesis was independently advanced by André-Marie Ampère in 1814, who suggested that equal volumes of gases under identical conditions hold the same number of "integral molecules," though he emphasized polyatomic structures for certain gases like oxygen.^[4] Despite these contributions, Avogadro's and Ampère's ideas faced resistance from prominent chemists, including Dalton, and remained overlooked for decades due to prevailing views favoring simpler atomic models without molecular distinctions.^[15] The revival of Avogadro's hypothesis came through the efforts of Stanislao Cannizzaro in 1858, who published a pamphlet applying it to determine atomic and molecular weights consistently across elements and compounds.^[16] Cannizzaro distributed this work at the 1860 Karlsruhe Congress, where he argued for its adoption to resolve ongoing debates in chemical nomenclature and atomic theory, influencing younger chemists like Dmitri Mendeleev.^[17] This advocacy shifted the focus toward a unified understanding of molecular quantities without yet assigning a specific numerical value to the constant. Conceptual progress continued with Wilhelm Ostwald, who in 1893 introduced the term "mole" (from the German "Mol," derived from "Molekül") to denote the quantity of a substance whose mass in grams equals its molecular weight, providing a practical link between chemical formulas and laboratory measurements.^[18] Building on this, Jean Perrin in 1909 used observations of Brownian motion to experimentally confirm the discrete nature of atoms and molecules, demonstrating that random particle movements aligned with kinetic theory predictions and reinforcing the existence of a fixed number of entities per mole.^[19] These developments established the theoretical foundation for the Avogadro constant as a universal proportionality factor, emphasizing its role in bridging observable chemical behavior to the unseen molecular world, though quantitative determination remained a future pursuit.

Initial Quantitative Determinations

The first quantitative estimate of what would later be recognized as the Avogadro constant emerged from Johann Josef Loschmidt's 1865 work on the kinetic theory of gases. Loschmidt calculated the number of molecules in one liter of an ideal gas at standard temperature and pressure (0°C and 1 atm), termed Loschmidt's number, to be approximately $2.7 \times 10^{22} molecules per liter. This value provided an early link to the Avogadro constant N_A through the relation N_A = n_L \times V_m, where n_L is Loschmidt's number density adjusted for volume and V_m is the molar volume of the gas at those conditions (approximately 22.4 liters per mole). Subsequent efforts in the late 19th and early 20th centuries employed methods such as electrolysis guided by Faraday's laws and applications of gas laws to refine estimates toward $6 \times 10^{23} mol^{-1}. Electrolysis experiments measured the charge required to liberate or deposit one gram-equivalent of a substance, yielding the Faraday constant F, which relates to N_A via F = N_A e (where e is the elementary charge); combined with kinetic gas theory for molecular sizes and densities, these yielded values around $6 \times 10^{23} mol^{-1}. A pivotal advancement came from Jean Baptiste Perrin's 1910 experiments on sedimentation equilibrium in colloidal suspensions, where the vertical distribution of particles under gravity mirrored the barometric formula for gases, providing a direct measure of N_A \approx 6.0 \times 10^{23} mol^{-1} and confirming the discrete nature of matter.^[20] By 1929, Raymond T. Birge and Donald H. Pegram synthesized data from multiple approaches—including electrolysis, gas viscosity, and early X-ray diffraction—into a comprehensive review, arriving at N_A = 6.06 \times 10^{23} mol^{-1}. This compilation marked a milestone in accuracy, reducing uncertainty to about 1%, though discrepancies persisted across methods.^[20] These initial determinations faced significant challenges, primarily from imprecise knowledge of atomic weights, which affected equivalent masses in electrolysis, and inaccuracies in gas density measurements at standard conditions, limiting the reliability of molar volume calculations.

Advances in Precision Measurement

The precision of the Avogadro constant was significantly advanced in the late 20th century through the X-ray crystal density (XRCD) method, which determines N_A by measuring the mass, volume, and lattice parameter of a silicon crystal to count its atoms. This technique relied on nearly perfect spheres of high-purity silicon, ideally the isotope ^{28}Si, whose diamond cubic lattice allows accurate atom counting via the relation N_A = M / (n \cdot \rho \cdot a^3), where M is the molar mass, \rho is the density, a is the lattice parameter, and n=8 is the number of atoms per unit cell. Efforts by the International Bureau of Weights and Measures (BIPM) in the 1970s initiated this approach with natural silicon crystals, achieving initial relative uncertainties around $10^{-6}, while the 1980s and 1990s saw refinements through international collaboration to produce enriched ^{28}Si spheres with isotopic purity exceeding 99.99%.^[3]^[21] The International Avogadro Project, launched in the early 1990s under the coordination of BIPM and involving institutes like NIST and PTB, targeted a relative uncertainty of $10^{-8} by combining X-ray interferometry for lattice parameter measurement (to nanometer precision) with hydrostatic weighing for density and isotope ratio mass spectrometry for molar mass. A landmark 1998 measurement using a ^{28}Si sphere yielded N_A = 6.02214199 \times 10^{23} mol^{-1} with a relative standard uncertainty of $7.8 \times 10^{-8}, incorporating improved crystal growth and surface metrology to minimize oxide layers and impurities. This result informed the 1998 CODATA recommended value of N_A = 6.02214199(47) \times 10^{23} mol^{-1}, reflecting a synthesis of XRCD data with other inputs. Cross-verification came from complementary techniques, including electron diffraction to confirm lattice structure and spacing in silicon samples, and neutron activation analysis combined with interferometry to quantify isotopic impurities and lattice parameters independently of X-ray absorption effects. These methods helped validate the XRCD results, with the 1980s precursor efforts to the Avogadro Project establishing protocols for $10^{-8} accuracy through enhanced purity (impurity levels below 10^{15} cm^{-3}) and angle [interferometry](/page/Interferometry). By the early 2000s, further optimizations in [sphere](/page/Sphere) polishing and volume correction led to the 2002 CODATA adjustment to N_A = 6.0221415(10) \times 10^{23} mol^{-1}

, with uncertainty reduced to &#36;1.7 \times 10^{-8}

.^[22]^[23] Prior to the 2019 SI redefinition, these high-precision N_A measurements played a pivotal role in linking atomic-scale counting to the kilogram by enabling computation of the Planck constant h via h = (M / N_A) \cdot (v / f), where comparisons with Kibble balance experiments confirmed consistency at the $10^{-8} level, supporting the mutual adoption of fixed values for N_A and h.^[3]

Incorporation into SI Definitions

In 1971, the 14th General Conference on Weights and Measures (CGPM) introduced the mole as a base unit of the International System of Units (SI), defining it as the amount of substance containing as many elementary entities as there are atoms in 0.012 kg of carbon-12.^[24] This definition linked the mole directly to the kilogram artifact and fixed the molar mass of carbon-12 at exactly 12 g/mol, thereby implicitly establishing the Avogadro constant N_A at approximately $6.022 \times 10^{23} mol^{-1}, based on contemporary measurements of the number of atoms in that mass.^[10] The specification of elementary entities—such as atoms, molecules, ions, or other particles—was required when using the mole, ensuring clarity in chemical and physical applications.^[24] The evolution toward a more stable and universal SI culminated in the 2019 redefinition, approved by the 26th CGPM in 2018 and effective from May 20, 2019. Under this revision, the mole is now defined such that one mole contains exactly $6.02214076 \times 10^{23} elementary entities, fixing the Avogadro constant precisely at N_A = 6.02214076 \times 10^{23} mol^{-1}.^[25] This change decoupled the mole from the kilogram's artifact-based definition, aligning it instead with invariant fundamental constants and enabling independent realization through quantum standards.^[10] The redefinition also abrogated the 1971 mole definition, shifting the molar mass of carbon-12 to an experimentally determined value rather than a fixed one.^[26] The primary rationale for incorporating the Avogadro constant into the SI definitions was to resolve the long-standing "kilogram problem," where the international prototype kilogram exhibited instability over time due to surface contamination and other effects, limiting measurement precision.^[10] This was addressed by redefining the kilogram in terms of the Planck constant h = 6.62607015 \times 10^{-34} J s, supported by complementary approaches like the Kibble balance—which relates mass to electrical power via h and the elementary charge—and the Avogadro experiment, which uses X-ray crystal density measurements of silicon-28 spheres to link N_A to the kilogram.^[26] The consistency of these methods was confirmed by the 2018 CODATA adjustment, which provided a recommended value for N_A of $6.02214076(59) \times 10^{23} mol^{-1} with relative uncertainty below $10^{-8}, meeting the criteria for fixation without disrupting existing measurements.^[27] As of 2025, the fixed value of the Avogadro constant has remained unchanged since the 2019 redefinition, maintaining the SI's stability and universality.^[25] Ongoing verification experiments, including refined Kibble balance operations and silicon sphere analyses at national metrology institutes, continue to test the consistency of N_A with other defining constants, ensuring no discrepancies arise from new data.^[26] These efforts affirm the redefinition's success in providing a robust foundation for metrology in chemistry and physics.

Physical Significance

Linking Macroscopic and Microscopic Scales

The Avogadro constant, N_A, plays a pivotal role in bridging the gap between macroscopic observations and microscopic realities by providing a universal scaling factor between the number of entities in a sample and measurable bulk properties. In essence, it defines the mole as the amount of substance containing N_A entities, allowing chemists and physicists to relate quantities like mass and volume at the laboratory scale to the counts of atoms or molecules. For a pure substance, the molar mass M (in grams per mole) equals the mass of N_A entities, expressed as M = N_A \times m_\text{entity}, where m_\text{entity} is the mass of a single particle; this relation directly converts between gram-scale measurements and atomic-level counts.^[28]^[29] A concrete example of this scaling is the calculation of an individual atom's mass from its molar mass. For hydrogen, with a molar mass of approximately 1.008 g/mol, the mass of a single hydrogen atom is m_\text{H} \approx 1.008 / N_A grams. Using N_A \approx 6.022 \times 10^{23} mol^{-1}, this yields about $1.67 \times 10^{-24} g per atom. More precisely, since the atomic mass unit (u) is defined such that 1 u corresponds to 1 g/mol divided by N_A, the mass of 1 u is $1.660539 \times 10^{-24} g, underscoring how N_A translates unified atomic masses into tangible gram values for everyday chemical handling.^[30]^[31] Similarly, N_A links particle counts to macroscopic volumes, as seen in the behavior of gases. One mole of an ideal gas at standard temperature and pressure (STP: 0°C and 1 atm) occupies approximately 22.4 L, meaning N_A particles fill this volume under those conditions; this molar volume provides a direct way to estimate the space required for vast numbers of molecules in bulk samples without needing to count them individually.^[32]^[33] The sheer magnitude of N_A vividly illustrates the vast disparity between atomic and human scales: even a small macroscopic sample, like a gram of material, contains N_A particles, a number so immense that if the entities in one mole were redistributed to occupy individual cubic meters of space, the total volume would encompass roughly 600 times the volume of Earth, highlighting the profound leap N_A enables across these realms.^[34]^[29]

Applications in Chemistry and Physics

In chemistry, the Avogadro constant serves as the bridge between macroscopic quantities like mass and microscopic entities in stoichiometric calculations, enabling the determination of reactant and product amounts in balanced equations through molar ratios. For instance, to calculate the number of molecules involved in a reaction such as the combustion of glucose, one mole of glucose (180.16 g) corresponds to exactly $6.022 \times 10^{23} molecules, allowing precise scaling of reaction yields.^[35] Similarly, empirical formulas are derived from mass percentage data by converting elemental masses to moles using the constant divided by atomic masses, as seen in analyzing compounds like caffeine from combustion analysis results.^[35] Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules, relies on the constant to quantify particle counts per mole, facilitating gas stoichiometry in reactions like the synthesis of ammonia. This application is crucial for predicting volumes in industrial processes, where deviations from ideality are corrected using van der Waals equations, but the constant remains the reference for ideal behavior./14%3A_The_Behavior_of_Gases/14.07%3A_Avogadro%27s_Law) In physics, the Avogadro constant is applied in particle physics to compute the number density of target atoms in accelerator experiments, where the interaction rate depends on the number of atoms per unit volume, calculated as \rho N_A / M with \rho as density and M as molar mass. For example, in fixed-target collisions at facilities like CERN, this determines the luminosity and expected event rates for subatomic particle production.^[36] In statistical mechanics, it scales ensemble averages over large particle numbers, such as in the ideal gas law derivation where the total energy U = \frac{3}{2} N k_B T uses N = n N_A to connect microscopic Boltzmann constant k_B to macroscopic gas constant R.^[37] Practical examples extend to nanotechnology and materials science, where the constant calibrates doping levels in semiconductors; dopant concentrations like $10^{15} atoms/cm³ are expressed relative to N_A for precise control in device fabrication, ensuring conductivity thresholds in silicon wafers.^[38] In pharmaceuticals, drug dosing for bioavailability often uses molar units to compare efficacy across compounds, as the therapeutic concentration of a drug like dopamine is interpreted in terms of molecules per vesicle, scaled by N_A for metabolic scaling.^[39] However, approximations involving the Avogadro constant falter in non-ideal gases, where intermolecular forces alter volume-mole relations beyond the ideal gas assumption, requiring corrections like the compressibility factor in real-gas equations. In quantum systems with few particles (far below N_A), statistical ensembles lose validity due to significant fluctuations, limiting its use in nanoscale or low-density regimes like ultracold atomic clouds./14%3A_The_Behavior_of_Gases/14.07%3A_Avogadro%27s_Law)

Relations to Other Constants

Thermodynamic Relations

The Avogadro constant N_A connects macroscopic thermodynamic quantities to microscopic statistical mechanics through its relation to the Boltzmann constant k_B and the molar gas constant R. Specifically, k_B = R / N_A, where R = 8.314462618 \, \mathrm{J \cdot mol^{-1} \cdot K^{-1}} links energy scales per mole to those per particle.^[40] This relation enables the translation of molar thermal energy expressions, such as the average kinetic energy per mole \frac{3}{2} R T, to the per-particle form \frac{3}{2} k_B T.^[40] In the ideal gas law, the Avogadro constant bridges the formulation PV = n R T—using moles n—to the particle-based version PV = N k_B T, where N = n N_A is the total number of particles, yielding PV = n N_A k_B T.^[41] This equivalence underscores N_A's fundamental role in unifying bulk thermodynamic behavior with molecular kinetics.^[41] The entropy of a monatomic ideal gas also incorporates N_A via the Sackur-Tetrode equation, derived from statistical mechanics. For N particles of mass m in volume V with internal energy U, the entropy S is given by

S = N k_B \left[ \ln \left( \frac{V}{N} \left( \frac{4 \pi m U}{3 N h^2} \right)^{3/2} \right) + \frac{5}{2} \right],

where h is Planck's constant; in molar form, this introduces logarithmic dependence on N_A through the phase space volume and Stirling's approximation for indistinguishability.^[42] The equation quantifies the configurational entropy, with N_A ensuring consistency between per-mole and per-particle entropies.^[43] Following the 2019 SI redefinition, N_A is fixed at exactly $6.02214076 \times 10^{23} \, \mathrm{mol^{-1}}, rendering k_B exactly $1.380649 \times 10^{-23} \, \mathrm{J \cdot K^{-1}} and eliminating experimental uncertainty in these thermodynamic relations.^[2] This exactness enhances precision in applications like equation-of-state modeling and statistical thermodynamics.^[2]

Electrochemical and Other Links

The Avogadro constant N_A is intrinsically connected to electrochemistry via the Faraday constant F, defined as F = N_A e, where e is the elementary charge with a fixed value of $1.602176634 \times 10^{-19} C.^[44]^[45] This relation establishes F as the charge carried by one mole of singly charged particles, approximately 96485.3321 C/mol, facilitating the quantification of electrical charge in molar terms during redox processes.^[46] In electrolysis, this linkage underpins Faraday's second law, which states that the mass m of a substance deposited or liberated is proportional to the total charge Q = I t passed through the electrolyte, given by the equation

m = \frac{M Q}{n F} = \frac{M I t}{n F},

where M is the molar mass of the substance, I is the electric current, t is the duration, and n is the stoichiometric number of electrons transferred per mole of substance.^[47]^[48] This formula allows precise determination of molar masses from measured deposition masses in electrolytic cells.^[48] The practical significance of this electrochemical tie is evident in applications such as electroplating, where F (and thus N_A) enables calculations of metal layer thickness from applied current and time, ensuring controlled deposition for corrosion-resistant coatings on industrial components.^[49] Similarly, in battery design, F is essential for computing theoretical capacities, as seen in lithium-ion systems where the specific capacity C (in mAh/g) relates to the active material's molar mass and electron transfer via C = \frac{n F}{3.6 M}, optimizing energy density and efficiency.^[50]^[51] Other connections to physical constants are more indirect but noteworthy; for example, N_A links to the Planck constant h through the fine-structure constant \alpha \approx 1/137, defined as \alpha = \frac{e^2}{4\pi\epsilon_0 \hbar c} with \hbar = h/(2\pi) and c the speed of light, reflecting the strength of electromagnetic interactions at atomic scales. In atomic units, the speed of light manifests as c_\text{au} = 1/\alpha, underscoring how N_A bridges molar quantities to quantum electrodynamic parameters via e. Nonetheless, the electrochemical relations via F remain the most direct and widely applied.^[46]

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Ultra low doses and biological amplification - PubMed - NIH
Jun 19, 2021 · This paper describes evidence establishing that ultra-low doses of diverse chemical agents at concentrations from 10 -18 to 10 -24 M (eg, approaching and/or ...
[40]
Fundamental Physical Constants from NIST
### Summary of Thermodynamic Constants (Post-2019, CODATA 2022)
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[PDF] Measured relationship between thermodynamic pressure and ...
and molar gas constant R ¼ kB NA is the product of. Boltzmann's constant kB and the Avogadro number NA. In the revised SI, R has no uncertainty.18 The ...
[42]
[PDF] Lecture 4: Temperature
stand this yet, but the correct formula for an ideal gas is the Sackur-Tetrode equation: S =NkB ln V. N. +. 3. 2ln. 4 mE. 3Nh2 + 52. (18). There are 3 di ...
[43]
[PDF] The Sackur-Tetrode equation and the measure of entropy
The number of configurations in phase space must be divided by N! to make entropy extensive (and to take into account the indistinguishability of par- ticles).Missing: monatomic | Show results with:monatomic
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elementary charge - CODATA Value
elementary charge $e$. Numerical value, 1.602 176 634 x 10-19 C. Standard uncertainty, (exact). Relative standard uncertainty, (exact).
[45]
Introduction to the constants for nonexperts 19001920
These two quantities are related by the simple equation that states that the Faraday constant is equal to the Avogadro constant times unit of charge, or F = Ne ...
[46]
[PDF] CODATA recommended values of the fundamental physical constants
Sep 26, 2016 · reports describing the 1998, 2002, 2006, 2010, and 2014 adjustments, or sometimes the adjustments themselves, as. CODATA-XX, where XX is 98 ...
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[PDF] For Peer Review Only - IUPAC
Feb 27, 2019 · Of importance to electroanalytical chemistry are the values of the Boltzmann constant, the elementary charge, and the Avogadro constant. These ...
[48]
[PDF] Determination of the value of the faraday with a silver-perchloric acid ...
An accurate value of the faraday has been determined by the electrolytic dissolution of metallic silver in aqueous solutions of perchloric acid.
[49]
Electrochemistry Encyclopedia -- Electroplating
... Faraday constant" "F". Therefore, the number of moles of metal reduced by charge "Q" can be obtained as: [3] m = Q / (n F). On the other hand, the total ...<|separator|>
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[PDF] Modeling the Performance and Cost of Lithium-Ion Batteries for ...
The relationship between capacity and battery energy is described by Equation 3.7. ... F is Faraday's constant. The influence of the interfacial impedance ...
[51]
Faradays Law of Electrolysis - an overview | ScienceDirect Topics
The charge of one mole of electrons is called Faraday's Constant and is denoted by F; Faraday's constant is equal to. (2.39) F = N A q e = 6.022140857 × 10 ...