Question: What had Faraday concluded based on his electrochemical experiments?
About the article "Electrochemistry", section "First law".

Candidate passages:
Faraday's laws of electrolysis are quantitative relationships based on the electrochemical researches published by Michael Faraday in 1834. 
Use in electrometallurgy.
Bird's cell.
A variant of the Daniell cell was invented in 1837 by the Guy's hospital physician Golding Bird who used a plaster of Paris barrier to keep the solutions separate.
Bird's experiments with this cell were of some importance to the new discipline of electrometallurgy.
A surprising result from Bird's experiments was the deposition of copper on the porous plaster and in veins running through it without any contact with the metal electrodes.
So surprising, in fact, that it was at first disbelieved by electrochemical investigators, including Michael Faraday.
Bird himself had to carefully examine his apparatus for inadvertent contact, perhaps through the growth of copper "whiskers", before he was convinced of the result.
Deposition of copper, and other metals, had been previously noted, but always previously it had been metal on metal electrode. 
In 1836, Michael Faraday observed that the excess charge on a charged conductor resided only on its exterior and had no influence on anything enclosed within it.
To demonstrate this fact, he built a room coated with metal foil and allowed high-voltage discharges from an electrostatic generator to strike the outside of the room.
He used an electroscope to show that there was no electric charge present on the inside of the room's walls.
Although this cage effect has been attributed to Michael Faraday's famous ice pail experiments performed in 1843, it was Benjamin Franklin in 1755 who observed the effect by lowering an uncharged cork ball suspended on a silk thread through an opening in an electrically charged metal can.
In his words, "the cork was not attracted to the inside of the can as it would have been to the outside, and though it touched the bottom, yet when drawn out it was not found to be electrified (charged) by that touch, as it would have been by touching the outside.
The fact is singular."
Franklin had discovered the behavior of what we now refer to as a Faraday cage or shield (based on one of Faraday's famous ice pail experiments which duplicated Franklin's cork and can). 
Faraday is best known for his work regarding electricity and magnetism.
His first recorded experiment was the construction of a voltaic pile with seven ha'penny coins, stacked together with seven disks of sheet zinc, and six pieces of paper moistened with salt water.
With this pile he decomposed sulphate of magnesia (first letter to Abbott, 12 July 1812).
In 1821, soon after the Danish physicist and chemist Hans Christian Ørsted discovered the phenomenon of electromagnetism, Davy and British scientist William Hyde Wollaston tried, but failed, to design an electric motor.
Faraday, having discussed the problem with the two men, went on to build two devices to produce what he called "electromagnetic rotation".
One of these, now known as the homopolar motor, caused a continuous circular motion that was engendered by the circular magnetic force around a wire that extended into a pool of mercury wherein was placed a magnet; the wire would then rotate around the magnet if supplied with current from a chemical battery.
These experiments and inventions formed the foundation of modern electromagnetic technology.
In his excitement, Faraday published results without acknowledging his work with either Wollaston or Davy.
The resulting controversy within the Royal Society strained his mentor relationship with Davy and may well have contributed to Faraday’s assignment to other activities, which consequently prevented his involvement in electromagnetic research for several years.
From his initial discovery in 1821, Faraday continued his laboratory work, exploring electromagnetic properties of materials and developing requisite experience.
In 1824, Faraday briefly set up a circuit to study whether a magnetic field could regulate the flow of a current in an adjacent wire, but he found no such relationship.
This experiment followed similar work conducted with light and magnets three years earlier that yielded identical results.
During the next seven years, Faraday spent much of his time perfecting his recipe for optical quality (heavy) glass, borosilicate of lead, which he used in his future studies connecting light with magnetism.
In his spare time, Faraday continued publishing his experimental work on optics and electromagnetism; he conducted correspondence with scientists whom he had met on his journeys across Europe with Davy, and who were also working on electromagnetism.
Two years after the death of Davy, in 1831, he began his great series of experiments in which he discovered electromagnetic induction, recording in his laboratory diary on 28 October 1831 he was; "making many experiments with the great magnet of the Royal Society".
Faraday's breakthrough came when he wrapped two insulated coils of wire around an iron ring, and found that upon passing a current through one coil a momentary current was induced in the other coil.
This phenomenon is now known as mutual induction.
The iron ring-coil apparatus is still on display at the Royal Institution.
In subsequent experiments, he found that if he moved a magnet through a loop of wire an electric current flowed in that wire.
The current also flowed if the loop was moved over a stationary magnet.
His demonstrations established that a changing magnetic field produces an electric field; this relation was modelled mathematically by James Clerk Maxwell as Faraday's law, which subsequently became one of the four Maxwell equations, and which have in turn evolved into the generalization known today as field theory.
Faraday would later use the principles he had discovered to construct the electric dynamo, the ancestor of modern power generators and the electric motor.
In 1839, he completed a series of experiments aimed at investigating the fundamental nature of electricity; Faraday used "static", batteries, and "animal electricity" to produce the phenomena of electrostatic attraction, electrolysis, magnetism, etc.
He concluded that, contrary to the scientific opinion of the time, the divisions between the various "kinds" of electricity were illusory.
Faraday instead proposed that only a single "electricity" exists, and the changing values of quantity and intensity (current and voltage) would produce different groups of phenomena.
Near the end of his career, Faraday proposed that electromagnetic forces extended into the empty space around the conductor.
This idea was rejected by his fellow scientists, and Faraday did not live to see the eventual acceptance of his proposition by the scientific community.
Faraday's concept of lines of flux emanating from charged bodies and magnets provided a way to visualize electric and magnetic fields; that conceptual model was crucial for the successful development of the electromechanical devices that dominated engineering and industry for the remainder of the 19th century. 
Cell emf dependency on changes in concentration.
Nernst equation.
The standard potential of an electrochemical cell requires standard conditions (ΔG°) for all of the reactants.
When reactant concentrations differ from standard conditions, the cell potential will deviate from the standard potential.
In the 20th century German chemist Walther Nernst proposed a mathematical model to determine the effect of reactant concentration on electrochemical cell potential.
In the late 19th century, Josiah Willard Gibbs had formulated a theory to predict whether a chemical reaction is spontaneous based on the free energy ΔG = ΔG° + RT·ln(Q) Here "ΔG" is change in Gibbs free energy, "ΔG°" is the cell potential when "Q" is equal to 1, "T" is absolute temperature(Kelvin), "R" is the gas constant and "Q" is reaction quotient which can be found by dividing products by reactants using only those products and reactants that are aqueous or gaseous.
Gibbs' key contribution was to formalize the understanding of the effect of reactant concentration on spontaneity.
Based on Gibbs' work, Nernst extended the theory to include the contribution from electric potential on charged species.
As shown in the previous section, the change in Gibbs free energy for an electrochemical cell can be related to the cell potential.
Thus, Gibbs' theory becomes nFΔE = nFΔE° – RT ln(Q) Here "n" is the number of electrons/mole product, "F" is the Faraday constant (coulombs/mole), and "ΔE" is cell potential.
Finally, Nernst divided through by the amount of charge transferred to arrive at a new equation which now bears his name: ΔE = ΔE° – (RT/nF)ln(Q) Assuming standard conditions (T = 25 °C) and R = 8.3145 J/(K·mol), the equation above can be expressed on base—10 logarithm as shown below: formula_3