Laws of Electrolysis — Core Principles

Core Principles

Faraday's Laws of Electrolysis provide a quantitative framework for understanding the chemical changes driven by electricity. The First Law states that the mass ($m$) of a substance deposited or liberated at an electrode is directly proportional to the total quantity of electricity ($Q$) passed through the electrolyte ($m propto Q$).

Since $Q = I \times t$, this can be written as $m = ZIt$, where $Z$ is the electrochemical equivalent (mass deposited per Coulomb). The Second Law applies when the same quantity of electricity is passed through different electrolytes connected in series.

It states that the masses of substances deposited ($m_1, m_2$) are directly proportional to their chemical equivalent weights ($E_1, E_2$), i.e., $m_1/m_2 = E_1/E_2$. This implies that $Z = E/F$, where $F$ is the Faraday constant ($96500,\text{C/mol}$).

Combining these, the general formula for mass deposited is $m = (E/F)It$. These laws are crucial for industrial applications like electroplating and metal refining, and for solving numerical problems in NEET.

Important Differences

vs Faraday's Second Law of Electrolysis

Aspect	This Topic	Faraday's Second Law of Electrolysis
Scope	Relates mass deposited to the quantity of electricity passed through a *single* electrolyte.	Relates masses deposited of *different* substances when the *same* quantity of electricity is passed through them (e.g., in series).
Mathematical Expression	$m = ZIt$ or $m = (E/F)It$	$m_1/m_2 = E_1/E_2$
Key Proportionality	Mass deposited is directly proportional to charge ($m propto Q$).	Masses deposited are directly proportional to their equivalent weights ($m propto E$). This also implies $Z propto E$ or $Z = E/F$.
Variables Involved	Mass ($m$), Electrochemical Equivalent ($Z$), Current ($I$), Time ($t$), Charge ($Q$).	Masses of substances ($m_1, m_2$), Equivalent weights of substances ($E_1, E_2$). Implicitly, the same charge ($Q$) is passed.
Primary Application	Calculating the amount of substance deposited for a given current and time in a single cell.	Comparing the amounts of different substances deposited by the same amount of electricity, often used in series cell problems.

Faraday's First Law focuses on the direct relationship between the total electrical charge passed and the mass of a single substance deposited or liberated. It quantifies the extent of reaction in a single electrolytic cell. In contrast, Faraday's Second Law extends this concept to compare the relative amounts of different substances deposited when an identical quantity of electricity flows through multiple electrolytic cells connected in series. It highlights that the deposition is proportional to the chemical equivalent weight, establishing a universal constant (Faraday constant) that links charge to the equivalent amount of any substance. Both laws are fundamental but address different aspects of quantitative electrolysis.