What is electrochemical equivalent Faraday?
2 Answers
The term "electrochemical equivalent" is often discussed in the context of electrolysis and Faraday's laws of electrolysis. The "Faraday constant" is related to it, and understanding it requires a bit of background in electrochemistry.
### Electrochemical Equivalent
The electrochemical equivalent of a substance is a measure of how much of that substance is deposited or dissolved during electrolysis per unit charge (usually per coulomb). It provides a way to relate the amount of chemical change to the amount of electric charge used.
**Definition:**
- The electrochemical equivalent (E) of a substance is the mass of the substance deposited or dissolved at an electrode when one coulomb of electric charge passes through the electrolyte.
**Formula:**
\[ E = \frac{m}{Q} \]
where:
- \( m \) = mass of the substance deposited or dissolved (in grams)
- \( Q \) = total electric charge passed (in coulombs)
### Faraday's Laws of Electrolysis
Faraday's laws provide a quantitative basis for electrochemical equivalence:
1. **First Law:** The amount of chemical change produced by an electric current is directly proportional to the quantity of charge passed through the electrolyte.
\[ m = Z \cdot Q \]
where:
- \( m \) = mass of the substance deposited or dissolved
- \( Z \) = electrochemical equivalent
- \( Q \) = total electric charge passed
2. **Second Law:** The amount of different substances altered by the same quantity of electricity are proportional to their equivalent weights.
### Faraday Constant
The Faraday constant (\( F \)) is a fundamental physical constant that represents the charge of one mole of electrons. It is approximately:
\[ F \approx 96485 \, \text{C/mol} \]
### Relation to Electrochemical Equivalent
The electrochemical equivalent can be calculated using the Faraday constant and the equivalent weight of the substance. The equivalent weight (E.W.) of a substance is the mass that reacts with or displaces one mole of hydrogen ions (or one mole of electrons):
\[ E = \frac{\text{Equivalent Weight}}{F} \]
In summary, the electrochemical equivalent gives a direct way to relate the amount of substance altered by electrolysis to the amount of electric charge used, while the Faraday constant provides a fundamental link between electric charge and the amount of substance.
### Electrochemical Equivalent
The electrochemical equivalent of a substance is a measure of how much of that substance is deposited or dissolved during electrolysis per unit charge (usually per coulomb). It provides a way to relate the amount of chemical change to the amount of electric charge used.
**Definition:**
- The electrochemical equivalent (E) of a substance is the mass of the substance deposited or dissolved at an electrode when one coulomb of electric charge passes through the electrolyte.
**Formula:**
\[ E = \frac{m}{Q} \]
where:
- \( m \) = mass of the substance deposited or dissolved (in grams)
- \( Q \) = total electric charge passed (in coulombs)
### Faraday's Laws of Electrolysis
Faraday's laws provide a quantitative basis for electrochemical equivalence:
1. **First Law:** The amount of chemical change produced by an electric current is directly proportional to the quantity of charge passed through the electrolyte.
\[ m = Z \cdot Q \]
where:
- \( m \) = mass of the substance deposited or dissolved
- \( Z \) = electrochemical equivalent
- \( Q \) = total electric charge passed
2. **Second Law:** The amount of different substances altered by the same quantity of electricity are proportional to their equivalent weights.
### Faraday Constant
The Faraday constant (\( F \)) is a fundamental physical constant that represents the charge of one mole of electrons. It is approximately:
\[ F \approx 96485 \, \text{C/mol} \]
### Relation to Electrochemical Equivalent
The electrochemical equivalent can be calculated using the Faraday constant and the equivalent weight of the substance. The equivalent weight (E.W.) of a substance is the mass that reacts with or displaces one mole of hydrogen ions (or one mole of electrons):
\[ E = \frac{\text{Equivalent Weight}}{F} \]
In summary, the electrochemical equivalent gives a direct way to relate the amount of substance altered by electrolysis to the amount of electric charge used, while the Faraday constant provides a fundamental link between electric charge and the amount of substance.
The term "electrochemical equivalent" refers to a measure used in electrochemistry to quantify the amount of a substance that is deposited or dissolved at an electrode during electrolysis for a given amount of electric charge. It is closely related to Faraday's laws of electrolysis, which describe how the amount of substance transformed during electrolysis is proportional to the electric charge passed through the cell.
Let's break it down:
### 1. **Faraday's Laws of Electrolysis:**
- **First Law:** The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electric charge passed through the cell.
- **Second Law:** The mass of different substances altered at an electrode by the same quantity of electric charge is proportional to their equivalent weights.
### 2. **Electrochemical Equivalent (E):**
The electrochemical equivalent of a substance is a way of quantifying these transformations. It represents the amount of a substance (in grams) that is deposited or dissolved when one coulomb (C) of electric charge is passed through an electrolytic cell.
Mathematically, it can be expressed as:
\[ E = \frac{M}{n \cdot F} \]
where:
- \( E \) is the electrochemical equivalent (in grams per coulomb),
- \( M \) is the molar mass of the substance (in grams per mole),
- \( n \) is the number of electrons required to deposit or dissolve one mole of the substance (valency or oxidation state),
- \( F \) is Faraday's constant (approximately 96485 coulombs per mole).
### 3. **Faraday’s Constant (F):**
Faraday’s constant (\( F \)) represents the charge of one mole of electrons. Its value is approximately 96485 coulombs per mole. It is crucial in electrochemistry because it allows for the conversion between charge and the amount of substance in reactions.
### 4. **Practical Use:**
In practical applications, knowing the electrochemical equivalent of a substance helps in calculating how much of a substance will be deposited or dissolved during electrolysis. This is particularly useful in industries that rely on electroplating, electrorefining, and other electrochemical processes.
### Example:
For instance, if you want to electroplate silver onto a surface, you need to know how much silver will be deposited for a given amount of electrical current and time. By using the electrochemical equivalent of silver, you can calculate the exact amount of silver that will be deposited for a specified amount of electric charge.
In summary, the electrochemical equivalent is a key concept in electrochemistry that helps translate electrical charge into physical amounts of materials processed during electrolysis. It is a practical tool for designing and controlling electrochemical processes.
Let's break it down:
### 1. **Faraday's Laws of Electrolysis:**
- **First Law:** The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electric charge passed through the cell.
- **Second Law:** The mass of different substances altered at an electrode by the same quantity of electric charge is proportional to their equivalent weights.
### 2. **Electrochemical Equivalent (E):**
The electrochemical equivalent of a substance is a way of quantifying these transformations. It represents the amount of a substance (in grams) that is deposited or dissolved when one coulomb (C) of electric charge is passed through an electrolytic cell.
Mathematically, it can be expressed as:
\[ E = \frac{M}{n \cdot F} \]
where:
- \( E \) is the electrochemical equivalent (in grams per coulomb),
- \( M \) is the molar mass of the substance (in grams per mole),
- \( n \) is the number of electrons required to deposit or dissolve one mole of the substance (valency or oxidation state),
- \( F \) is Faraday's constant (approximately 96485 coulombs per mole).
### 3. **Faraday’s Constant (F):**
Faraday’s constant (\( F \)) represents the charge of one mole of electrons. Its value is approximately 96485 coulombs per mole. It is crucial in electrochemistry because it allows for the conversion between charge and the amount of substance in reactions.
### 4. **Practical Use:**
In practical applications, knowing the electrochemical equivalent of a substance helps in calculating how much of a substance will be deposited or dissolved during electrolysis. This is particularly useful in industries that rely on electroplating, electrorefining, and other electrochemical processes.
### Example:
For instance, if you want to electroplate silver onto a surface, you need to know how much silver will be deposited for a given amount of electrical current and time. By using the electrochemical equivalent of silver, you can calculate the exact amount of silver that will be deposited for a specified amount of electric charge.
In summary, the electrochemical equivalent is a key concept in electrochemistry that helps translate electrical charge into physical amounts of materials processed during electrolysis. It is a practical tool for designing and controlling electrochemical processes.