What is the unit of electrochemical equivalent?
2 Answers
The unit of electrochemical equivalent (ECE) is typically expressed in terms of mass per unit charge. It is commonly given in grams per coulomb (g/C). This value represents the mass of a substance that is deposited or dissolved during electrolysis per unit of electric charge passed through the electrolyte.
The unit of electrochemical equivalent (ECE) is typically expressed in terms of grams per coulomb (g/C). This unit reflects the mass of a substance that is deposited or dissolved by one coulomb of electric charge.
### Understanding Electrochemical Equivalent
1. **Definition**: Electrochemical equivalent (ECE) is the mass of a substance that is deposited or dissolved at an electrode during electrolysis when one coulomb of electric charge passes through the electrolyte. It is essentially a measure of how much substance is affected by a unit charge.
2. **Calculation**: The ECE of a substance can be determined using Faraday's laws of electrolysis. For a given substance, it is calculated using the formula:
\[
\text{ECE} = \frac{M}{nF}
\]
where:
- \( M \) is the molar mass of the substance.
- \( n \) is the number of electrons transferred per ion of the substance during the electrochemical reaction.
- \( F \) is Faraday's constant (approximately \( 96485 \) C/mol), which is the charge of one mole of electrons.
3. **Units**:
- **Grams per Coulomb (g/C)**: This is the most common unit, where 1 g/C means that 1 gram of the substance is deposited or dissolved by passing 1 coulomb of electric charge.
- **Kilograms per Coulomb (kg/C)**: Sometimes used in different contexts, but essentially the same idea scaled by a factor of 1000.
### Example
For instance, consider the electrochemical equivalent of silver (Ag), which has a molar mass of about 107.87 g/mol, and in its electrochemical reaction, 1 mole of Ag requires 1 mole of electrons. Using Faraday's constant:
\[
\text{ECE}_{\text{Ag}} = \frac{107.87 \, \text{g/mol}}{1 \times 96485 \, \text{C/mol}} \approx 1.12 \times 10^{-3} \, \text{g/C}
\]
So, the electrochemical equivalent of silver is approximately 0.00112 g/C.
In summary, the unit of electrochemical equivalent is grams per coulomb (g/C), representing the mass of a substance that is deposited or dissolved per unit of electric charge.
### Understanding Electrochemical Equivalent
1. **Definition**: Electrochemical equivalent (ECE) is the mass of a substance that is deposited or dissolved at an electrode during electrolysis when one coulomb of electric charge passes through the electrolyte. It is essentially a measure of how much substance is affected by a unit charge.
2. **Calculation**: The ECE of a substance can be determined using Faraday's laws of electrolysis. For a given substance, it is calculated using the formula:
\[
\text{ECE} = \frac{M}{nF}
\]
where:
- \( M \) is the molar mass of the substance.
- \( n \) is the number of electrons transferred per ion of the substance during the electrochemical reaction.
- \( F \) is Faraday's constant (approximately \( 96485 \) C/mol), which is the charge of one mole of electrons.
3. **Units**:
- **Grams per Coulomb (g/C)**: This is the most common unit, where 1 g/C means that 1 gram of the substance is deposited or dissolved by passing 1 coulomb of electric charge.
- **Kilograms per Coulomb (kg/C)**: Sometimes used in different contexts, but essentially the same idea scaled by a factor of 1000.
### Example
For instance, consider the electrochemical equivalent of silver (Ag), which has a molar mass of about 107.87 g/mol, and in its electrochemical reaction, 1 mole of Ag requires 1 mole of electrons. Using Faraday's constant:
\[
\text{ECE}_{\text{Ag}} = \frac{107.87 \, \text{g/mol}}{1 \times 96485 \, \text{C/mol}} \approx 1.12 \times 10^{-3} \, \text{g/C}
\]
So, the electrochemical equivalent of silver is approximately 0.00112 g/C.
In summary, the unit of electrochemical equivalent is grams per coulomb (g/C), representing the mass of a substance that is deposited or dissolved per unit of electric charge.