What is electrochemical equivalent class 12th chemistry?
2 Answers
In Class 12 Chemistry, the electrochemical equivalent (ECE) is a measure used to relate the amount of a substance that is deposited or dissolved at an electrode during electrolysis to the amount of electric charge passed through the electrolyte.
The electrochemical equivalent of a substance is defined as the mass of that substance deposited or dissolved by the passage of one coulomb of electric charge through an electrolyte. It’s given by the formula:
\[ \text{ECE} = \frac{M}{nF} \]
where:
- \( M \) is the molar mass of the substance,
- \( n \) is the number of electrons involved in the electrochemical reaction (valency),
- \( F \) is the Faraday constant (approximately \( 96500 \text{ C/mol} \)).
In simpler terms, the electrochemical equivalent tells you how much of a substance will be deposited or dissolved per unit charge. It helps in quantifying the efficiency of electrolysis processes and understanding the relationship between the electrical charge and chemical changes.
The electrochemical equivalent of a substance is defined as the mass of that substance deposited or dissolved by the passage of one coulomb of electric charge through an electrolyte. It’s given by the formula:
\[ \text{ECE} = \frac{M}{nF} \]
where:
- \( M \) is the molar mass of the substance,
- \( n \) is the number of electrons involved in the electrochemical reaction (valency),
- \( F \) is the Faraday constant (approximately \( 96500 \text{ C/mol} \)).
In simpler terms, the electrochemical equivalent tells you how much of a substance will be deposited or dissolved per unit charge. It helps in quantifying the efficiency of electrolysis processes and understanding the relationship between the electrical charge and chemical changes.
The term "electrochemical equivalent" is a concept in chemistry and electrochemistry, particularly relevant for students studying at the 12th-grade level. Here's a detailed explanation:
### Electrochemical Equivalent
**Definition:**
The electrochemical equivalent of a substance is the amount of that substance deposited or dissolved at an electrode during electrolysis when a unit charge (typically one coulomb) is passed through the electrolyte. It’s a way to quantify how much of a substance (usually in grams) is involved in an electrochemical reaction for a given amount of electric charge.
**Mathematical Expression:**
The electrochemical equivalent (\( E \)) can be expressed as:
\[ E = \frac{m}{Q} \]
where:
- \( m \) is the mass of the substance deposited or dissolved,
- \( Q \) is the total electric charge passed through the electrolyte.
**Units:**
The units of electrochemical equivalent are typically grams per coulomb (g/C).
### Calculation and Application
1. **Faraday’s Laws of Electrolysis:**
The electrochemical equivalent is closely related to Faraday's laws of electrolysis. According to Faraday's first law:
\[ m = \frac{Q}{F} \times E \]
where:
- \( m \) is the mass of the substance deposited,
- \( Q \) is the total charge,
- \( F \) is Faraday's constant (\( F \approx 96485 \) C/mol),
- \( E \) is the electrochemical equivalent.
2. **Determination:**
To determine the electrochemical equivalent of a substance, you can perform an electrolysis experiment where you measure the amount of substance deposited on the electrode for a known amount of electric charge. By dividing the mass of the substance by the charge, you get the electrochemical equivalent.
3. **Practical Example:**
If you have a substance like copper and you perform electrolysis, you might find that 0.63 grams of copper are deposited when 1 coulomb of charge is passed through the solution. Therefore, the electrochemical equivalent of copper is 0.63 g/C.
4. **Usefulness:**
The concept of electrochemical equivalent is important in industrial applications like electroplating and electrorefining. It helps in designing and controlling the amount of material deposited during these processes.
### Summary
In summary, the electrochemical equivalent of a substance is a measure of how much of that substance is deposited or dissolved per unit charge during electrolysis. It provides a way to relate the physical amount of substance involved in the electrochemical process to the electric charge passed through the system. This concept is foundational in understanding electrochemical reactions and is essential for practical applications in chemistry and industry.
### Electrochemical Equivalent
**Definition:**
The electrochemical equivalent of a substance is the amount of that substance deposited or dissolved at an electrode during electrolysis when a unit charge (typically one coulomb) is passed through the electrolyte. It’s a way to quantify how much of a substance (usually in grams) is involved in an electrochemical reaction for a given amount of electric charge.
**Mathematical Expression:**
The electrochemical equivalent (\( E \)) can be expressed as:
\[ E = \frac{m}{Q} \]
where:
- \( m \) is the mass of the substance deposited or dissolved,
- \( Q \) is the total electric charge passed through the electrolyte.
**Units:**
The units of electrochemical equivalent are typically grams per coulomb (g/C).
### Calculation and Application
1. **Faraday’s Laws of Electrolysis:**
The electrochemical equivalent is closely related to Faraday's laws of electrolysis. According to Faraday's first law:
\[ m = \frac{Q}{F} \times E \]
where:
- \( m \) is the mass of the substance deposited,
- \( Q \) is the total charge,
- \( F \) is Faraday's constant (\( F \approx 96485 \) C/mol),
- \( E \) is the electrochemical equivalent.
2. **Determination:**
To determine the electrochemical equivalent of a substance, you can perform an electrolysis experiment where you measure the amount of substance deposited on the electrode for a known amount of electric charge. By dividing the mass of the substance by the charge, you get the electrochemical equivalent.
3. **Practical Example:**
If you have a substance like copper and you perform electrolysis, you might find that 0.63 grams of copper are deposited when 1 coulomb of charge is passed through the solution. Therefore, the electrochemical equivalent of copper is 0.63 g/C.
4. **Usefulness:**
The concept of electrochemical equivalent is important in industrial applications like electroplating and electrorefining. It helps in designing and controlling the amount of material deposited during these processes.
### Summary
In summary, the electrochemical equivalent of a substance is a measure of how much of that substance is deposited or dissolved per unit charge during electrolysis. It provides a way to relate the physical amount of substance involved in the electrochemical process to the electric charge passed through the system. This concept is foundational in understanding electrochemical reactions and is essential for practical applications in chemistry and industry.