What is the electrochemical equivalent of cl2?
2 Answers
The electrochemical equivalent (ECE) of a substance is a measure of how much of that substance is deposited or liberated at an electrode during electrolysis for a given amount of electric charge. It's typically expressed in grams per coulomb (g/C) or in other units like milligrams per coulomb (mg/C).
For chlorine gas (Cl₂), the electrochemical equivalent refers to the amount of chlorine gas evolved at an electrode during electrolysis. Chlorine gas is produced at the anode during the electrolysis of chloride solutions.
To determine the electrochemical equivalent of Cl₂, you need to know the molar mass of chlorine gas and the number of electrons involved in its formation.
1. **Molar Mass of Chlorine Gas (Cl₂):**
- Chlorine gas (Cl₂) has a molecular weight of about 70.9 g/mol (each Cl atom has an atomic weight of about 35.45 g/mol).
2. **Electrochemical Reaction:**
- The formation of Cl₂ gas from chloride ions (Cl⁻) at the anode during electrolysis can be represented by the reaction:
\[ 2 \text{Cl}^- (aq) \rightarrow \text{Cl}_2 (g) + 2 \text{e}^- \]
- This shows that 2 moles of chloride ions are needed to produce 1 mole of Cl₂ gas, which involves the transfer of 2 moles of electrons.
3. **Faraday’s Constant:**
- Faraday's constant (F) is approximately 96485 C/mol, which is the charge of 1 mole of electrons.
4. **Calculation of Electrochemical Equivalent (ECE):**
- The electrochemical equivalent can be calculated using the formula:
\[
\text{ECE} = \frac{\text{Molar Mass of Cl}_2}{\text{n} \times \text{Faraday's Constant}}
\]
where \( n \) is the number of electrons involved in the reaction.
- For Cl₂, \( n = 2 \) (since 2 electrons are involved per Cl₂ molecule).
- Thus:
\[
\text{ECE of Cl}_2 = \frac{70.9 \text{ g/mol}}{2 \times 96485 \text{ C/mol}}
\]
- Performing the calculation:
\[
\text{ECE of Cl}_2 \approx \frac{70.9}{192970} \approx 0.000368 \text{ g/C}
\]
So, the electrochemical equivalent of chlorine gas (Cl₂) is approximately \(0.000368\) grams per coulomb.
For chlorine gas (Cl₂), the electrochemical equivalent refers to the amount of chlorine gas evolved at an electrode during electrolysis. Chlorine gas is produced at the anode during the electrolysis of chloride solutions.
To determine the electrochemical equivalent of Cl₂, you need to know the molar mass of chlorine gas and the number of electrons involved in its formation.
1. **Molar Mass of Chlorine Gas (Cl₂):**
- Chlorine gas (Cl₂) has a molecular weight of about 70.9 g/mol (each Cl atom has an atomic weight of about 35.45 g/mol).
2. **Electrochemical Reaction:**
- The formation of Cl₂ gas from chloride ions (Cl⁻) at the anode during electrolysis can be represented by the reaction:
\[ 2 \text{Cl}^- (aq) \rightarrow \text{Cl}_2 (g) + 2 \text{e}^- \]
- This shows that 2 moles of chloride ions are needed to produce 1 mole of Cl₂ gas, which involves the transfer of 2 moles of electrons.
3. **Faraday’s Constant:**
- Faraday's constant (F) is approximately 96485 C/mol, which is the charge of 1 mole of electrons.
4. **Calculation of Electrochemical Equivalent (ECE):**
- The electrochemical equivalent can be calculated using the formula:
\[
\text{ECE} = \frac{\text{Molar Mass of Cl}_2}{\text{n} \times \text{Faraday's Constant}}
\]
where \( n \) is the number of electrons involved in the reaction.
- For Cl₂, \( n = 2 \) (since 2 electrons are involved per Cl₂ molecule).
- Thus:
\[
\text{ECE of Cl}_2 = \frac{70.9 \text{ g/mol}}{2 \times 96485 \text{ C/mol}}
\]
- Performing the calculation:
\[
\text{ECE of Cl}_2 \approx \frac{70.9}{192970} \approx 0.000368 \text{ g/C}
\]
So, the electrochemical equivalent of chlorine gas (Cl₂) is approximately \(0.000368\) grams per coulomb.
The electrochemical equivalent (ECE) of a substance is a measure of how much of that substance is produced or consumed during an electrochemical reaction per unit of electric charge passed. It’s often used in electrolysis calculations.
For chlorine gas (Cl₂), the electrochemical equivalent can be calculated based on its molecular weight and the charge needed to produce it during electrolysis.
**Here's a step-by-step breakdown of how to calculate it:**
1. **Determine the molecular weight of Cl₂:**
- Chlorine has an atomic weight of approximately 35.5 g/mol.
- Therefore, Cl₂ (which consists of two chlorine atoms) has a molecular weight of \( 35.5 \times 2 = 71 \) g/mol.
2. **Find the number of electrons required for the electrochemical process:**
- Chlorine gas is typically produced through the electrolysis of sodium chloride (NaCl) solution. In this process, Cl₂ is formed from chloride ions (Cl⁻).
- The reaction is: \( 2 \text{Cl}^- \rightarrow \text{Cl}_2 + 2 \text{e}^- \).
- Therefore, 2 moles of electrons are needed to produce 1 mole of Cl₂.
3. **Calculate the charge needed:**
- Faraday’s constant (F) is approximately 96485 C/mol, representing the charge per mole of electrons.
- Therefore, to produce 1 mole of Cl₂, 2 moles of electrons are needed, which equals \( 2 \times 96485 = 192970 \) C.
4. **Compute the electrochemical equivalent:**
- The ECE can be found using the formula:
\[
\text{ECE} = \frac{\text{Molecular weight}}{\text{Total charge needed per mole of substance}}
\]
- Substituting the values:
\[
\text{ECE} = \frac{71 \text{ g/mol}}{192970 \text{ C}}
\]
- This simplifies to approximately \( 3.69 \times 10^{-4} \text{ g/C} \).
Therefore, the electrochemical equivalent of Cl₂ is approximately \( 3.69 \times 10^{-4} \text{ g/C} \), meaning that for every coulomb of charge passed through the system, about \( 3.69 \times 10^{-4} \) grams of chlorine gas are produced.
For chlorine gas (Cl₂), the electrochemical equivalent can be calculated based on its molecular weight and the charge needed to produce it during electrolysis.
**Here's a step-by-step breakdown of how to calculate it:**
1. **Determine the molecular weight of Cl₂:**
- Chlorine has an atomic weight of approximately 35.5 g/mol.
- Therefore, Cl₂ (which consists of two chlorine atoms) has a molecular weight of \( 35.5 \times 2 = 71 \) g/mol.
2. **Find the number of electrons required for the electrochemical process:**
- Chlorine gas is typically produced through the electrolysis of sodium chloride (NaCl) solution. In this process, Cl₂ is formed from chloride ions (Cl⁻).
- The reaction is: \( 2 \text{Cl}^- \rightarrow \text{Cl}_2 + 2 \text{e}^- \).
- Therefore, 2 moles of electrons are needed to produce 1 mole of Cl₂.
3. **Calculate the charge needed:**
- Faraday’s constant (F) is approximately 96485 C/mol, representing the charge per mole of electrons.
- Therefore, to produce 1 mole of Cl₂, 2 moles of electrons are needed, which equals \( 2 \times 96485 = 192970 \) C.
4. **Compute the electrochemical equivalent:**
- The ECE can be found using the formula:
\[
\text{ECE} = \frac{\text{Molecular weight}}{\text{Total charge needed per mole of substance}}
\]
- Substituting the values:
\[
\text{ECE} = \frac{71 \text{ g/mol}}{192970 \text{ C}}
\]
- This simplifies to approximately \( 3.69 \times 10^{-4} \text{ g/C} \).
Therefore, the electrochemical equivalent of Cl₂ is approximately \( 3.69 \times 10^{-4} \text{ g/C} \), meaning that for every coulomb of charge passed through the system, about \( 3.69 \times 10^{-4} \) grams of chlorine gas are produced.