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What is the value for electrochemical equivalents?

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Best answer
The electrochemical equivalent (ECE) is a measure used in electrochemistry to quantify the amount of a substance that is deposited or dissolved during an electrochemical process. It is defined as the amount of a substance (usually in grams) that is deposited or dissolved by the passage of one coulomb of electric charge.

The electrochemical equivalent \( E \) can be calculated using the following formula:

\[ E = \frac{M}{nF} \]

Where:
- \( M \) is the molar mass of the substance (in grams per mole).
- \( n \) is the number of moles of electrons required to deposit or dissolve one mole of the substance.
- \( F \) is the Faraday constant, which is approximately \( 96,485 \text{ C/mol} \) (coulombs per mole).

For common elements and ions, the electrochemical equivalents are:

- **Copper (Cu)**: Approximately \( 0.000329 \text{ g/C} \) or \( 329 \text{ mg/C} \)
- **Zinc (Zn)**: Approximately \( 0.000318 \text{ g/C} \) or \( 318 \text{ mg/C} \)
- **Silver (Ag)**: Approximately \( 0.000001118 \text{ g/C} \) or \( 1.118 \text{ mg/C} \)

These values are specific to the elements and their common oxidation states in electrolytic processes. For other substances, you would need to calculate the electrochemical equivalent using the provided formula based on the molar mass, number of electrons involved in the reaction, and the Faraday constant.
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Electrochemical equivalents are constants used in electrolysis calculations. They are essentially the amount of substance (in grams) that will be deposited or dissolved by the electrochemical equivalent of a given current over a certain period of time. The value for electrochemical equivalents depends on the substance being considered.

Here's how you can calculate it for different substances:

1. **For Metals**: The electrochemical equivalent (E) can be calculated using the formula:
   \[
   E = \frac{M}{n \cdot F}
   \]
   where:
   - \( M \) is the molar mass of the metal (in grams per mole),
   - \( n \) is the number of electrons involved in the electrochemical reaction,
   - \( F \) is Faraday’s constant (approximately \( 96485 \, \text{C/mol} \)).

2. **For Water Electrolysis**: The electrochemical equivalent for water electrolysis is commonly used and is approximately:
   - For the production of hydrogen: \( 0.000091 \, \text{g/C} \) (grams per Coulomb),
   - For the production of oxygen: \( 0.000091 \, \text{g/C} \) (grams per Coulomb), given the reactions involved.

### Examples:

- **Copper (Cu)**: The molar mass of copper is \( 63.55 \, \text{g/mol} \), and it typically involves 2 electrons for deposition (Cu²⁺ + 2e⁻ → Cu). Thus, the electrochemical equivalent of copper is:
  \[
  E = \frac{63.55}{2 \cdot 96485} \approx 0.000658 \, \text{g/C}
  \]

- **Zinc (Zn)**: The molar mass of zinc is \( 65.38 \, \text{g/mol} \), and it involves 2 electrons for deposition (Zn²⁺ + 2e⁻ → Zn). Thus, the electrochemical equivalent of zinc is:
  \[
  E = \frac{65.38}{2 \cdot 96485} \approx 0.000678 \, \text{g/C}
  \]

These values are crucial in electroplating, electrolysis, and other electrochemical processes.
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