The electric charge required for electrode deposition of one gram-equivalent of a substance is :

Options

A. (a) one ampere per second
B. (b) 96500 coulombs per second
C. (c) one ampere for one hour
D. (d) charge on one mole of electrons

Answer

To determine the electric charge required for the electrode deposition of one gram-equivalent of a substance, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Gram-Equivalent**:
- One gram-equivalent of a substance is defined as the amount of the substance that will combine with or displace one mole of hydrogen ions (H⁺) or one mole of electrons in a redox reaction.

2. **Faraday's Law of Electrolysis**:
- According to Faraday's law, the quantity of electricity (Q) required to deposit or liberate a substance during electrolysis is directly proportional to the amount of substance involved in the reaction. The relationship can be expressed as:
\[ Q = n \cdot F \]
where \( n \) is the number of equivalents and \( F \) is Faraday's constant (approximately 96500 coulombs).

3. **Charge for One Gram-Equivalent**:
- For one gram-equivalent of a substance, \( n = 1 \). Therefore, the charge required is:
\[ Q = 1 \cdot F = F \approx 96500 \text{ coulombs} \]

4. **Conclusion**:
- Thus, the electric charge required for the electrode deposition of one gram-equivalent of a substance is approximately 96500 coulombs.

5. **Identifying the Correct Option**:
- Among the given options, the one that matches our calculation is "96500 coulombs".

### Final Answer:
The electric charge required for electrode deposition of one gram-equivalent of a substance is **96500 coulombs**.

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