The quantity of electricity required to librate 0.1 g equivalent of an element at the electrode is

Options

A. 9650 C
B. 96500 C
C. 965 C
D. 96.5 C

Explanation

To solve the problem of determining the quantity of electricity required to liberate 0.1 g equivalent of an element at the electrode, we can use Faraday's laws of electrolysis. Let's break down the steps:

### Step-by-Step Solution:

1. **Understand the Concept**: According to Faraday's first law of electrolysis, the quantity of electricity (Q) required to liberate a certain amount of substance at an electrode is directly proportional to the amount of substance liberated. The relationship can be expressed as:
\[ Q = n \times F \]
where \( n \) is the number of equivalents of the substance and \( F \) is Faraday's constant (approximately 96500 C/mol).

2. **Identify the Given Data**:
- We are given that the equivalent mass of the element is 0.1 g equivalent.

3. **Calculate the Quantity of Electricity**:
- Since we know that 1 equivalent of an element corresponds to a charge of 96500 C, we can calculate the charge required for 0.1 g equivalent:
\[ Q = \text{equivalent} \times F \]
- Substituting the values:
\[ Q = 0.1 \, \text{g equivalent} \times 96500 \, \text{C/g equivalent} \]
\[ Q = 0.1 \times 96500 = 9650 \, \text{C} \]

4. **Final Answer**: The quantity of electricity required to liberate 0.1 g equivalent of the element at the electrode is **9650 C**.

### Summary of the Solution:
The quantity of electricity required is calculated using the formula \( Q = n \times F \), where \( n \) is the amount in equivalents and \( F \) is Faraday's constant. For 0.1 g equivalent, the quantity of electricity required is 9650 C.