The quantity of electricity needed to liberate 0.5 gram equivalent of an element, during electrolysis is

Options

A. 48250 Faraday
B. 96500 Faraday
C. 48250 Coulomb
D. 193000 Coulomb.

Answer

To solve the problem of determining the quantity of electricity needed to liberate 0.5 gram equivalent of an element during electrolysis, we can follow these steps:

### Step 1: Understand the relationship between Faraday and gram equivalent
- One Faraday of electricity is required to liberate one gram equivalent of an element during electrolysis.

### Step 2: Know the value of one Faraday
- One Faraday is equivalent to 96,500 coulombs.

### Step 3: Calculate the quantity of electricity for 0.5 gram equivalent
- Since one Faraday (96,500 coulombs) is needed for one gram equivalent, for 0.5 gram equivalent, we need half of that amount.

\[ \text{Quantity of electricity} = 0.5 \times 96,500 \text{ coulombs} \]

### Step 4: Perform the calculation
- Now, calculating the above expression:

\[ \text{Quantity of electricity} = 0.5 \times 96,500 = 48,250 \text{ coulombs} \]

### Final Answer
- Therefore, the quantity of electricity needed to liberate 0.5 gram equivalent of an element during electrolysis is **48,250 coulombs**.

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