A current of `1 A` is possed through a dilute solution of sulphuric acid for some time to liberate `1 g` of oxygen. How much hydrogen is liberated during this period? How long was the current passed? Faraday constant `= 96500 C mol^(-1)`.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Determine the chemical equivalent of oxygen and hydrogen.
- The atomic mass of oxygen (O) is 16 g/mol, and its valency is 2. Therefore, the chemical equivalent of oxygen (XO) is given by:
\[ XO = \frac{\text{Atomic mass of O}}{\text{Valency of O}} = \frac{16}{2} = 8 \text{ g/equiv} \]
- The atomic mass of hydrogen (H) is 1 g/mol, and its valency is 1. Therefore, the chemical equivalent of hydrogen (XH) is:
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