A flask of 1.5 L capacity contains 400 mg of `O_(2)` and 60 mg of `H_(2)` at `100^(@)C`. Calculate the total pressure of the gaseous mixture. If the mixture is permitted to react to form water vapour at `100^(@)C`, what materials will be left and what will be their partial pressures?

Explanation

To solve the problem step by step, we will follow these calculations:

### Step 1: Convert Masses to Grams
Given:
- Mass of \( O_2 = 400 \, \text{mg} = 400 \times 10^{-3} \, \text{g} = 0.4 \, \text{g} \)
- Mass of \( H_2 = 60 \, \text{mg} = 60 \times 10^{-3} \, \text{g} = 0.06 \, \text{g} \)

### Step 2: Calculate Moles of Each Gas
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