What will be the strength of 50ml `K_(2)Cr_(2)O_(7)` that completely reacts with 11.2 litre of `H_(2)S` oxidizing it into sulphur?

Explanation

To determine the strength of 50 ml of \( K_2Cr_2O_7 \) that completely reacts with 11.2 liters of \( H_2S \), we will follow these steps:

### Step 1: Determine the moles of \( H_2S \)

Given that the volume of \( H_2S \) is 11.2 liters, we can find the number of moles using the ideal gas law at standard temperature and pressure (STP), where 1 mole of gas occupies 22.4 liters.

\[
\text{Moles of } H_2S = \frac{\text{Volume of } H_2S}{\text{Molar volume at STP}} = \frac{11.2 \, \text{L}}{22.4 \, \text{L/mol}} = 0.5 \, \text{moles}
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