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 find 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: Write the balanced chemical equation
The balanced chemical equation for the reaction between \( K_2Cr_2O_7 \) and \( H_2S \) is:
\[ K_2Cr_2O_7 + 3H_2S \rightarrow K_2SO_4 + Cr_2(SO_4)_3 + 3S + 7H_2O \]
This indicates that 1 mole of \( K_2Cr_2O_7 \) reacts with 3 moles of \( H_2S \).
...