A mixture of `2` moles of `CH_(4)` and `34 g` of `H_(2)S` was placed in an evacuated chamber, which was then heated to an maintained at `727^(@)C`. When equilibrium was established in the gaseous phase reaction: `CH_(4)+2H_(2)ShArrCS_(2)+4H_(2)`, the total pressure in the container was `0.92 atm` and the partial pressure of hydrogen was `0.2 atm`. Calculate the volume of container.

A mixture of `2` moles of `CH_(4)` and `34 g` of `H_(2)S` was placed i

1.	A mixture of `2` moles of `CH_(4)` and `34 g` of `H_(2)S` was placed in an evacuated chamber, which was then heated to an maintained at `727^(@)C`. When equilibrium was established in the gaseous phase reaction: `CH_(4)+2H_(2)ShArrCS_(2)+4H_(2)`, the total pressure in the container was `0.92 atm` and the partial pressure of hydrogen was `0.2 atm`. Calculate the volume of container.
Answer» Correct Answer - `300.38 litre` ,

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