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A mixture of 2 moles of CH4 and 34 g of H2S was placed in an evacuated container, which was then heated to & maintained at 7270C. When equilibrium is established as the gaseous reaction CH4+2H2S⥂CS2+4H2 , the total pressure in the container was 0.92 atm and the partial pressure of hydrogen was 0.2 atm. What was the volume of container ?

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a

25 L

b

300 L

c

200 L

d

10 L

answer is B.

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Detailed Solution

CH4+2H2S→CS2+4H2 Total moles = 3+2x Initial 2 1 0 0 given PH2=0.2=4x3+2x×0.92 moler At equilibrium 2-x 1-2x x 4x ∴ x = 0.183Total moles in flask = 3+2x = 3.366V=nRTP=299.84 L

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A mixture of 2 moles of CH4 and 34 g of H2S was placed in an evacuated container, which was then heated to & maintained at 7270C. When equilibrium is established as the gaseous reaction CH4+2H2S⥂CS2+4H2 , the total pressure in the container was 0.92 atm and the partial pressure of hydrogen was 0.2 atm. What was the volume of container ?