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 ?

Question

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 ?

Infinity Learn · Accepted Answer

$$CH4+2H2S$$→$$CS2+4H2$$                    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

Want to Fund your own JEE / NEET / Foundation preparation ??

Detailed Solution

Get Expert Academic Guidance – Connect with a Counselor Today!