Ammonia under a pressure of $$15atm$$ at $$27oC$$ is heated to $$347oC$$ in a closed vessel in the presence of a catalyst. Under the conditions, $$NH3$$ is partially decomposed according to the equation, $$2NH3$$⇌$$N2+3H2$$ the vessel is such that the volume remains effectively constant where as pressure increases to $$50$$ atm. Calculate the percentage of $$NH3$$. actually decomposed :

Question

Ammonia under a pressure of $$15atm$$ at $$27oC$$ is heated to $$347oC$$ in a closed vessel in the presence of a catalyst. Under the conditions, $$NH3$$ is partially decomposed according to the equation, $$2NH3$$⇌$$N2+3H2$$ the vessel is such that the volume remains effectively constant where as pressure increases to $$50$$ atm. Calculate the percentage of $$NH3$$. actually decomposed :

Infinity Learn · Accepted Answer

$$NH3$$ ⇌ $$12N2$$ $$+$$ $$32H2$$   Total no. of moles Initially;   $$1mol$$        $$0$$          $$0$$              $$1$$   at equil.; $$1-x$$        $$x/2$$      $$3x/2$$        $$1+xFrom$$ ideal gas equation, $$PV=nRT$$ at constant V , $$nTP=constant$$   i.e. $$n1T1P1=n2T2P2$$ $$1$$×$$30015=(1+x)62050$$ $$x=0.613$$∴% of dissociation $$=$$ $$61.3$$%

Q.

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