A definite amount of solid ${\rm{N}}{{\rm{H}}_4}{\rm{HS}}$ is placed in a flask already containing ${\rm{N}}{{\rm{H}}_3}$ gas at certain temperature and $0.50\;{\rm{ }}atm$ pressure. ${\rm{N}}{{\rm{H}}_4}{\rm{HS}}$ decomposes to give ${\rm{N}}{{\rm{H}}_3}$ and ${{\rm{H}}_2}{\rm{S}}$ and total equilibrium pressure in flask is $0.84\;{\rm{ }}atm$. The equilibrium constant for the reaction is :Failed to load question data. Please try again later.
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