102 g of solid NH_(4)HS is taken in the 2L evacuated flask at 57^(@). Following two equilibrium exist simultaneously NH_(4)(s)iffNH_(3)(g)+H_(2)S(g) NH_(3)(g)iff(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) one mole of the solid decomposes to maintain both the equilibrium and 0.75 mol e of H_(2) was found at the equilibrium then find the equilibrium concentration of all the species and K_(C) for the both the reaction.

102 g of solid NH_(4)HS is taken in the 2L evacuated flask at 57^(@).

1.	102 g of solid NH_(4)HS is taken in the 2L evacuated flask at 57^(@). Following two equilibrium exist simultaneously NH_(4)(s)iffNH_(3)(g)+H_(2)S(g) NH_(3)(g)iff(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) one mole of the solid decomposes to maintain both the equilibrium and 0.75 mol e of H_(2) was found at the equilibrium then find the equilibrium concentration of all the species and K_(C) for the both the reaction.
Answer» Solution :Moles of `NH_(4)HS=(102)/(51)=2` `NH_(4)(s)iffNH_(3)(g)+H_(2)S(g)` `{:(2,0,0),(1,1-x,1):}` `NH_(3)(g)IFF(1)/(2)N_(2)(g)+(3)/(2)H_(2)(g) K_(C_(2))` `1-x (x)/(2) (3x)/(2)` Given that moles of `H_(2)=(3x)/(2)=0.75 iff x=(1)/(2)` `K_(C_(2))=1/2 ((1-x))/(2)=1/8` [SINCE `V=2L`] `K_(C_(2))=(((3x)/(4))^(3//2)((x)/(4))^(1//2))/(((1-x)/(2)))=(((3)/(8))^(3//2)((1)/(8))^(1//2))/(1/4)=(3)^(3//2)1/64xx4/1=(3)^(3//2)/(16)`