5.1 g `NH_(4)SH` is introduced in 3.0 L evacuated flask at `327^(@)C`, 30% of the solid `NH_(4)SH` decomposed to `NH_(3)` and `H_(2)S` as gases. The `K_(p)` of the reaction at `327^(@)C` is : `(R = 0.082 L atm mol^(-1)K^(-1), "Molar mass of S =" 32 g mol^(-1) , "molar mass of N" = 14 g mol^(-1))`
When 5.1 g of solid \(NH_{4}\) HS is introduced into a two litre evacuated flask at 27^@C , 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K_p for the reaction at 27^@C is "x" xx 10^(-2) . The value of x is ______ (Integer answer) [Given R = 0.082 L atm K^(-1)" mol"^(-1) ]
When 3.06 g of solid NH_(4)HS is intoduced into a 2-L evacuated flask at 27^(@)C, 30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. a. Calculate K_(c) and K_(p) for the reaction at 27^(@)C . b. What would happen to the equilibrium when more solid NH_(4)HS is introduced into the flask?
When 3.06 g of solid NH_(4)HS is introduced into a two-litre evacuated flask at 27^(@)C, 30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. (i) Calculate K_(c ) and K_(p) for the reaction at 27^(@)C . (ii) What would happen to the equilibrium when more solid NH_(4)HS is introduced into the flask?
1.7g of NH_3(g) is present in a 2-L flask. The active mass of NH_3(g) is
The osmotic pressure of solution containing 34.2 g of cane sugar (molar mass = 342 g mol^(-1) ) in 1 L of solution at 20^(@)C is (Given R = 0.082 L atm K^(-1) mol^(-1) )
5.1g of solid NH_(4)HS is introduced in a 16.4 lit. vessel & heated upto 500 K K_(B) for equilibrium NH_(4)HS(s) hArr NH_(3)(g)+H_(2)S(g) is 0.16 . The maximum pressure developed in the vessel will be :
Calculate the pressure of 154 g carbon dioxide in a vessel of 2.0 L capacity at 30^(@)C , a = 648 L bar atm K^(-1) mol^(-1), b = 0.0427 L mol^(-1)
