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))`

5.1 g of solid NH_(4)SH is introduced into a evacuated 3L flask at 600 K. 30% of the NH_(4)SH dissociated into NH_(3) and H_(2)S gases by the time equilibrium is reached. The K_(p) of the reaction at 600 K is (R = 0.082 L atm mol^(-1)K^(-1), N=14, S=32 )

For the reaction at 800 K N_(2)(g)+3H_(2)(g)hArr 2NH_(3)(g) the ratio of K_(p) and K_(c ) is : (R = 0.082 L atm mol^(-1)K^(-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?

What is the molar mass of a gas whose density is 1.5 g L^(-1) at 27^(@)C and 1 atm pressure ? (Use R = 0.08L atm mol^(-1) K^(-1) )

The Osmotic pressure of solution containing 4.0g of solute (molar mass 246) per litre at 27^@C is (R = 0.082L atm "k"^(-1) "mol"^(-1) )

A gas of molar mass 84.5 g//mol is enclosed in a flask at 27^@C has a pressure of 2 atm. Calculate the density of the gas. [R = 0.082 L atm K^(-1) mol^(-1)]