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 × 10 - 2 . The value of x is (Integer answer) [Given 1 R = 0 . 082 L atm K - 1 mol - 1

Step-by-step solution

Moles of NH 4 HS initially taken = 5 . 1   g 51   g / mol = 0 . 1   mol volume of vessel = 2   L NH 4 HS ( s ) ⇌ NH 3 (   g ) + H 2 S ( g ) t = 0    0 . 1   mol t = ∞ 0 . 1 ( 1 - 0 . 2 ) 0 . 1 × 0 . 2 0 . 1 × 0 . 2 Partial pressure of each gaseous component P = n R T V = 0 . 1 × 0 . 2 × 0 . 082 × 300 2 = 0 . 246   atm ⇒ k P = P NH 3 × P H 2   S = ( 0 . 246 ) 2 = 0 . 060516 = 6 . 05 × 10 - 2 ⇒ 6