[" When "306g" of solid "NH_(4)HS" introduced into a two-litre evacuated flask "],[" the solid decomposes into gaseous ammonia and hydrogen sulphide."],[" (i) Calculate "K_(C)" and "K_(p)" for the reaction at "27C" ,"],[" (ii) What would happen to the equilibrium when more solid "NH_(4)" .HS intrate,"],[" 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?

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?

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 3.06g of solid NH_4HS is introduced into a 21 evacuated flask at 27^(@) C, 30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. Calculate K_c and K_p for the reaction at 27^(@) C

When 3.06g of solid NH_4HS is introduced into a 21 evacuated flask at 27^(@) C, 30% of the solid decomposes into gaseous ammonia and hydrogen sulphide. what would happen to the equilibrium when more solid NH_4HS is introduced into the flask?

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) ]