[" The dissociation of ammonium carbamate "],[" may be represented by the equation : "],[NH_(4)CO_(2)NH_(2)(s)rightleftharpoons2NH_(3)(g)+CO_(2)(g)],[Delta H^(0)" for the forward reaction is negative.The "],[" equilibrium will shift from right to left if there "],[" is "]

NH_(4)COONH_(4)(s) hArr 2NH_(3)(g)+CO_(2)(g) . for the above reaction, K_(p) is 4, K_c will be

Unit of K_p for NH_4COONH_(2(s)) harr 2NH_(3(g))+ CO_(2(g)) is

NH_(2)COONH_(2)(s) harr 2NH_(3)(g) + CO_(2)(g) If equilibrium pressure is 3 atm for the above reaction, K_(p) will be

The equilibrium constant Kp for the reaction NH_(4)HS_((s)) Leftrightarrow NH_(3(g))+H_(2)S_((g)) is

NH_(4)COONH_(4)(s) hArr 2NH_(3)(g)+CO_(2)(g) . If equilibrium pressure is 3 atm for the above reaction, K_(p) will be

The K_(p) of the reaction is NH_(4)HS_((s)) Leftrightarrow NH_(3(g))+H_(2)S_((g)) . If the total pressure at equilibrium is 30 atm.

The decomposition of solid ammonium carbamete, (NH_(4))(NH_(2)CO_(2)) , to gaseous ammonia and carbon dioxide is an endothermic reaction. (NH_(4))(NH_(2)CO_(2)) (s)hArr2NH_(3) (g) + CO_(2)(g) Given that the decomposition reaction is at equilibrium, how would the following changes affect the total quantity of NH_(3) in the flask once equilibrium is re-established ? Adding (NH_(4)) (NH_(2)CO_(2))

In the equilibrium NH_(4) HS_(s) hArr NH_(3(g)) + H_(2) S_((g)) . the forward reaction can be favoured by