T emperature range. When equilibrium is set up. 132. In a vessel, two equilibriurn are simultaneously established at the same temperature as follows: N(g) + 3H2(g) + 2NH3(g) N (g) + 2H2(g) N H (g) Initially the vessel contains N, and H, in the molar ratio of 9:13. The equilibrium pressure is 7Poin pressure due to ammonia is Po and due to hydrogen is 2P. Find the values of equilibrium constant (kpl both the reactions -214

In a vessel, two equilibrium are simultaneously established at the same temperature as follows N_2(g)+3H_2(g) hArr 2NH_3(g), K_(P_1) N_2(g)+2H_2(g) hArr N_2H_4(g), K_(P_2) Initially , vessel contains N_2 and H_2 in molar ratio 9:13. The equilibrium pressure is 7P_0 in which pressure due to NH_3 is P_0 and due to H_2 to 2P_0 Find the value of K_(P_2)/K_(P_1)

In a vessel, two equilibrium are simultanceously established at the same temperature as follows: N_(2)(g)+3H_(2)(g)hArr2 NH_(3)(g) .... (1) N_(2)g)+2H_(2)(g)hARrN_(2)H_(4)(g) ....(2) Initially the vessel contains N_(2) "and" H_(2) in the molar ratio of 9:13 . The equilibrium pressure is 7P_(0) , in wich pressure due to ammonia is P_(o) and due to hydrogen is 2P_(0) . Find the values of equilibrium constats (K_(p)'S) for both the reactions

In the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) the value of the equilibrium constant depends on

For gaseous reaction N_2(g) +3H_2(g) hArr 2NH_3(g) , the units of equilibrium constant K_p are ………..

In a container of constant volume at a particular temparature N_(2) and H_(2) are mixed in the molar ratio of 9:13 . The following two equilibria are found o be coexisting in the container N_(2)(g)+3H_(2)(g)harr2NH_(3)(g) N_(2)(g)+2H_(2)(g)harr N_(2)H_(4)(g) The total equiibrium pressure is found to be 305 atm while partial pressure of NH_(3)(g) and H_(2)(g) are 0.5 atm and 1 atm respectivly. Calculate of equilibrium constants of the two reactions given above.

N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) + heat .What is the effect of the increase of temperature on the equilibrium of the reaction ?