For the reaction `N_2O_4 hArr 2NO_2`, at 350 K, the value of `K_c =0.4`.The value of `K_p` for the reaction at the same temperature would be :

For a reaction N_2+3H_2 hArr 2NH_3 , the value of K_c would depend upon

For a reaction N_2+3H_2 hArr 2NH_3 , the value of K_c would depend upon

At 700 K , the equilibrium constant , K_p for the reaction 2SO_3(g) hArr 2SO_2(g) +O_2 (g) is 1.8 xx10^(-3) atm. The value of K_c for the above reaction at the same temperature in moles per litre would be

At 700 K , the equilibrium constant , K_p for the reaction 2SO_3(g) hArr 2SO_2(g) +O_2 (g) is 1.8 xx10^(-3) atm. The value of K_c for the above reaction at the same temperature in moles per litre would be

At 700K, the equilibrium constant K_(p) , for the reaction 2SO_(3(g))hArr2SO_(2(g))+O_(2(g)) is 1.8xx10^(-3) atm. The value of K_(c) for the above reaction at the same temperature in moles per litre would be

Value of K_(p) for the equilibrium reaction N_(2)O_(4(g)) hArr 2NO_(2(g)) " at " 288K is 47.9. The K_(C ) for this reaction at same temperature is _____(Nearest integer) (R=0.083 L "bar" K^(-1) mol^(-1))

For a reaction N_2 + 3H_2 harr 2NH_3 the value of K_C would depend upon

Calculate K_p from K_c : The equilibrium constant, K_c , for the reaction N_2O_4(g) hArr 2NO_2(g) is 3.64xx10^-3 at 25^@C . What is the value of K_p at this temperature?