The equilibrium constant for the reaction `N_2(g) +O_2(g) hArr 2NO(g) "is" 4 xx 10^(-4)` at 200 k . In the presence of a catalyst the equilibrium is attained 10 times faster therefore, the equillbrium constant in presence of the catalyst at 200 k is

The equilibrium constant for the reaction N_(2)(g)+O_(2)(g) hArr 2NO(g) is 4.0xx10^(-4) at 2000 K . In the presence of a catalyst, the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in presence of the catalyst at 2000 K is

The equilibrium constant for a reacton N_(2)(g)+O_(2)(g)=2NO(g) is 4xx10^(-4) at 2000 K . In the presence of catalyst, the equilibrium constant is attained 10 times faster. The equilibrium constant in the presence of catalyst, at 2000 K is

The equilibrium constant for the reaction N_(2(g))+O_(2(g)) Leftrightarrow 2NO_((g)) at 2000K is 4 * 10^-4 In presence of a catalyst the equilibrium is attained three times faster. The equilibrium constant in presence of the catalyst at 2000 K

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

Equilibrium constants (K) for the reaction 2NO(g)+Cl_(2)(g)hArr2NOCl(g) is correctly given by the expression

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?