For the reaction `2NOCl(g) hArr 2NO(g)+Cl_(2)(g)`, the equilibrium constant is `2.8xx10^(-5)` at `300 K` and `7.0xx10^(-1)` at `400 K`. What is the activation energy for the reaction?

For the reaction, 2NOCl(g)hArr2NO(g)+Cl_(2)(g) the value of K_(c)=3.75xx10^(-6) at 1069K. Calculate K_(p) .

For the reaction, 2HCl_((g))hArrH_(2(g))+Cl_(2(g)) , the equilibrium constant is 1.0xx10^(-5) . What is the concentration of HCl if the equilibrium concentrations of H_(2) and Cl_(2) are 1.2xx10^(-8)M and 1.2xx10^(-9)M respectively?

For the equilibrium 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) the value of the equilibrium constant, K_(c) is 3.75 xx 10^(-6) at 1069 K . Calcualate the K_(p) for the reaction at this temperature?

For the equilibrium 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) the value of the equilibrium constant, K_(c) is 3.75 xx 10^(-6) at 1069 K . Calcualate the K_(p) for the reaction at this temperature?

For the reaction: NOCl(g) hArr 2NO(g) +Cl_(2)(g), K_(c) at 427^(@)C is 2xx10^(6) L mol^(-1) . The value of K_(p) is

For the equilibrium , 2NOCl(g)hArr2NO(g)+Cl_(2)(g) the value of the equilibrium constant, K_(c) is 3.75xx10^(-6) at 1069K . Calculate the K_(p) for the reaction at this temperature ?