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. Calculate the K_p for the reaction at this temperature ?

For the equilibrium 2NOCl_((g)) hArr 2NO_((g)) + Cl_(2(g)) the value

1.	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. Calculate the K_p for the reaction at this temperature ?
Answer» Solution :`{:("Reaction equilibrium:", 2NOCl hArr , 2NO_((G)) + , Cl_(2(g)) ), ("Stoichiometric :", 2,2,1):}` `therefore Deltan_((g))= sumn_("(g)product")-sumn_("(g)REACTANT")` =(2+1)-2 =+1 At given temperature equilibrium at gas phase, the reaction between `K_p` and `K_c`. `K_p=K_c (RT)^(Deltan)` where , `K_c=3.75xx10^(-6), Deltan = +1 , T=1069 K` R=0.0831 BAR L `"mol"^(-1) K^(-1)` `therefore K_p=(3.75xx10^(-6))(1069xx0.0831)` =`333.1 xx 10^(-6)=3.331xx10^(-4)` bar