For the reaction : `2NO(g) + Cl_(2) (g) hArr 2NOCl (g), NO` and `Cl_(2)` are initially taken in mole ratio `2 : 1`. The total pressure at equilibrium is found to be `1 atm`. If mole of `NOCl` are one fourth of that of `Cl_(2)` at equilibrium, `K_(p)` for the reaction is:

For the reaction : 2NO(g)+Cl_(2)hArr 2NOCl (g) : which is true :

Equilibrium constant for the reaction 2NO(g) + Cl_(2)(g) hArr 2NOCl(g) is correctly given by the expression

For the equilibrium 2NO(g)+Cl_(2)(g)hArr 2NOCl(g) K_(p) is related to K_(c) by the reaction

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

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

In the reaction, PCl_5 hArr PCl_3 + Cl_2 , the amounts of PCl_5 PCl_3 and Cl_2 at equilibrium are 2 mole each and the total pressure is 3 atm. The equilibrium constant K_p is:

For the reaction, 2NO(g)+Cl_(2)(g)hArr 2NOCl(g) a reaction mixture containing NO(g) and Cl_(2)(g) at partial pressure of 0.373 atm and 0.310 atm at 300 K respectively, is taken. The total pressure of the system at equilibrium was found to be 0.544 atm at 300 K. The value of K_(C) for the reaction, 2NOCl(g)hArr 2NO(g)+Cl_(2)(g) at 300 K would be

For the reaction, 2NO(g)+Cl_(2)(g)hArr 2NOCl(g) a reaction mixture containing NO(g) and Cl_(2)(g) at partial pressure of 0.373 atm and 0.310 atm at 300 K respectively, is taken. The total pressure of the system at equilibrium was found to be 0.544 atm at 300 K. The value of K_(C) for the reaction, 2NOCl(g)hArr 2NO(g)+Cl_(2)(g) at 300 K would be