For `COCl_(2)(g) hArr CO(g) +Cl_(2)(g), K_(p)=8xx10^(-8)` atm. units at a certain temperature. Find the degree of dissociation of `COCl_(2)` at given temperature if the equilibrium pressure is 2.0 atm.

At 30^(@)C, K_(p) for the dissociation reaction : SO_(2)Cl_(2)(g) hArr SO_(2)(g)+Cl_(2)(g) is 2.9xx10^(-2) atm. If the total pressure is 1 atm, the degree of dissociation of SO_(2)Cl_(2) is : (assume 1-alpha^(2)=1 ).

For PCl_(5 (g)) hArr PCl_(3 (g)) + Cl_(2 (g)) at equilibrium , K_(P) = P//3 . Then degree of dissociation of PCl_(5) at that temperature is

For the reaction : CO(g)+Cl_(2)(g)hArr COCl_(2)(g) the K_(p)//K_(c ) is equal to :

The dissociation of phosgene, which occurs according to the equation COCl_2(g) iff CO(g) + Cl_2(g) is an endothermic process. Which of the following will increase the degree of dissociation of COCl_2 at constant pressure.

For the reaction CO_((g)) + Cl_(2(g)) hArr COCl_(2(g)). The K_(p)//K_(c) is equal to

The dissociation of phosgene gas (COCl_(2)) is represented as : COCl_(2) (g) hArr CO(g) + Cl_(2)(g) When the mixture of these three gases is compressed at constanat temperature , what happens to (i) the amount of CO in the mixture (ii) the partial pressure of COCl_(2) (iii) the equilibrium constant for the reaction ?