`COCl_(2)` gas dissociates according to the equation, `COCl_(2)hArrCO(g)+Cl_(2)(g)`. When heated to 700 K the density of the gas mixture at 1.16 atm and at equilibrium is `1.16 g//litre` The degree of dissociation of `COCl_(2)` at 700K is :

The dissociation of phosgene, which occurs according to the reaction COCl_(2)(g)hArrCO(g)+Cl_(2)(g) Is an endothermic process. Which of the following will increase the degree of dissociation of COCl_(2)?

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.

Phosgene, COCl_(2) , a poisonous gas decomposes according to the equation COCl_(2)(g)hArrCO(g)+Cl_(2)(g) If K_(c)=0.083 at 900^(@)C , What is the value of K_(p) ?

Phosgene, COCl_(2) , a poisonous gas decomposes according to the equation COCl_(2)(g)hArrCO(g)+Cl_(2)(g) If K_(c)=0.083 at 900^(@)C , What is the value of K_(p) ?

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

PCl_(5) vapour decomposes on heating according to the reaction : PCl_5 (g) hArr PCl_(3) (g) + Cl_(2)(g) The density of a sample of a partially dissociated PCl_(5) at 1.0 atm and 500 K was found 4.8 g/L . Calculate the degree of dissociation and DeltaG^(@) for the reaction at 500 K (Given R=0.082 L atm K^(-1)mol^(-1) ) , R=8.314 JK^(-1) mol^(-1) , In x=2.3031 log_(10)x )

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

For the reactions, CO(g) +Cl_2( g) hArr COCl_2(g), " the " (K_P)/(K_c) is equal to