a' moles of `PCI_(5)`, undergoes, thermal dissociation as: `PCI(5)hArrPCI_(3)+CI_(2)`, the mole of `PCI_(3)` equilibrium is `0.25` and the total pressure is `2.0` atmosphere. The partial pressure of `CI_(2)` at equilibrium is:

For the reaction PCI_(5)(g) rightarrow PCI_(3)(g) + CI_(2)(g)

For the reaction PCI_(3)(g) + CI_(2)hArrPCI_(5)(g) the position of equilibrium can be shifted to the right by

For PCI_5(g) hArr PCI_3(g) +CI_2(g) , write the expression of K_c .

For PCI_5(g) hArr PCI_3(g) +CI_2(g) , write the expression of K_c .

In a reaction PCI_(5)hArrPCI_(3) + CI_(2) degree of dissociation is 30% . If initial moles of PCI_(3) is one then total moles at equilibrium is

Phosphorous pentachloride dissociates as follows (in a closed reaction vessel): PCI_(5)(g)hArrPCI_(3)(g)+CI_(2)(g) If the total pressure at equilibrium on the reaction mixture is P and the degree of dissociation of PCI_(5) is x, the partial pressure of PCI_(3) will be

4.0 moles of PCI_5 dissociated at 760 K in a 2 litre flask PCI_5 (g) hArr PCI_3 (g) +CI_2(g) at equilibrium . 0.8 mole of CI_2 was present in the flask .The equilibrium constant would be

4.0 moles of PCI_5 dissociated at 760 K in a 2 litre flask PCI_5 (g) hArr PCI_3 (g) +CI_2(g) at equilibrium . 0.8 mole of CI_2 was present in the flask .The equilibrium constant would be

The dissociation of PCI_5 decreases in presence of CI_2 Why ?

A quantity of PCI_(5) was heated in a 10 litre vessel at 250^(@)C, PCI_(5)(g)hArrPCI_(3)(g) + CI_(2)(g) . At equilibrium the vessel contains 0.1 mole of PCI_(5), 0.20 mole of PCI_(3) and 0.2 mole of CI_(2) . The equilibrium constant of the reaction is