`COCl_(2)` gas decomposes as:
`COCl_(2)(g) hArr CO(g)+Cl_(2)(g)`
If one mole of He gas is added in the vessel at equilibrium at constant pressure then

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 ?

The dissociation of phosgene is represented as follows: COCl_2 (g) hArr CO(g) +Cl_2( g) When a mixture of these three gasses at equilibrium is compressed at constant temperature , what happens to the partial pressure of COCl_2 :

The dissociation of phosgene is represented as follows: COCl_2 (g) hArr CO(g) +Cl_2( g) When a mixture of these three gasses at equilibrium is compressed at constant temperature , what happens to the equilibrium constant for the reactions?

The dissociation of phosgene is represented as follows: COCl_2 (g) hArr CO(g) +Cl_2( g) When a mixture of these three gasses at equilibrium is compressed at constant temperature , what happens to the amount of CO in the mixture.

The equilibrium showing dissociation of phosgene gas is given below: COCl_2(g) harr CO(g) + Cl_2(g) When a mixture of these three gases at equilibrium is compressed at constant temperature, what happens to The partial pressur of COCl_2 ?

The equilibrium showing dissociation of phosgene gas is given below: COCl_2(g) harr CO(g) + Cl_2(g) When a mixture of these three gases at equilibrium is compressed at constant temperature, what happens to the equilibrium constant for the reaction?

The equilibrium showing dissociation of phosgene gas is given below: COCl_2(g) harr CO(g) + Cl_2(g) When a mixture of these three gases at equilibrium is compressed at constant temperature, what happens to The amount of CO in mixture?