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?

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?

N_2(g) + O_2(g) harr 2NO_(g) what is the effect of pressur on the above equilibrium?

Consider the equilibrium, PCl_(5(g)) harr PCl_(3(g)) + Cl_(2(g)) What happens to the above equillibrium when an inert gas is added at constant pressure? Justify.

A system at equilibrium is described by the equation "Heat" + SO_2CI_2 (g) ⇌ SO_2 (g) + CI_2(g) the addition of CI_2 in the reaction mixture will shift the equillibrium into?

At 1000K, equilibrium constant K_c for the reaction 2SO_3(g) harr 2SO_2(g)+O_2(g) is 0.027. What is the value of K_p at this temperature?

The equilibrium constant of the reaction H_2(g) + I_2(g) harr 2HI(g) is 57 at 700 K. Now, give the equilibrium constants for the following reaction at the same temperature: 4HI(g) harr 2H_2(g) +2I_2(g)