Dissociation of `PCl_(5)` decreases in presence of increase in `Cl_(2)` why ?

Why does dissociation rate of H_(2)S is decreased in presence of HCl in aqueous solution ?

Why does dissociation rate H_2S is decreased in presence of HCL in aqueous solutio?

Does the number of moles of reaction products increase, decrease of remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume? PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g)

The equilibrium established during thermal dissociation of PCl_(5)(g) in a closed vessel is as follows: PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g) If the degree of dissociation of PCl_(5)(g) at equilibrium be 'x', then show that (1) 'x' is inversely proportional to the square root of the total pressure of reaction mixture at equilibrium and (2) 'x' increases with increase in volume of the system.

For a weak electrolyte, the degree of dissociation decreases but specific conductance increases with the increase in concentration of its solution. Why?

Give the reactions of Cl_2 and CH_4 in presence of diffused sunlight.

At 473K, equilibrium constant K_(c) for decomposition of PCl_(5) is 8.3x10^(-3) . If decomposition is depicted as, PCl_(5)(g)hArr PCl_(3)(g)+Cl_(2)(g), DeltaH_(r)^(0)=124.0kJ*mol^(-1) What would be the effect on K_(c) if (i) more PCl_(5) is added (ii) presure is increased (iii) the temperature is increased?

How does PCl_(5) exist in the solid state ?