Two moles of `PCl_5` were introduced in a 2L flask and heated at `600 K` to attain the equilibrium. `PCl_5` was found to be `40 %` dissociated into `PCl_3` and `Cl_2`. Calculate the value of `K c`.

For the reaction PCl_5 harr PCl_3 + Cl_2 Write the expression of Kc'

2AB_(2)(g) iff A_(2)(g)+2B_(2)(g) . 5 moles of AB_(2) were heated in a closed vessel to constant temperature. Equilibrium was attained by the time 2 moles of it dissociated. If the equilibrium pressure was 12 atm, the K_(p) of the reaction is very close to

One mole of H_2O and one mole of CO are taken in a 10L vessel and heated to 725K. At equilibrium 40% of water (by mass) reacts with CO according to the equation CO(g)+H_2O(g) iff H_2(g)+CO_2(g) Calculate the equilibrium constant for the reaction.

1.6 moles of PCl_(5)(g) is placed in 4dm^(3) closed vessel . When the temperature is raised to 500 K, it decomposes and at equilibrium 1.2 moles of PCl_(5)(g) remains . What is the K_(c) value for the decomposition of PCl_(5)(g) to PCl_(3)(g)andCl_(2)(g) at 500 K?