Mole of `PCl_(5)` is heated in a closed vessel of 1 litre capacity. At equilibrium 0.4 moles of chlorine is found. Calculate the equilibrium constant.

Starting from one mole each of anol and acetic acid, at equilibrium 2//3 mole of ester is formed . Calculate the equilibrium constant.

A mixture of 2 moles of N_(2) and 8 moles of H_(2) are heated in a 2 lit vessel, till equilibrium is established. At equilibrium, 04 moles of N_(2) was present. The equilibrium concentration of H_(2) will be

4.5 moles, each of hydrogen and iodine was heated in a sealed 10 L vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H_(2) (g) + I_(2) (g) rarr 2HI (g) , is

1.0 mole of ethyl alcohol and 1.0 mole of acctic acid are mixed. At equilibrium, 0.666 mole of ester is formed. The value of equilibrium constant is

3.00 mol of PCl_(5) kept in 1L closed reaction vessel was allowed to attain equilibrium at 380K . Calculate composition of the mixture at equlibrium K_(c)=1.80

One mole of A_((g)) is heated to 300^(@) C in a closed one litre vessel till the following equilibrium is reached. A_((g)) hArr B_((g) . The equilibrium constant of the reaction at 300^(@) C is 4. What is the conc. of B ("in. mole. lit"^(-1)) at equilibrium ?

1.1 mole of A and 2.2 moles of B reach an cquilibrium in I lit container according to the reaction. A + 2B hArr 2C + D. If at equilibrium 0.1 mole of D is present, the equilibrium constant is: