For a reaction :
`H_(2) (g) + I_(2) (g) hArr 2HI (g)`
at 721 K, the value of the equilibrium constant is 50. If 0.5 mole each of `H_(2) " and "I_(2)` are added to the system the value of the equilibrium constant will be :

For a reaction, H_2+I_2hArr 2HI at 721 K , the value of equilibrium constant is 50. If 0.5 moles each of H_2 and I_2 is added to the system the value of equilibrium constant will be :

For a reaction H_(2(g))+I_(2(g))rArr2HI_((g))at 721^(@)C the value of equilibrium constant is 50 . If 0.5 moles each of H_(2) & I(2) is added to the system the value of equilibrium constant will be .

For a reaction H_(2(g))+I_(2(g))rArr2HI_((g))at 721^(@)C the value of equilibrium constant is 50 . If 0.5 moles each of H_(2) & I(2) is added to the system the value of equilibrium constant will be .

For the reversible reaction H_2(g)+I_2(g)hArr2HI(g) the value of the equilibrium constant depends on the

2HI(g) rarr H_(2)(g) + I_(2)(g) The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H_(2) "and" I_(2) are added to the system, the equilibrium constant will be

2HI(g) rarr H_(2)(g) + I_(2)(g) The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H_(2) "and" I_(2) are added to the system, the equilibrium constant will be

2HI_((g))hArrH_(2(g))+I_(2(g)) The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole of H_(2) and I_(2) are added to the system, the equilibrium constant will be

For reaction : H_(2)(h)+I_(2)(g) hArr 2HI(g) at certain temperature, the value of equilibrium constant is 50 . If the volume of the vessel is reduced to half of its original volume, the value of new equilibrium constant will be