`1.50` moles each of hydrogen and iodine is p[laced in a sealed 10 litre container maintained at 717 K. At equilibrium `1.25` moles each of hydrogen and iodine were left behind. The equilibrium constant `K_(c)` for the reaction `H_(2)(g) + I_(2)(g)hArr2HI(g) at 717` K is

Options

A. `0.4`
B. `0.16`
C. 25
D. 50

Answer

B

Explanation

`H_(2)(g) + I_(2)(g)hArr2HI(g)`
`t = 0` `1.5` `1.5` 0
`t = t_(equiv)` `1.5-x` `1.5-x` 2x
We, know, `1.5-x = 1.23`, or `x = .25`
`K_(c) = ((.5)^(2))/((1.25)^(2)) = 0.16`