1.50 moles each of hydrogen and iodine were placed 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) hArr 2Hl(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) harr 2HI(g)`
`{:(t=0, " "1.5, " "1.5, " "0),(t=t_(eq), " "1.5-x, " "1.5-x, " "2x):}`
We know, 1.5-x=1.25, or x= .25
`K_c=((.5)^2)/((1.25)^2)= .16`