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
A
`0.4`
B
`0.16`
C
25
D
50
Text Solution
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The correct Answer is:
2
`{:(,H_(2)(g),+,l_(2)(g),hArr,2Hl(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`
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
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