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1.50 moles each of hydrogen and iodine w...

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

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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

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

What will be the equilibrium constant at 717K for the reaction 2HI(g) hArr H_2(g) +I_2(g) if K for H_2(g) +I_2(g) hArr 2HI at 717 K is 50.