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1.50 moles each of hydrogen and iodine i...

`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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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

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

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.

4.5 moles each of hydrogen and iodine heated in a sealed 10 litrevesel. At equilibrium, 3 moles of HI was foun. The equilibrium constant for H_(2)(g) + I_(2) (g)hArr2HI(g) is