1. Tardigrade
  2. Question
  3. Chemistry
  4. 1.50 moles each of hydrogen and iodine is 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 Kc for the reaction. H2(g) + I2(g) leftharpoons 2HI(g) at 717 K is

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Q. $1.50$ moles each of hydrogen and iodine is 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. $H_{2}(g) + I_{2}(g) \rightleftharpoons 2HI(g)$ at $717$ K is

Equilibrium

Solution:

Correct answer is (b) $0.16$

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