One mole of `H_(2)` and 2 moles of `I_(2) ` are taken initially in a two litre vessel. The number of moles of `H_(2)` at equilibrium is 0.2. Then the number of moles of `I_(2)` and `HI` at equilibrium is

1 mol of hydrogen and 2 mol of iodine are taken initially in a 2L vessel. The number of moles of hydrogen at equilibrium is 0.2 . Then the number of moles of iodine and hydrogen iodide at equilibrium are

In 5 litre container 1 mole of H_(2) and 1 mole of I_(2) are taken initially and at equilibrium of HI is 40% . Then K_(p) will be

In 5 litre container 1 mole of H_(2) and 1 mole of I_(2) are taken initially and at equilibrium of HI is 40% . Then K_(p) will be

Hydrogen (a moles) and iodine (b moles) react to give 2x moles of the HI at equilibrium. The total number of moles at equilibrium is

Hydrogen (a moles ) and iodine (b moles ) react to give 2x moles of the HI at equilibrium . The total number of moles at equilibrium is

Hydrogen (a moles ) and iodine (b moles ) react to give 2x moles of the HI at equilibrium . The total number of moles at equilibrium is

2 mole of H_(2) and "1 mole of "I_(2) are heated in a closed 1 litre vessel. At equilibrium, the vessel contains 0.5 mole HI. The degree of dissociation of H_(2) is

2 mole of H_(2) and "1 mole of "I_(2) are heated in a closed 1 litre vessel. At equilibrium, the vessel contains 0.5 mole HI. The degree of dissociation of H_(2) is

15 moles of H_(2) and 5.2 moles of I_(2) are mixed and allowed to attain equilibrium at 500^(@)C . At equilibrium, the number of moles of HI is found to be 10 mole. The equilibrium constant for the formation of HI is