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

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

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

The number of moles of H_(2) in 2.24 litre of hydrogen gas at STP

The number of moles of H_(2) in 0.224 litre of hydrogen gas at STP is

An equilibrium system for the reaction between hydrogen and iodine to give hydrogen iodide at 765 K in a 5 litre volume contains 0.4 mole of hydrogen, 0.4 mole of iodine and 2.4 moles of hydrogen iodide, The equilibrium constant for the reaction is : H_2+I_2 hArr 2HI , is :

Number of moles of hydrogen will required for complete hydrogenation of one mole of following compound