In a reaction between hydrogen and iodine `6.84 mol` of hydrogen and `4.02` mol of iodine are found to be in equilibrium with `42.85` mol of hydrogen iodide at `350^(@)C.` Calculate the equilibrium constant.

An equillibrium reaction between hydrogen and iodine to give hydrogen iodide at 670 K in a 5 litre flask contains 0.4 mole of hydrogen 0.4 mole of iodine and 2.4 mole of hydrogen iodide. Calculate the equillibrium constants.

An equilibrium system for the reaction between hydrogen and iodine to give hydrogen iodide at 670 K in a 5 litre flask contains 0.4 mole of hydrogen , 0.4 mole of iodine and 2.0 moles of hydrogen iodide. Calculate equilibrium constant.

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 :

one mole of hydrogen iodide is heated in a closed container of 2 litre. At equilibrium half mole of hydrogen iodide has dissociated. What is the value of the equilibrium constant ?

An equilibrium system for the reaction between hydrogen and iodien to give hydrogen iodide at 765 K in a 5 litre volume contains 0.4 mole of hydrogen iodide. The equilibrium constant for the reaction H_(2) + I_(2)hArr 2HI is