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

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 :

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 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.

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: