At a certain temp. `2HI hArrH_(2) + I_(2)` . Only `50%` HI is dissociated at equilibrium. The equilibrium constant is

At a certain temperature , 2HI ⇌ H_2 + I_2 on 50 % HI is dissolved at equilibrium .What the value of equilibrium constant ?

When 2.00 mol each of H_2(g) and I_2(g) are reacted in a 1.00 L container at a certain temperature , 3.50 mol of HI is present at equilibrium.Calculate the value of the equilibrium constant , K_c for the reaction : H_2+I_2hArr 2HI

At a certain temperature , only 50% HI is dissociated at equilibrium in the following reaction: 2HI(g)hArrH_(2)(g)+I_(2)(g) the equilibrium constant for this reaction is:

At a certain temperature , only 50% HI is dissociated at equilibrium in the following reaction: 2HI(g)hArrH_(2)(g)+I_(2)(g) the equilibrium constant for this reaction is:

At a certain temperature , only 50% HI is dissociated at equilibrium in the following reaction: 2HI(g)hArrH_(2)(g)+I_(2)(g) the equilibrium constant for this reaction is:

For the reaction 2 HI hArr H_(2) + I_(2) the equilibrium constant K at 440^(@)C is 0.022 . The equilibrium constant for I_(2) + H_(2) hArr 2 HI is

256 g of HI were heated in a sealed bulb at 444°C till the equilibrium was attained. The acid was found to be 22% dissociated at equilibrium. Calculate the equilibrium constant for the reaction 2HI(g) hArr H_2(g) +I_2 (g)