In an experiment , 2 moles of HI are taken into an evacuated 10.0 litre container at 720 K. The equilibrium constant equals to 0.0156for the gaseous reaction, `2 HI (g) hArr H_(2) (g) + I_(2)(g).` find equilibrium concentration of ` HI (g) , H_(2) (g) , I_(2)(g).`

In an experiment 5 moles of HI were enclosed in a 5 litre container . At 717 K equilibrium constant for the gaseous reaction , 2HI (g) hArr H_2(g) +I_2(g) is 0.025 . Calculate the equilibrium concentration of HI ,H_2 and I_2 . What is the fraction of HI that decomposes ?

In an experiment 5 moles of HI were enclosed in a 5 litre container . At 717 K equilibrium constant for the gaseous reaction , 2HI (g) hArr H_2(g) +I_2(g) is 0.025 . Calculate the equilibrium concentration of HI H_2 and I_2 . What is the fraction of HI that decomposes ?

the value of equilibrium constant for the reaction HI(g) hArr 1//2 H_(2) (g) +1//2 I_(2) (g) " is " 8.0 The equilibrium constant for the reaction H_(2) (g) +I_(2) (g) hArr 2HI(g) will be

If the equilibrium constant of the reaction 2HI(g)hArrH_(2)(g)+I_(2)(g) is 0.25 , find the equilibrium constant of the reaction. (1)/(2)H_(2)+(1)/(2)I_(2)hArrHI(g)

If the equilibrium constant of the reaction 2HI(g)hArrH_(2)(g)+I_(2)(g) is 0.25 , find the equilibrium constant of the reaction. (1)/(2)H_(2)+(1)/(2)I_(2)hArrHI(g)

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:

The value of equilibrium constant of the reaction, H(g) hArr(1)/(2) H_(2)(g) is 0.8 . The equilibrium constant of the reaction H_(2)(g) + I_(2)(g)hArr2HI(g) will be

The value of equilibrium constant for the reaction H_(2)(g)+ I_(2) (g) hArr 2HI (g) is 48 at 720 K What is the value of the equilibrium constant for the reaction 2HI (g) hArr H_(2) (g) + I_(2) (g)