At a certain temperature and total pressure of `10^(5)Pa`, iodine vapour contains `40%` by volume of `I` atoms
`I_(2)(g)hArr2I(g)`
Calculate `K_(p)` for the equilibrium

At 1127K and 1 atm pressure, a gaseous mixture of CO and CO_(2) in equilibrium with soild carbon has 90.55% CO by mass C(s)+CO_(2)(g)hArr2CO(g) Calculate K_(c) for this reaction at the above temperature.

A mixture of one mole of CO_(2) and one mole of H_(2) attains equilibrium at a temperature of 250^(@)C and a total pressure of 0.1 atm for the change CO_(2(g)) +H_(2(g)) harr CO_((g))+H_(2)O_((g)) . Calculate K_(P) if the analysis of final reaction mixture shows 0.16 volume fraction of CO

0.5 mol of H_(2) and 0.5 mole of I_(2) react in 10 litre flask at 448^(@)C . The equilibrium brium constant K_(C) is 50 for H_(2)(g)I_(2)(g) hArr 2HI(g) Calcualte mole of I_(2) at equilibrium.

One mole of H_(2)O and one mole of CO are taken in 10L vessel and heated to 725K . At equlibrium 40% of water (by mass) reacts with CO according to the equation. H_(2)O(g)+CO(g)hArrH_(2)(g)+CO_(2)(g) Calculate the equilibrium constant for the reaction.

4.5 mol each of H_(2) and I_(2) are present in a 10 lit vessel . At equilibrium the mixture contains 3 mole . HI , Kp for H_(2) + I_(2) hArr 2 HI and mass of I_(2) at equilibrium (in g) respectively are

At constant temperature & volume , 50% of ozone is decomposed out of 2 atm of ozone taken initially and the equilibrium 2O_(3 (g)) hArr 3O_(2 (g)) is established , K_(p) for the decomposition of ozone is

At a certain temperature the equilibrium constant K_c is 0.25 for the reaction A_(2(g))+B_(2(g)) harr C_(2(g))+D_(2(g)) If we take 1 mole of each of the four gases in a 10 litre container, what would be equilibrium concentration of A_(2(g)) ?

A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is K_(p) for the given equilibrium ? 2HI(g)hArrH_(2)(g)+I_(2)(g)

0.5 mol of H_(2) and 0.5 mole of I_(2) react in 10 litre flast at 448^(@)C . The equilibrium constant K_(c) is 50 for H_(2)(g)+I_(2)(g)hArr2HI(g) a. What is the value of K_(p) b. Calculate mole of I_(2) at equilibrium.

Consider the following equilibrium PCl(g) hArr PCl_(3)(g) + Cl_(2)(g) in a closed container. At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements holds true regarding the equilibrium constant (K_(p)) and degree of dissocitation (alpha) ?