1. The problem statement, all variables and given/known data Calculate the equilibrium constant for the reaction H2(g) + I2(g) <---> 2HI(g) at 80oC. The vapor pressure of solid iodine is 0.0216 bar at that temperature. If 52.7g of solid iodine are placed in a 10.0 L vessel at 80.0oC, what is the minimum amount of hydrogen gas that must be introduced in order to remove all of the solid iodine? 2. Relevant equations ΔrG = ΔfG(products) - ΔfG(reactants) ln K = -ΔrG / RT 3. The attempt at a solution ΔfG for HI(g) = 1.70, for H2(g) = 0 and for I2(g) = 19.33 KJ mol-1 ΔrG = 2(1.7) - 0 - 19.33 ΔrG = -15.93 KJ mol-1 ln K = -ΔrG / RT ln k = -(-15.93E3) / (8/314)(353) = 5.42 k = 225.9 Now I need to find the minimum amount of hydrogen gas and I have no idea where to start. Thanks for any help.