- #1
johnny b
- 8
- 0
Homework Statement
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?
Homework Equations
ΔrG = ΔfG(products) - ΔfG(reactants)
ln K = -ΔrG / RT
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.