CO (g) CO2 (g) H2O (g) H2O (l) ‐137.1 ‐394.01 ‐228.4 ‐274.4 Given the above standard...

CO (g)	CO2 (g)	H2O (g)	H2O (l)
‐137.1	‐394.01	‐228.4	‐274.4

Given the above standard free energies of formation at 25oC in kJ/mole,

(a) Find ΔGo and the equilibrium constant Kp for the reaction CO (g) + H2O (g)CO2 (g) + H2 (g) at 25oC

(b) Find the vapor pressure of H2O (g) at 25oC.

(c) If CO (g) , CO2 (g) and H2 (g) are mixed so that the partial pressure of each is 1.00 atm and the mixture is brought into contact with excess liquid H2O, what will be the partial pressure of each gas when equilibrium is attained at 25oC? The volume available to the gases is constant.

Solutions

Expert Solution

B) the vapor pressure of H2O (g) at 25oC = 0,03128 atm ( vapor tables of thermodynamic)

queen_honey_blossom answered 5 months ago

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