Be sure to answer all parts. the equilibrium constant (kp) for the reaction below is 4.40 at 2000. k. h2 (g) + co2 (g) ⇌ h2o (g) + co (g) calculate δg o for the reaction. kj/mol calculate δg for the reaction when the partial pressures are ph2

When we have the balanced reaction equation is:

H2 (g) + CO2 (g) ↔ H2O (g) + CO (g)

a) first, to calculate ΔG° for the reaction:

we will use this formula:

ΔG° = - RT㏑Kp

when R is R - rydberg constant = 8.314J/mol. K

and T is the temperature in Kelvin = 2000 K

and Kp = 4.4

so, by substitution:

ΔG° = - 8.314 * 2000 * ㏑4.4

= - 24624 J/mol = - 24.6 KJ/mol

b) to calculate ΔG so, we will use this formula:

ΔG = ΔG° + RT㏑Qp

So we need first, to get Qp from the reaction equation:

when Qp = P products / P reactants

= PH2O*PCO / PH2 * PCO2

= (0.66 atm * 1.2 atm) / (0.25 * 0.78)

= 4.1

so by substitution:

ΔG = - 24624 + 8.314*2000*㏑4.1

= - 1162 J/mol = - 1.16 KJ/mol