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

The net force is 100

Aquantity of that isotope to decay to 1/2 of  its original value