A mixture of 0.2000 mol of CO2, and 0.4000 mol of H2 is placed in a 2.000L vessel. The following equilibrium is established at 400.K; CO(g) + H2O(g) ↔ CO2(g) + H2(g)
At equilibrium PH2O = 2.35 atm
a.) Calculate the equilibrium partial pressure of CO2, H2 and CO.

NEED HELP ASAP

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole