The elementary reaction 2h2o(g)↽−−⇀2h2(g)+o2(g) proceeds at a certain temperature until the partial pressures of h2o, h2, and o2 reach 0.0750 atm, 0.00700 atm, and 0.00200 atm, respectively. what is the value of the equilibrium constant at this temperature?

is the value of the equilibrium constant at this temperature.

Explanation:

We are given:

Partial pressure of

Partial pressure of

Partial pressure of

The expression of for the given chemical equation is:

Putting values in above equation, we get:

is the value of the equilibrium constant at this temperature.

b.final

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