Acetic acid and water react to form hydronium cation and acetate anion, like this: HCH3CO2(aq) + H2O(l) →H3O+ (aq) + CH3CO2-(aq)

Imagine 226. mmol of CH3CO2- are added to a flask containing a mixture of HCH3CO2, H2O, H3O + and CH3CO2- at equilibrium, and then answer the following questions.

a. What is the rate of the reverse reaction before any CH3CO2- has been added to the flask?
b. What is the rate of the reverse reaction just after the CH3CO2- has been added to the flask?
c. What is the rate of the reverse reaction when the system has again reached equilibrium?
d. How much more CH3CO2- is in the flask when the system has again reached equilibrium?

we need the questions , i may then you.

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