Need help asap - There is an error in the rate-determining step of the following proposed mechanism. Slow step: CH3(g) + Cl2(g) → CH3(g) + HCl(g) and the rate rule is k1 = [CH4][Cl2]
Fast step: CH3(g) + Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]
Overall : CH4(g) + 2Cl2(g) → CH3Cl(g) + HCl(g) + Cl–(g)

Which shows the correct rate-determining step for the mechanism?

CH4(g) + 2Cl(g) → CH3Cl(g) + HCl(g) + Cl–(g)
CH4(g) + Cl2(g) → CH3(g) + HCl(g) and the rate rule is k1 = [CH4][Cl2]
CH4(g) + Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]
CH3(g) + 2Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]

Explanation:

Need help asap - There is an error in the rate-determining step of the following proposed mechanism.

Slow step: CH3(g) + Cl2(g) → CH3(g) + HCl(g) and the rate rule is k1 = [CH4][Cl2]

Fast step: CH3(g) + Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]

Overall : CH4(g) + 2Cl2(g) → CH3Cl(g) + HCl(g) + Cl–(g)

Which shows the correct rate-determining step for the mechanism?

CH4(g) + 2Cl(g) → CH3Cl(g) + HCl(g) + Cl–(g)

CH4(g) + Cl2(g) → CH3(g) + HCl(g) and the rate rule is k1 = [CH4][Cl2]

CH4(g) + Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]

CH3(g) + 2Cl2(g) → CH3Cl(g) + Cl–(g) and the rate rule is k2 = [CH4][Cl2]

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