The following is a proposed mechanism for the chlorination of methane. Use the information to solve for a,b, and c. step 1 CH) + Cl{g}CH3) + HCl) + Cl •slowstep 2 CH) + Clu9)CH;Cl(g) +Cl •fasta. Write the overall chemical reaction and write an overall rate expression for the appearance ofCH3CI(g)-Note that this rate expression can include the concentration of intermediates.b. Using your answer to part b, write the rate expression for the change in concentration of CH3(g)-c. Using the steady state approximation. give an expression for the appearance of CH3CI (g) thatdoes not depend on the concentration of CH3 e). Note that the first reaction is reversible and thesecond is not.

Steady state approximation is used to determine the rate law of an equation, it uses the fact that an intermediate formed in a reaction is consumed so quickly as it formed, therefore, practically its concentration is remained constant.Ans a) Overall chemical reaction: To write the balanced chemical reaction, the intermediate should be removed from the equation, therefore we get, CH4(g)+2Cl2→CH3Cl(g)+HCl(g)+2Cl∙ Rate expression for CH3Cl : Let the K1 and K2 be the forward rate constant for equation 1 and 2 respectively. Rate= K2 [CH3][Cl2] -------1 Ans b) Rate expression for CH3 :- Rate = K1[CH4][Cl2] - K2[CH3][Cl2] Ans c) Using steady state approximation, Rate of formation of CH3 = Rate of deformation of CH3 K1[CH4][Cl2]= K2[CH3][Cl2] [CH3]=K1[CH4][Cl2]K2[Cl2]=K1[CH4]K2 Using the determine value for concentration of CH3 in equation 1, we will get Rate = K1[CH4][Cl2]