If the reaction A+3B-> D+F follows the mechanism : A+ B-> C fast C+ B-> D + E sl
ID: 677140 • Letter: I
Question
If the reaction A+3B-> D+F follows the mechanism : A+ B-> C fast C+ B-> D + E slow E+ B-> F fast The rate law for the reaction is A. rate = k[A]2[B] B. rate =k[A][B]3 C. rate = k[D]2[E] D. rate = k[D][E] E. rate = k [C][B] A+ B-> C fast C+ B-> D + E slow E+ B-> F fast The rate law for the reaction is A. rate = k[A]2[B] B. rate =k[A][B]3 C. rate = k[D]2[E] D. rate = k[D][E] E. rate = k [C][B]Explanation / Answer
the rate determining step is c+b> D+E but C is an intermediate so we cant have that in teh final rateexpression inplace we can replace c with the first equation a+b+b> D+ e then add this to the 3rd fast step a+b+b+b>D+f so the rate expression would be rate= k [A][B]^3 so B