Question

A student proposed the following mechanism for the gas phase reaction of fluorine with chlorine dioxide. step 1 fast: 2C10, C1,04 step 2 slow: Cl,04 + F2 — 2 FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"B"... , where 'l' is understood (so don't write it if it's a 'l') for m, n etc. Rate - Submit Answer Retry Entire Group 4 more group attempts remaining

Answer 1

solution : Mechanism :- u stept fast: quo2 - chou stap2 slow! Cl204+f2 25 02 overall sueaction - - Adding both steps 1 and 2 3 2002 + Cl20y + f2 choy +2 fc02 [2102 + Fz 2FCO2 is the overall reaction = 19 , P. (3 Any species wheils is formed in one step and consumed in next step is alled intermediate raction intermediate is (204) m a multistep reaction, rate low is given by slowest step. - rate Low from slow step 2 is nate = K (83[ck Oy)

But Chou is reactions intermediate so eliminating it with the help of step). Applying low af equilibria on Step ka [ulzou] [102] [c2y] = k fung? Puthy (chon] in ero >> rate = k ke[1037Ba] =) rate = K [dz]²/[z] 5 the requred rate how