Suppose the formation of iodine proceeds by the following mechanism: step elementary reaction rate constant 1 H2(9) + ICI(9) - HI(g) + HCl(9) ki 2 HI(g) + ICI(9) 1 (9) + HCI(9) k Suppose also kk2. That is, the first step is much slower than the second. 0-0 J. Write the balanced chemical equation for the overall chemical reaction: so Write the experimentally- observable rate law for the overall chemical reaction. 5 rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2 and (if necessary) the rate constants k-1 and K-2 for the reverse of the two elementary reactions in the mechanism. k = = 0 Consider the following elementary reaction: NO2(9) +F2(9) NO F(g) +F(9) Suppose we let ky stand for the rate constant of this reaction, and k_1 stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of F2 in terms of kj, k-2, and the equilibrium concentrations of NO2, NO2F, and F. [F2] = 0 0/6 . 6 J