Question

Consider the chemical reaction: NO + Cl2 → NOCI + CI This reaction is first order in each reactant and second order overall. To measure the rate constant, k, you decide to overload the amount of Cl2, at a concentration of 4 mol/L. The NO concentration used is much lower than this value. It is a good approximation to assume that the concentration of Cl2 does not change during the time that the reaction is studied, because it is in great excess. You measure [NO] as a function of time and plot the data as In([NO]/[NO].) versus time, where [NO], is the initial concentration of NO. You then fit a line to the data, as shown below, with the value of the slope indicated on the graph. -1 -2 slope = -12 s 80 -6 In ([NO]/[NON 80000 -8 -10 -12 0 0.2 0.4 0.6 time / s 0.8 Based on data in the plot, what is the value of the overall second order rate constant, k, for this reaction? 1 k= L-mol-1.9-1 OK 1 L.mol-1 -1 . S 3 ok 3 L.mol-1 • S -1 O k = 4 L.mol-1 • S Ok= 12 L.mol-1.s-1 O k= 24 L.mol-1 S s-1 O k= 48 L.mol-1.8-1

please show the work

Answer 1

We know, Rate = k [NO] [ce When [ce] is taken in excess , Rate KENO] where k'=k [Cl] Cconstane) You, we are geven, k" = 19 s-1 [es] - 4 mol/L k = [ce, 19 - 4 mol IL k = 3 mol-Ls - se cond order rate constant