A reaction has the stoichiometry X+Y Product The following data were obtained for the reaction of 5.0 mM X with 5.0 mM Y at 25 C: [X] (MM) 2.1 1.4 1.0 0.71 0.45 0.28 Time (S) 10 20 30 45 75 125 A student plots In([X]) vs. time to determine the order (as in question 1c, above) and produces the following plot: Graph to Determine Order of Reaction 1.0 0.5- In([X]) Slope -0.017 +0.0024 Y-intercept 0.62 +0.15 0.0- In([X]) -0.54 -1.0- -1.5- -2.0+ 0 50 100 150 Time (s) a) What order is the reaction? What is happ? [4] b) [4] For a second-order reaction, and assuming that the orders with respect to the individual reactants are integral, what are the possible rate laws for a reaction X + Y Product ? How would you distinguish experimentally between the possibilities? Calculate the first and second half-times for the reaction in part (a). Calculate the concentration of X that would be present after 5.0 s if the initial concentrations of both X and Y were 20 mM. [2] [3] d)