13. Two students are measuring the rate of the reaction S2O32- (aq) + 3 I-(aq) + 2 SO42- (aq) + 13- (aq) One student follows the disappearance of I-(aq) and states that the rate of reaction is 5.1 M/s. The other student observes the production of I3- (aq) and states that the rate of reaction is 1.7 M/s. Their experimental design and equipment used are valid. (See Section 11-1 and 11-1a) a. How can one observed-rate have a positive value and the other observation be a negative value? b. Explain why the magnitude of the rate with respect to iodide (1-) is three time that of the triiodide (137) c. How are the observed rates related to the "rate of reaction"? 14. Given the following set of data, determine the rate law expression and the value of the rate constant. Reaction: A + B products Initial Conc. of A Initial Conc. of B Initial Rate (M) (M) (M/s) 0.10 0.10 0.20 0.20 0.10 0.40 0.30 0.10 0.60 0.30 0.20 2.40 0.30 0.30 5.40 12. The data below were obtained for decomposition of aqueous hydrogen peroxide at 20C. 2 H2O2(aq) + 2 H2O(1) + O2(g) Time (min) [H202] (mol/L) 0 0.0200 200 0.0160 400 0.0131 600 0.0106 800 0.0086 1000 0.0069 1200 0.00535 1600 0.0037 2000 0.0024 a. Have each member of the group calculate the rate over a different time period (i.e., t=0 to t=200 min and t=400 min to t=600 min). Explain why each member of the group should have a different rate. b. Suppose you wanted the initial rate of reaction to be twice the initial rate observed without raising the temperature. (The initial rate is the rate from t=0 to t=200 min) What could you do? C. Sketch a plot of concentration versus time. And, sketch a plot of initial rate of reaction (these are the answers to a.) versus the initial time (the first or smallest time point). (the x-axis should be time for both plots) The shape of the plots are not expected to be the same. Which one is linear