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- List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
- The aqueous-phase decarboxylation of CH2NO2CO2H, CH2NO2CO2H CH3NO2(aq) + CO2(g), is studied at a certain temperature, giving the following data: Time (s) [CH2NO2CO2H] (M) 0.0e+00 0.100 1.0e-01 0.0466 2.0e-01 0.0217 3.0e-01 0.0101 4.0e-01 0.00473 Figure out whether this reaction is first-order or second-order with respect to the concentration of CH2NO2CO2H. Calculate the value of the rate constant. Pick the choice from below which gives the correct reaction order and value of the rate constant for this reaction.(a) Can an intermediate appear as a reactant in the firststep of a reaction mechanism? (b) On a reaction energyprofile diagram, is an intermediate represented asa peak or a valley? (c) If a molecule like Cl2 falls apart inan elementary reaction, what is the molecularity of thereaction?Suppose that for the reaction K + L------->M, you monitorthe production of M over time, and then plot the followinggraph from your data: (a) Is the reaction occurring at a constant rate from t = 0to t = 15 min? (b) Is the reaction completed at t = 15min? (c) Suppose the reaction as plotted here were startedwith 0.20 mol K and 0.40 mol L. After 30 min, an additional0.20 mol K are added to the reaction mixture.Which of the following correctly describes how the plotwould look from t = 30 min to t = 60 min? (i) [M] wouldremain at the same constant value it has at t = 30 min,(ii) [M] would increase with the same slope as t = 0 to15 min, until t = 45 min at which point the plot becomeshorizontal again, or (iii) [M] decreases and reaches0 at t = 45 min.
- (a) Most commercial heterogeneous catalysts are extremelyfinely divided solid materials. Why is particle sizeimportant? (b) What role does adsorption play in the actionof a heterogeneous catalyst?Use the following experimental data to determine the rate law of the reaction. Exp # [A]o [B]o d[C]/dt (M/s) 1 1.0 1.0 0.015 2 2.0 1.0 0.030 3 3.0 1.0 0.045 4 4.0 2.0 0.015Please include the reaction mechanism aswell
- of the units below which are appropriate for a second order reaction rate constantFor a first order reaction Arightwards arrowB the following data is collected at 3000C. Use the data in the table to determine concentration of A at 84 s. Time (s) Concentration of A (M) 0.00 0.350 10.00 0.185 Hint: Integrated Rate equation in relation to first order reactionMention the two important features of solid catalysts and explain with thehelp of suitable examples.