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- The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
- 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.(b) The reaction between H2O2 and lodide; H,0, + 21 + 2H*→ 2H,0 + 12 Proceeds by two parallel mechanism and led to a rate laws, k, [H,0][I] and = k, [H,0][][#*] %3D dt dt The change in observed rate constants with ionic strength for both the mechanisms is given in the following table. k (M's) 0.69 k2 (M's') Sr. no. Ionic strength (1) 19.0 0.00 0.0207 0.66 15.0 3 0.0525 0.67 12.0 4 0.0925 0.68 11.3 0.69 0.1575 0.2025 9.7 0.71 9.2 With the help of this data and corresponding plots, comment on which mechanism between these two would follow Primary salt effect more prominently. rhich tyne of complex mechanism T-jumpThe following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.
- (1) The gas phase decomposition of dinitrogen pentoxide at 335 KN2O5(g)2 NO2(g) + ½ O2(g)is first order in N2O5 with a rate constant of 4.70×10-3 s-1.If the initial concentration of N2O5 is 3.97×10-2 M, the concentration of N2O5 will be 8.22×10-3 M after ______s have passed. (1b) The gas phase decomposition of sulfuryl chloride at 600 K SO2Cl2(g) SO2(g) + Cl2(g) is first order in SO2Cl2 with a rate constant of 2.80×10-3 min-1. If the initial concentration of SO2Cl2 is 4.90×10-3 M, the concentration of SO2Cl2 will be M after ______ 499 min have passed.In a study of the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C HzOz(aq)+HzO(l) + % Oz(E) the concentration of H₂O₂ was followed as a function of time. It was found that a graph of In[H₂O₂] versus time in minutes gave a straight line with a slope of -1.51×10-3 min-1 and a y-intercept of -3.47. min-1. Based on this plot, the reaction is ✓order in H₂O₂ and the rate constant for the reaction isIn a study of the decomposition of nitramide in aqueous solution at 25 °C NH,NO2(aq)N20(g) + H20(1) the concentration of NH2NO2 was followed as a function of time. It was found that a graph of In[NH,NO2] versus time in seconds gave a straight line with a slope of -7.00x10-5 5-1 and a y-intercept of -1.84. Based on this plot, the reaction is reaction is order in NH,NO2 and the rate constant for the
- The reaction of ethyl acetate with sodium hydroxide, CH3 COOC,H; (aq) + NaOH(aq) = CH3COONA(aq) + C2H; OH(aq) is first order in CH3 COOC,H; and first order in NaOH. If the concentration of CH3 COOC2H; was increased by half and the concentration of NaOH was increased by four, by what factor would the reaction rate increase? Express your answer numerically.The reaction (CH3)3CBr + OH- -> (CH3)3COH + Br- in a certain solvent is first order with respect to (CH3)CBr and zero roder with respect to OH-. In several experiemnts, the rate constant was determined at different temepratures. A plot of ln(k) vs. 1/T was constructed resulting in a straight line with a slope of -1.10x104 K and a y-intercept of 33.5 a. determine the activation energy b. determine the frequceny factor and rate constant at 25.0C c. determine the rate constant when the temperature drops to 15.0CThe rate constant for the fi rst-order decomposition of N2O5 in the reaction 2 N2 O5(g) → 4 NO2(g) + O2(g) with v = kr[N2O5] is kr = 3.38 x 10-5 s-1 at 25 oC. What is the ha lf- life of N2O5? What w ill be the total pressure, init ial ly 78.4 kPa for the pure N2O5 vapour, (a) 5.0 s, (b) 5.0 min after init iation of the reaction?