35. be deduced from the rate equation of the reaction, CH;COCH, + I2 → CH;COCH21 + H* +F given by rate = K[CH;COCH3][H*], that the reaction is 1 Second order 2 Zero order with respect to Iz. 3 Unimolecular ABCD
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- Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.Given the 1st order rxn A(g) --- > B(g) + C(g) + 3D(g) with a rate constant of 6.0x10-4 s-1 at 298 K. With a starting mol of 1.00 mol of A(g), how long in seconds does it decrease to 0.500 mol?2A + B -> products, rate = k[A]-1 what is the derived expression for half-life with respect to A in terms of ? and [A]o?
- For a certain alkane the activation energies for the rate determining step of fluorination and chlorination are 8.0 kJ/mole and 20 kJ/mole, respectively. Calculate the ratio of the rate of fluorination to that of chlorination at 27oC assuming that the values of A (Arrhenius constant) are the same. (R=8.314 J/mol-K)The rate of a first-order reaction is followed by spectroscopy,monitoring the absorbance of a colored reactant at 520 nm.The reaction occurs in a 1.00-cm sample cell, and the onlycolored species in the reaction has an extinction coefficientof 5.60 x 103 M-1 cm-1 at 520 nm. (a) Calculate the initialconcentration of the colored reactant if the absorbance is0.605 at the beginning of the reaction. (b) The absorbancefalls to 0.250 at 30.0 min. Calculate the rate constant inunits of s - 1. (c) Calculate the half-life of the reaction.(d) How long does it take for the absorbance to fall to 0.100?The second-order rate constants for the reaction of oxygen atoms ·with aromatic hydrocarbons have been measured (R. Atkinson and J.N . Pitts, J. Phys. Chem. 79, 295 (1975)). In the reaction with benzene the rate constants are 1.44x 107dm' mor ' s ' at 300.3 K, 3.03 x 107 dm' mol"'s"' at 34 1.2K, and 6.9 x 107 dm' mor's ' at 392.2K. Find the frequency factor and activation energy of the reaction.
- In the experiment, below gas-phase homogenous oxidation, k 2 NO + O2 -------> 2NO2 was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is known that any elementary reaction must have a positive energy. Provide an explanation, starting from the fact that an active intermediate species, NO3, is a participant in some other know reactions that involve oxides of nitrogen. Other active intermediates could be NO* and O2* and O* (oxygen atom). Using chemical reactions, or reaction pathway, to describe the mechanism, and using your own reactions suggest how to postulate the formation rate of NO2.The 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?The ha lf-l ife of pyruvic acid in the presence of an aminotransferaseenzyme (which converts it to alanine) was found to be 221 s. How long will it take for the concentration of pyruvic acid to fal l to 1/ 64 of its in it ial va lue in th is first-order reaction?
- 2A + B --> 3C + 2D The rate of formation of C in the above reaction is measured at 2.2 mol dm-3 s-1. What are the rates of formation and consumption of D, A, and B? Ans: 1.5 mol dm-3 s-1, 1.5 mol dm-3 s-1, and 0.73 mol dm-3 s-1 respectively.The activation energy for the gas phase isomerization of cyclobutene is 136 kJ.(CH2)2(CH)2CH2=CHCH=CH2The rate constant at 429 K is 3.24×10-4 /s. The rate constant will be /s at 469 K.At 147oC, the initial rate of the gas-phase decomposition of 1,1-dimethyl peroxide (DMP) depends on the initial concentration of DMP: [DMP], mol dm-3 0.0200 0.0625 0.1720 0.520 Rate (-d[DMP]/dt), mol dm-3 s-1 2.0 x 10-6 8.75 x10-6 2.40 x10-5 7.2 x10-5 From the data, establish that the reaction is first order, and calculate the rate constant at 147oC. [138421] The answer is in the bracket, thank you!