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![2 (CN 33etermination of Reaction Order
Example 2: The decomposition of acetaldehyde at 600°C:
CH,CHO > CH, + Co
Determine rate law expression and rate constant based on the
data given below.
[CH,CHO), M
0.10
0.20
0.30
0.40
Initial rate, M/s
0.085
0.34
0.76
1.4
rate = k[CH,CHO]2
k= 8.5 Ms
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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.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 first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.
- For the gas phase decomposition of t-butyl propionate,C2H5COOC(CH3)3(CH3)2C=CH2 + C2H5COOHthe rate constant at 534 K is 5.82×10-4 /s and the rate constant at 583 K is 1.30×10-2 /s.The activation energy for the gas phase decomposition of t-butyl propionate is _____ kJ.Two prominent gas-phase atmospheric reactions are written below with rate coefficients in units of cm3 molecule-1 sec-1 (T= temperature in K and [M] = the number density of air in molecules cm-3). Convert theserate constants to ppm-1 min-1, again assuming standard sea-level pressure and T = 288 K.i. O + O2 =O3 k = [M]*6.0*10^-34*(T/300)^-2.3ii. NO + O3 = NO2 + O2 k = 3.0*10^-12*e^(-1500/T)Conventional equilibrium considerations do not apply when a reaction is driven by light absorption and the steady-state concentration of products and reactants might differ significantly from equilibrium values. For instance, suppose the reaction A → B is driven by light absorption, and that its rate is Ia, but that the reverse reaction B → A is bimolecular and second order with a rate kr[B]2. What is the stationary state concentration of B? Why does this ‘photostationary state’ differ from the equilibrium state?
- 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?1. The following initial rate data are for the ozonization of pentene in carbon tetrachloride solution at 25 oC:C5H10 + O3 C5H10O3 Experiment [C5H10]o, M [O3]o, M Initial Rate, Ms-1 1 6.32×10-2 1.34×10-2 76.0 2 6.32×10-2 2.68×10-2 152 3 0.126 1.34×10-2 151 4 0.126 2.68×10-2 303 Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is ________ M-1s-1.The conversion of dissolved carbon dioxide in blood to HCO3- and H3O+ is catalyzed by the enzyme carbonic anhydrase. The Michaelis–Menten constants for this enzyme and substrate are Km = 8 × 10-5 mol L-1 andk2=6 × 105 s-1. (a) What is the maximum rate of reaction of carbon dioxide if the enzyme concentration is 5 × 10-6 M?(b) At what CO2 concentration will the rate of decomposition be 30% of that calculated in part (a)?
- 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 a temperature-jump experiment to investigate the kinetics of an isomerization reaction that is first-order in both directions, the relaxation t ime was measured as 27.6 μS. The rate constant for the forward reaction is known to be 12.4 ms-1. Ca lcu late the rate constant for the reverse reaction.The composition of a liquid phase reaction 2A → B was monitored by aspectrophotometric method with the following results: t, s [B], mol/L 0 0 600 0.089 1200 0.153 1800 0.200 2400 0.230 ∞ 0.312 Identify the rate law, integrated rate law, and rate constant for thereaction based on the obtained data.
