P17B.4 The data below apply to the reaction, (CH,),CBr(aq) + H,0(1) → (CH,),COH(aq) + HBr(aq). Identify the order of the reaction and calculate the rate constant and the molar concentration of (CH,),CBr remaining after 43.8h. t/h 3.15 6.20 10.00 18.30 30.80 [(CH,),CBr]/(10²mol dm³) 10.39 8.96 7.76 6.39 3.53 2.07

P17B.4 The data below apply to the reaction, (CH,),CBr(aq) + H,0(1) → (CH,),COH(aq) + HBr(aq). Identify the order of the reaction and calculate the rate constant and the molar concentration of (CH,),CBr remaining after 43.8h. t/h 3.15 6.20 10.00 18.30 30.80 [(CH,),CBr]/(10²mol dm³) 10.39 8.96 7.76 6.39 3.53 2.07

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 91AE: For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time...

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The progress of the reaction between Iodine ions and potassium iodate(V) can be followed by withstanding samples of the reaction mixture at various times, quenching and then titrating with standard thiosulphate solution. The reaction equation is: I(aq) + IO3(aq) + 6H+(aq) + 4e ➡ I2(aq) + 3H2O(l) In one such experiment the following data were obtained. (see figure below) Determine the order of the reaction with respect to I(aq) and IO3(aq) ions Write the rate expression for the reaction.
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The oxidation of HSO3− by O2 in an aqueous solution is a reaction of importance to the processes of acid rain formation and flue gas desulfurization. R.E. Connick et al. (Inorg. Chem. 34, 4543 (1995)) report that the reaction 2 HSO3−(aq) + O2(g) → 2 SO42−(aq) + 2 H+(aq) follows the rate law v = kr[HSO3−]2[O2]2. Given pH = 5.6 and an O2 molar concentration of 0.24 mmol dm−3 (both presumed constant), an initial HSO3− molar concentration of 50 μmol dm−3, and a rate constant of 3.6 × 106 dm9 mol−3 s−1, what is the initial rate of reaction? How long would it take for HSO3− to reach half its initial concentration?
Given Zn(s)| Zn 2+ (aq) (1M) || Ag+2+ (aq) (1M) | Ag (s) Eocell = 1.562V What will the Ecell be if the [Zn2+] = 0.75M and [Ag+] =0.25 M at 40.00oC (313.15K)? The overall reaction is Zn(s) + 2 Ag+ (aq) --> 2 Ag (s) + Zn 2+ (aq) (Answer has 3 digits after the decimal)
For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.
For an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 1
What is the effect of catalyst on:(i) Gibbs energy (ΔG) and(ii) activation energy of a reaction?
For the reaction NH2SO2OH + H2O → NH4HSO4 In aqueous solution at 80.35oC, the following constants were observed at the indicated ionic strength μ x103 k (L/mol hr) 5.06 1.07 11.21 1.02 15.85 0.976 22.94 0.886 From these data ascertain: a.) the valence of the reacting ions and b.) the rate constant for the primary salt effect.
The Gibbs free energy change at standard state for the reaction A+B+C->D+E is known to equal -20 kJ/mol. What is the activation energy for the forward rate constant for this reaction if the forward rate constant increases by 72% at T=44.6C compared to its value at 25 celsius?
The binding of Mg2+ to glycolate anion, (HO-CH2-COO-) proceeds by thisequilibrium:Mg2+ + HO-CH2-COO- ->Mg2+(HO-CH2-COO-) a) Write the expression for Keq for this reversible reaction. b) If you begin with 5 mM Mg2+ and 0.1 mM HO-CH2-COO-, and with a value of Keq = 103 M-1, calculate the concentrations of Mg2+ , HO-CH2-COO-, and Mg2+(HO-CH2-COO-) at equilibrium.
The rate constant of the reaction H2O2(aq) + I−(aq) + H+(aq) → H2O(l) + HIO(aq) is sensitive to the ionic strength of the aqueous solution in which the reaction occurs. At 25 °C, kr = 12.2 dm6 mol−2 min−1 at an ionic strength of 0.0525. Use the Debye–Hückel limiting law to estimate the rate constant at zero ionic strength.
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