What is the value of K. expression for the following reaction? Iz(aq) + 5HsIOg(aq) 5710;"(aq) + 9H2O +7H“(aq) In case of first order type "1".
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What is the value of Kc expression for the following reaction?:
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- 5 Br-(aq) + BrO3-(aq) + 6 H+(aq)--> 3 Br2(aq) + 3 H2O(l); (a) write the expressions of the reaction rates mathematically in terms of (i) the disappearance of Br- (Reactant); (ii) the disappearance of BrO3- (Reactant), and (iii) the formation of Br2 (Product). (b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C102(aq) + 2OH(aq) → ClO₂ (aq) + CIO; (aq) + H₂O(!) A kinetic study of this reaction under a certain set of conditions yielded the data below. Exp [CIO₂] (M) [OH-] (M) A[CIO₂]/At (M/s). 0.100 1 5.75 x 10-2 2 0.100 3 0.0500 0.0500 0.100 0.100 0.10 0.25 2.30 x 10-¹ 1.15 x 10-¹ a. What is the rate law? b. What is rate constant, k? c. fill in the missing cell in the table.The elementary steps for a catalyzed reaction are shown below. Identify the catalyst? Identify the reactive intermediate? HyOy(0g) + I" (aq) —+ H_O(0) + IOT (sq) IO"(@a) + HyOz(0g) - HyO0+O2{0) +F(31) O The catalyst is H₂O2(aq); the reactive intermediate is 1(aq). Ob The catalyst is (aq); the reactive intermediate is 10"(aq). The catalyst is H₂O(); the reactive intermediate is 1" (aq). Od The catalyst is 1"(aq); the reactive intermediate is H₂O2(aq). The catalyst is 10(aq); the reactive intermediate is 1(aq).
- First order: [A]o In———- = kt [A]t t1/2= .693/k6. To observe the effect of temperature on reaction rate, the reaction between MnO, ag) and C204(ag) in acidic media is performed according to the given redox reaction: 2 MnO4 (aq) + 16 H*(aq) + 5 C204²(aq) → 10 CO2(g) + 2 Mn²"(aq) + 8 H2O(1) At various temperatures, the rate constants were determined experimentally as follows: k (M s') 5.03x105 T (°C) 20 35 3.68×104 60 6.71×103 90 0.119 (a) Determine Ea for this reaction by a graphical method (see the graph given below). (b) Determine E. using Arrhenius equation using tabulated data. (c) Calculate the value of the rate constant, k at 100°C. -2 -4 兰 -6 -8 -10 -12 0.0025 0.0027 0.0029 0.0031 0.0033 0,0035 1/T (K)2. For the reaction: 3. 5 Br (aq) + BrO3 (aq) + 6 H*(aq)--> 3 Br2(aq) + 3 H2O(1); (a) write the expressions of the reaction rates mathematically in terms of (1) the disappearance of Br" (Reactant); (ii) the disappearance of BrO3" (Reactant), and (iii) the formation of Br2 (Product).
- 8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of NThe Eºcell = 0.135 V for the reaction 31₂(s) + 5Cr₂O7²-(aq) + 34H*(aq) ? 6103¯ (aq) + 10Cr³+ (aq) + 17H₂O What is Ecell if [Cr₂O72] = 0.027 M, [H+] = 0.21 M, [103] = 0.00028 M, and [Cr³+] = 0.0030 M?(a) Explain the meaning of the sentence:“The velocity laws of reactions are empirical” (b) It can be determined that the velocity law of a generic reaction A +B→Pév = k[A]x[B]y. Plot on a graph the variation of [A] and [P] with time, and explain why v= d[P]/dt = -d[A]/dt. (c) Explain the meaning of the terms k, x and y, in the velocity law, presented in item b: (d) Explain what it means in practice for a velocity law to be of zero order. Plot ,A as a function of t, for the zero-order reaction A→Products. (e) Explain what elementary reactions are and how they can be classified.
- Chlorine dioxide, Cl02, is a reddish-yellow gas that is soluble in water. In basic solution it gives Cl03- and CIO2 ions. 2C1O:(aq) + 20н (ад) —> СIО3 (aд) + CIO, (aq) + H;0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Initial Concentration Initial Concentration Initial Rate of Cl02 (mol/L) of OH (mol/L) (mol(L's) Exp. 1 0.21 1.6 x 10-2 0.162 Exp. 2 7.0 x 10-2 1.6 x 10-2 1.80 x 10-2 Exp. 3 7.0 x 10-2 4.8 x 10-2 5.39 х 10-2 a Obtain the rate law. (Use k for the rate constant.) Rate law =Expt. 1 2 3 NH; (aq) + NO; (aq) >Nz (aq) + 2 H2O (l) [NO₂] Rate (at 298 K) 0.020 M/s 0.020 M 0.020 M 0.030 M/s 0.010 M 0.0050 M/s [NH+] 0.010 M 0.015 M 0.010 M Determine the complete rate law (rate law and rate constant) for the reaction. Show all work. What is the initial rate of this reaction if the concentrations in Expt. 2 above are tripled. Show work. What is the rate of H₂O formation in Expt. 1? A 4th trial is conducted at 273 K, using the concentrations from Expt. 1. If the rate was found to be 0.016 M/s, calculate the activation energy of this reaction.Part II. Solve each of the following problems. A. Iodide ion is oxidized to hypoiodite ion, IO", by hypochlorite ion, CIOʻin basic solution. The equation is I (aq) + Cl0" (aq) + OH° → I0' (aq) + Cl (aq) + H20 The following data were obtained for initial rates Expt. [I] (M) [CIO'] (M) [ОН] (М) Rate (mol/L s) 12.2 X 10-2 12.2 X 10 -2 6.1 X 10 -2 3.0 X 102 1 0.010 0.020 0.010 2 0.020 0.010 0.010 3 0.010 0.010 0.020 4 0.010 0.010 0.010 Calculate the order of the reaction with respect to I; with respect to CIO; with respect to OH; and the overall order of reaction. What is the rate constant of the reaction? The reaction is done at 22.0 C. It is determined that the activation energy of the reaction is 62 kJ/ mol. What is the rate constant of the reaction at 27.0 C
