The rate constant of the hydrolysis of ethyl acetate (conc = 0.08 M) by sodium hydroxide(conc = 0.08 M) was determined by monitoring the conductance of the solution overtime. Determine the rate constant and briefly discuss how you were able to solve for it.t (s)L (uS)160101402012030108409850927085100801506518065

The progress of the reaction of hydrolysis of ethyl acetate by sodium hydroxide can be monitored…

Answered: The rate constant of the hydrolysis of…

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.38E: List at least four experimentally determined parameters that you, an experimenter, can define when...

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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.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.
The rate constants for the first order decomposition of an organic compound in solution are measured at several temperatures: k (s-¹) 0.00492 0.0216 0.0950 0.326 1.15 288 298 308 318 T (K) 278 Perform linear regression using the given data and fill in the information being asked for. Slope of the line: y-intercept of the line: r² value of regression: Activation energy of the reaction (with units, rounded off to two decimal places): Arrhenius constant of the reaction (with units, rounded off to two decimal places):
A typical diffusion constant for small molecules in aqueous solution at 25 °C is 6 × 10−9 m2 s−1. If the critical reaction distance is 0.5 nm, what value is expected for the second-order rate constant for a diffusion-controlled reaction?
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant H,(g) + 2 NO(g) → N20(g) + H,O(g) k1 1 2 H,(g) + N,0(g) → N2(9) + H2O(g) k2 Suppose also k,»k,. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k || Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k.2 for k the reverse of the two elementary reactions in the mechanism.
1) The rate constant for the gas-phase reaction H2(g) + I2(g) → 2 HI(g) has the value 4.45 x 10-5 mol-1 dm³ s-1. What is the equivalent rate constant in units of molecule-1 cm³ s- 1? 2) The kinetics of the hydrolysis of methyl methanoate, CH3COOCH3, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction (must provide best fit graph). 3600 time, t/s 1800 5400 7200 9000 concentration, c/ (mol dm-3) 0.300 0.191 0.135 0.081 0.055 0.035
Suppose that the typical diffusion coefficient for a reactant in aqueous solution at 25 °C is 5.2 × 10−9 m2 s−1. If the critical reaction distance is 0.4 nm, what value is expected for the second-order rate constant for the diffusion-controlled reaction?
Writing the rate law implied by a simple mechanism Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant 1 (CH,),CBr(aq) → (CH3),C"(aq) + Br (aq) 2 (CH3),C"(aq) + OH (aq) → (CH3),COH(aq) kz Suppose also k,»k,. That is, the first step is much faster than the second. olo Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k I Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k.2 for k = the reverse of the two elementary reactions in the mechanism. olo ||
The reaction between fluorine and chlorine dioxide, F2(g) + ClO2(g) → 2FClO2(g) Proceeds according to the following rate Law: r=k⋅PF2⋅PClO2 where k= 0.0489 bar-1 s-1. In an isolation experiment, the initial partial pressures are: PF2(t=0) = 0.04687 bar and PClO2(t=0) = 3.606 bar. Note: Ukeff means units of keff . You need to use a string with no spaces. For example enter gm3 as g*m^{-3} or g/m^3 . (a) Calculate the effective rate constant keff= Ukeff= (b) Compute the pressure of fluorine in bar after 55.8 s. PF2(t=55.8s)= bar (c) How long will it take for the pressure of fluorine to drop to 0.01318 bar? t = s
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N20(g) + H,O(g) k1 2 H2(g) + N,0(g) → N,(g) + H,O(g) k2 Suppose also k,«k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k, k2, and (if necessary) the rate constants k.1 and k.2 for the reverse of the tae k =
The decomposition of urea in 0.1 M of HCl occurs according to the reaction NH,CONH, +2H,0→2NH;+CO; The first-order rate constant for this reaction was measured as a function of temperature, with the following results Expt. T /°C kx 106 / min-1 1 61.0 7.13 71.2 27.7 Calculate the entropy of activation at 71.2 °C for the reaction of decomposition of urea. Make the assumptions you need.
Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A + B → P and the reactants are initially present in (a) their stoichiometric proportions ([B]0 = 12[A]0); (b) with B present initially in twice that amount ([B]0 = [A]0). Express your rate law in terms of [A]0, [B]0, and x, where [A] = [A]0 − 2x.

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The rate constant of the hydrolysis of ethyl acetate (conc = 0.08 M) by sodium hydroxide (conc = 0.08 M) was determined by monitoring the conductance of the solution over time. Determine the rate constant and briefly discuss how you were able to solve for it.