The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows.C12H22011 + H20 → C;H1206 + CgH1206This reaction follows a first-order rate equation for the disappearance of sucrose: rate =k [C,,H,,0,1] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are22isomers.)1.8x10-11Arrhenius equation at this temperature). (Enter unrounded values.)(a) In neutral solution, kat 26°C and 8.5x10-11-1at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s), and the rate constant (in s) for this equation at 48°C (assuming the kinetics remain consistent with theactivation energy108kJ/molfrequency factorrate constantX s-1(b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10 M. How long (in s) will it take the solution to reach equilibrium at 26°C in the absence of a catalyst? Because the concentration ofsucrose at equilibrium is so low, assume that the reaction is irreversible. (Enter an unrounded value.)

Answered: Image /qna-images/answer/a73756cf-bb30-4028-a89f-92c286ea4e6e.jpg

The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H,0 - C,H120, + C,H1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate - k [C,,H2,0,1 (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, I.e. they are Isomers.) (a) In neutral solution, k- 1.8 x 10"1 s at 26°C and 8.5 x10-" s- at 37°C. Determine the activation energy (in k)/mol), the frequency factor (in s"), and the rate constant (In s) for this equation Arrhenlus equation at this temperature). (Enter unrounded values.) 48°C (assuming the kinetics remain consistent with the activation energy 108 v k)/mol frequency factor s-1 rate constant x s1 (b) When a solution of sucrose with an Initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10- M. How long (In s) will it take the solution to reach equilibrlum at 26°C in the absence of a catalyst? Because the concentration of sucrose at equilbrium is so low, assume that the reaction is Irreversible. (Enter an unrounded value.)

The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H,0 - C,H120, + C,H1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate - k [C,,H2,0,1 (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, I.e. they are Isomers.) (a) In neutral solution, k- 1.8 x 10"1 s at 26°C and 8.5 x10-" s- at 37°C. Determine the activation energy (in k)/mol), the frequency factor (in s"), and the rate constant (In s) for this equation Arrhenlus equation at this temperature). (Enter unrounded values.) 48°C (assuming the kinetics remain consistent with the activation energy 108 v k)/mol frequency factor s-1 rate constant x s1 (b) When a solution of sucrose with an Initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10- M. How long (In s) will it take the solution to reach equilibrlum at 26°C in the absence of a catalyst? Because the concentration of sucrose at equilbrium is so low, assume that the reaction is Irreversible. (Enter an unrounded value.)

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine Ea and A, the activation energy and pre-exponential factor. What is the value of the rate constant at 100(⁰C)?
CO(g) + Cl2(g) COCl2(g) The above reaction obeys the mechanism: Cl2 2Cl Fast equilibrium Cl + CO COCl Fast equilibrium COCl + Cl2 COCl2 + Cl Slow 2Cl Cl2 Fast Consider each of the following expressions and select "Yes" or "No" to indicate which represent a correct statement of the rate law that is consistent with the given mechanism. d[COCl2]/dt = k[Cl2]3[CO] d[COCl2]/dt = k[Cl2]3/2[CO] -d[CO]/dt = k[CO][Cl2]3/2 -d[Cl2]/dt = k[Cl]2 d[COCl2]/dt = k[CO][Cl2] d[COCl2]/dt = k[CO][Cl2]1/2
What is meant by the term elementary reaction? What is the difference between a unimolecular and a biomolecular elementary reaction? What is a reaction mechanism? What is meant by the term rate determining step?
Two molecules of 1,3-butadiene (C4H6) form 1,5-cyclooctadiene, C8H12 at higher temperatures.2 C4H6(g) → C8H12(g) Use the following data to determine the order of the reaction the rate constant, k. (Note that the total pressure is the pressure of the unreacted C4H6 at any time and the pressure of the C8H12.) Time (min) Total Pressure (mmHg) 0 436 3.5 428 11.5 413 18.3 401 25.0 391 32.0 382 41.2 371
Rate constants for the decomposition of gaseous dinitrogen pentoxide are 3.7×10−53.7×10−5 s−1s−1 at 25 ∘C∘C and 1.7×10−31.7×10−3 s−1s−1 at 55 ∘C∘C.2N2O5(g)→4NO2(g)+O2(g What is the activation energy for this reaction in kJ/molkJ/mol? What is the rate constant at 35 ∘C∘C?
The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
A proposed mechanism for the decomposition of hydrogen peroxide consists of three elementary steps: (1) H₂O2(g) →>> 2OH(g) (2) H₂O2(g) + OH(g) → H₂O(g) + HO₂(g) (3) HO₂(g) + OH(g) → H₂O(g) + O₂(g) If the rate law for the reaction is first order in H₂O2, which step in the mechanism is the rate-determining step? O Step 1 O None of the steps O Step 3 O Impossible to determine Steps 1 and 2 O All of the steps O Step 2 Hint: The slowest step in a mechanism determines the rate law. From each elementary reaction we can write a rate-law expression. Submit Question
Nitrification is a biological process for removing NH3 from wastewater as NH4+: NH, +20, → NO3 + 2H + H2O The first-order rate constant is given as k₁ = 0.47e0.095(T-15°C) where k₁ is in day¹ and T is in °C. If the initial concentration of NH3 is 3.0 mol/m³, how long will it take to reduce the concentration to 0.66 mol/m³: (a) in the spring (T = 20°C)? days (b) in the winter (T = 10°C)? days
Gaseous SO2Cl2 undergoes the following decomposition: SO2Cl2 (g) --> SO2(g) +Cl2(g) The above reaction has a second-order kinetic dependence on the SO2Cl2 concentration with a rate constant of (0.00400 M-1* s-1). If one starts with 0.0641 molar SO2Cl2 at time zero, what is the calculated molar concentration of SO2Cl2 remaining after 40.23 minutes of decomposition of the initial SO2Cl2
The conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °C CH3NC(g)CH3CN(g) is first order in CH3NC with a rate constant of 3.00x103 s1. If the initial concentration of CH3NC is 3.45×10-2 M, the concentration of CH3NC will be 4.11x10-3 M after have passed.
The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1
The gas phase decomposition of hydrogen peroxide at 400 °C H,O2(gH,0(g) +¾ O2(g) is second order in H2O2 with a rate constant of 0.650 M- s-1 If the initial concentration of H,O, is 0.218 M, the concentration of H,0, will be |Mafter 58.3 seconds have passed.