In the hydrolysis (saponification) of ethylacetate, a plot of In(k,-k) against time isa straight line. The conductivity of thereaction mixture was 1438 μS cm after 10min and 1030 μS cm after 40 min ofmixing reaction components. If K∞ = 653US cm, calculate the reaction rateconstant in s.Select one:1.1 × 10251x4.1 × 10-4 s18.1 x 10-5 512.5 × 10-3 s-1

To determine the reaction rate constant k for the hydrolysis of ethyl acetate, we need to use the…

Answered: In the hydrolysis (saponification) of…

Human Anatomy & Physiology (11th Edition)

11th Edition

ISBN:9780134580999

Author:Elaine N. Marieb, Katja N. Hoehn

Publisher:Elaine N. Marieb, Katja N. Hoehn

Chapter1: The Human Body: An Orientation

Section: Chapter Questions

Problem 1RQ: The correct sequence of levels forming the structural hierarchy is A. (a) organ, organ system,...

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What are the benefits of measuring the initial rate of a reaction Vå for use in kinetic studies? (This is a multi-select question). [ES] can be measured accurately. changes in [S] are negligible, so the value of [S] is known. changes in Km are negligible, so Km can be treated as a constant. V₁ = Vmax. --> A negligible amount of product has formed, so that the back reaction P -- need not be considered. ES
Direct methanol fuel cells (DMFCS) have shown some promise as a viable option for providing "green" energy to small electrical devices. Calculate E° for the reaction that takes place in DMFCS: CH3OH(I) + 3/2 02(g) → CO2(g) + 2 H20(1) Use the following values. AG°H,0(1) = -237 kJ/mol AG°O2(g) = 0 kJ/mol AG°CO2(9) = -394 kJ/mol AG°CH3OH(I) = -166 kJ/mol. E° = V
The following values were taken from the Richard's table on the thermal death kinetics of B. stearothermophi. cal/mol K): (A=4.9x1037min', E=67.48 kcal/mol, R=1.987 Temperature, °C rate The cumulative del factor Specific constant k, min death -1 V 120 1.47 7.25 121 1.83 9.08 125 4.35 22.08 130 12.55 65.10 (i) The time taken for heating, cooling and holding periods in the sterilisation of a batch fermentor medium for the destruction of B. stearothermophilus were: time to heat from 100 to 121°C = 30 min time to cool from 121 to 100 °C =16 min time of holding at 121 °C = 12 min Calculate the destruction ratio (No/N) for the process. (ii) If the sterilisation were to be carried out continuously at 130 °C, and the heating and cooling characteristics were: time to heat from 100 to 130 °C = 2 min time to cool from 130 to 100 °C = 1 min what holding time would be required to achieve the same ratio of (No/N) as in section (i) above? State all the assumptions made in your calculations.
The value of AH° for HBr(g) was first evaluated using the following standard enthalpy values obtained experimentally. Use these data to calculate the value of AHf° for HBr(g). Cl,(g)+2KB1(ag) – Br, (ag)+2KCI(ag) AH° =-96.2 kJ H,(g)+Cl, (g)- HCl(aq)+ KOH(aq) KC(aq)+H,O(!) 2HCI(g) AH° =-184 kJ AH° =-57.3 kJ HBr(aq)+ KOH(aq) KBr(aq)+ H,O(!) AH° =-57.3 kJ AH° =-77.0 kJ HC(g) Br,(g) HBr(g)- HCl(aq) disdlving in water Br, (aq) AH° =-4.2 kJ disolving in water HBr(aq) AH° =-79.9 kJ dissolving in water ΔΗΡ- i kJ
What is the likely keq for an enzyme that has a deltaG =-18.3kj/mol?
Consider the following reaction: Glucose 6-phosphate + Glucose 1-phosphate After reactant and product were mixed and allowed to reach equilibrium at 25C, the concentration of each compound was measured: (Glucose 1-phosphate] - 0.002 M [Glucose 6-phosphate 0.05 mM Calculate the Keg and the AG knot prime (e.g. standard free energy change). O Keg- 40: AG knot prime 9.14 kJ/mol O Ken- 19: AG knot prime -7.3 kJ/mol O Keg" 0.04: AG knot prime-7.98 kJ/mol Kea 4: AG knot prime -914 kJ/mol O Keg 40: AG knot prime - 9.14 k/mol
If glucose, phosphate, and glucose-6-phosphate arecombined in concentrations of 4.8, 4.8, and 0.25 mM,respectively, what is the equilibrium constant for thehydrolysis of glucose-6-phosphate at a temprature of258C?
From a kinetics experiment, Kcat was determined to be 55sec^-1. For the kinetic assay, 0.05mL of a 0.05mg/mL solution of enzyme was used, and the enzyme has a molecular weight of 30,000g/mole. Assume a reaction volume of 3mL. Calculate Vmax (um*min^-1) for the enzyme and catalytic efficiency (in M^-1sec^-1) for the enzyme. The Km for the enzyme was determined to be 8.3*10^-2M.
A particular reaction has ΔH°' = 1 kJ mol-1 and ΔS°' = -104 J mol-1 K-1. Calculate the value of ΔG°' in kJ mol-1 at 25.0 °C.
A biochemist is trying to determine the type of proteases they have isolated from walrus blubber. The three proteases and their relative activities in the presence of the indicated non-specific irreversible inhibitors are shown in the table below: Protease a Protease B Protease y Given this data, please answer the following question: The catalytic site of Protease ß contains an important: C R H + lodoacetate Normal Activity Normal Activity No Activity U + Tetranitromethane Normal Activity No Activity Normal Activity
The Ksp values of silver chromate Ag2CrO4 and silver iodate Ag(IO3) are given below. Ag2CrO4 Ag(IO3) Ksp 1.12 x 10-12 3.17 x 10-8 Based on these Ksp values, which of the following is true? Choose one option only. Options: a. In the solution consisting of 1.00 x10-4 M Ag+ and 5.00 x10-5 M CrO42-, Ag2CrO4 precipitate will form. b. In the solution consisting of 1.0 x10-4 M Ag+ and 1.0 x10-4 M IO3-, Ag(IO3) precipitate will form. c. In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3). d. In the solution consisting of 0.200 M CrO42- and 0.200 M IO3-, Ag2(CrO4) will precipitate first if we add Ag+ ions gradually into the above mixture.
Benzene, C6H6, is an aromatic hydrocarbon that exists as a liquid at 298 K and 1 bar. The solubility of benzene in water, defined as the concentration of the saturated solution, is 2.23×10¬3 M at 298 K and 1 bar, and its standard Gibbs free energy of formation is AfG° (C6H6, ) = 124.3 kJ/mol. a. Calculate the standard Gibbs free energy change for the process of dissolution of benzene in water a. Find the chemical potential of the benzene solute standard state AFG° (C6H6, aq).

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