For the gas phase decomposition of trichloromethyl chloroformate,CICOOCCI32 COCI2the rate constant has been determined at several temperatures. When In k in s is plotted against the reciprocal of the Kelvintemperature, the resulting linear plot has a slope of -2.09×104 K and a y-intercept of 30.3.The activation energy for the gas phase decomposition of trichloromethyl chloroformate iskJ/mol.

Arrhenius equation is k=A.exp{-EaR.T}Wherek = rate constant Ea=Activation energyR = gas constant =…

Answered: For the gas phase decomposition of…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter8: Sampling, Standardization, And Calibration

Section: Chapter Questions

Problem 8.19QAP

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
The decomposition of NH3 to N2 and H2 was studied on two surfaces: Surface Ea (kJ/mol) W 163 Os 197 Without a catalyst, the activation energy is 335 kJ/mol. a. Which surface is the better heterogeneous catalyst for the decomposition of NH3? Why? b. How many times faster is the reaction at 298 K on the W surface compared with the reaction with no catalyst present? Assume that the frequency factor A is the same for each reaction. c. The decomposition reaction on the two surfaces obeys a rate law of the form Rate=k[NH3][H2] How can you explain the inverse dependence of the rate on the H2 concentration?
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at various temperatures. Plot the natural logarithm of k versus l/T and from the graph obtain the energy of activation. Temperature (oC) k (L/mol s) 320 0.527 330 0.776 340 1.121 350 1.607
Consider the first-order decomposition of phosgene at a certain temperature. COCl2(g)productsIt is found that the concentration of phosgene is 0.0450 M after 300 seconds and 0.0200 M after 500 seconds. Calculate the following: (a) the rate constant at the temperature of the decomposition (b) the half-life of the decomposition (c) the intial concentration of phosgene
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.

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