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- Q26 (D) Explain with figure the role of a catalyst on speed of areaction.a plausible mechanism (i) MeCCLi (ii) BRCH 2COME (ii) CH 3CO2HCalculate the activation energy for vacancy formatiın in Aluminuim, given that theequibilirium number of vacancies 500 C is 7.57x1023 m-3. The atomic weigth and density (500C) for aluminium are, respectively, 26.98 g/mol and 2.62 g/cm3.
- (d) The first-order rate constants for the fluorescence and phosphorescence of molecule X are 4.5 × 10" s' and 0.50 s', respectively. Briefly explain the large order of magnitude difference in the rate constant values. (e) Explain how long (in s) it takes for 1.0% of fluorescence and phosphorescence to occur following termination of excitation.Identify the mechanismwrite the mechanism 2.3 NaOH, H₂O & Heat
- E17C.1(b) The equilibrium constant for the binding of a drug molecule to a protein was measured as 200. In a separate experiment, the rate constant for the binding process, which is second order overall, was found to be 1.5 x 10 dm mol s. What is the rate constant for the first-order dissociation of the drug molecule from the protein- drug complex?The activation energy for the isomerization reaction ofCH3NC in Problem 14 is 161 kJ mol-1, and the reactionrate constant at 600 K is 0.41 s-1.(a) Calculate the Arrhenius factor A for this reaction.(b) Calculate the rate constant for this reaction at 1000 K.The mechanism for the reaction described by nust. A common d(a stronger whch ont of ice prhct NO,(g) + CO(g) → CO,(g) + NO(g) coor on be c is suggested to be (1) 2NO,(g) –→ NO,(g) + NO(g) k1 -> k2 (2) NO,(g) + CO(g) → NO,(g) + CO,(g) d[CO2] k[NO2]? %3D The experimental rate law for the production of [CO2] = k1 [NO2J² or dt d[NO3] 0 ), is this a valid mechanism? i.e show Assuming that [NO3] is governed by a steady state ( dt that using elementary reactions 1 and 2, the experimental rate law can found. (Hint write out all the ways d[NO3] = ? d[C02] = ? ) %3| and %3D dt that [NO3] and [CO2] are created and destroyed, dt owing clecre cel at 25 C NiC C)Cu a062 0.62 V 0.00 V 4. 460 V
- (f) The following data were recorded for the bimolecular reaction of CIO free radicals as a function of temperature: TIK 298 312.5 323 k/ 10-15 cm3 molec-1 s-1 11.30 11.80 12.10 Determine the Arrhenius parameters A and Ea for this reaction.(Q3)(b) How is Langmuir adsorption isotherm different from Gibb's adsorption isotherm? (O2) Ca) WhThe degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.