2. Derive an expression for the time dependence of the degree of polymerization for the stepwise polymerization of a hydroxyacid HO – R – COOH for which the rate law is 414 = -k,[A]²[OH] ,where A denotes the carboxylic acid group. dt
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- Derive an expression for the time dependence of the degree of polymerization for the stepwise polymerization of a hydroxyacid HO−R−COOH for which the rate law is d[A]/dt = −kr[A]2[OH], where A denotes the carboxylic acid group.Give clear handwritten answer- Derive an expression for the time dependence of the degree of polymerization (the average number of monomer residues per polymer molecule) for a condensation polymerization in which the reaction is known to have rate law d[M]/dt = -k[M] 3 , where [M] represents the concentration of the monomer!A particular reactant molecule "R" is capable of undergoing condensation and forming either a single closed loop (R-> L) or long chain polymer (R+R+R ->P). The rate law for the loop forming reaction is rate(loop) = kLoop[R]; the rate lw for the polymerization reaction is rate(poly) = kpoly[R]^2 a) a beaker with a starting concentration of R equals 0.50M at 60degrees. After 75 minutes of reacting, the concentration of L is 0.10M. Assuming no change in volume or temperature, find k(loop) b. At the 75 minute mark the remaing concentration of R is 0.398M. What can you conclude (qualitatively) about the magnitude of k(poly) relative to k(loop)?
- The rate law for the reaction of phenolphthalein with NaOH was determined to be Rate = k[P2−][OH−]. What are the units on the value of the rate constant, k?The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figuresFor the rate law Rate = k[A]2.5[B]2, the partial order with respect to A is ________, the partial order with respect to B is ________, and the total order is ________.
- In the experiment, below gas-phase homogenous oxidation, k 2 NO + O2 -------> 2NO2 was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is known that any elementary reaction must have a positive energy. Provide an explanation, starting from the fact that an active intermediate species, NO3, is a participant in some other know reactions that involve oxides of nitrogen. Other active intermediates could be NO* and O2* and O* (oxygen atom). Using chemical reactions, or reaction pathway, to describe the mechanism, and using your own reactions suggest how to postulate the formation rate of NO2.Calculate the magnitude of the diffusion-controlled rate constant at 320 K for the recombination of two atoms in benzene, for which η = 0.601 cP. Assuming the concentration of the reacting species is 2.0 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.Calculate the magnitude of the diffusion-controlled rate constant at 320 K for the recombination of two atoms in water, for which η = 0.89 cP. Assuming the concentration of the reacting species is 1.5 mmol dm−3 initially, how long does it take for the concentration of the atoms to fall to half that value? Assume the reaction is elementary.
- The 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.Using the given data in Expt 1, find the rate constant value (with its corresponding units). See table for the given.The rate law for the reaction between catalase and hydrogen peroxide can be written as Speed = k [ H 2 O 2 ] x [ catalase ] there . A catalase solution of unknown but constant concentration was prepared. a.Is it possible to find the partial order with respect to peroxide? b. If so, how will you find it? Describe the steps in detail or show a calculation.