A sólution of g/L acrylamide in than is polymerized at /L isobutyryi peroxide (initiator) whose half life is 9.0 h at this temperature and efficiency in methanol is 0.3. For acrylamide, k,²/k= 22 L mol· s·l at 25°C and termination is by coupling alone. (a) What is the initial steady state rate of polymerization ? (b) Find the percentage conversion of monomers in the first 10 min of reaction in 1L of solution? Acrylamide H H C=C C-NH2 Hi Hint : Find the initial concentration of monomer in mol/L [M] =(100 g/L)/(Molecular weight of acrylamide) Given the half-life time of the initiator used. Find dissociation rate constant of the initiator. In(2). Half-life t/2= 1/2 fks R, = k, k, ka 0.693/K. %3D [M] 1/2 - In = 2 [M], ka

A sólution of g/L acrylamide in than is polymerized at /L isobutyryi peroxide (initiator) whose half life is 9.0 h at this temperature and efficiency in methanol is 0.3. For acrylamide, k,²/k= 22 L mol· s·l at 25°C and termination is by coupling alone. (a) What is the initial steady state rate of polymerization ? (b) Find the percentage conversion of monomers in the first 10 min of reaction in 1L of solution? Acrylamide H H C=C C-NH2 Hi Hint : Find the initial concentration of monomer in mol/L [M] =(100 g/L)/(Molecular weight of acrylamide) Given the half-life time of the initiator used. Find dissociation rate constant of the initiator. In(2). Half-life t/2= 1/2 fks R, = k, k, ka 0.693/K. %3D [M] 1/2 - In = 2 [M], ka

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

Give detailed Solution .. don't give Handwritten answer....show work
The sucrose hydrolysis reaction is pseudo-first order, which means that...(1). The rate constant is practically 1.(2). The rate of transformation of sucrose into glucose and fructose is practically constant over time.(3). the concentrations of the products (glucose and fructose) will be approximately equal to 1 at the end of the reaction.(4). The plot of the logarithm of sucrose concentration versus time should be approximately a straight line.
The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: As033- + 2 Ce4+ + H20→AS043- + 2 Ce3+ + 2 H+ Experiment [As033-]o, M [Ce4+]o, M Initial Rate, M s1 2.86x10-2 4.52x10-3 1 0.545 2 5.72x10-2 0.545 9.04x10-3 2.86x10 2 1.81x10-2 3 1.09 5.72x10-2 3.62x10-2 4 1.09 Complete the rate law for this reaction in the box below. Use the form k[A]™[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-25-1.
only solve 16.16 using information in ques 16.15
:(:(/)/)/$$;&&(&;&:$:$;$;$;;
Question No., 4: The homogeneous dimerization of butadiene: 2C,Hs(g) = C8H12(g), has been studied by a number of investigators and found to have an experimental activation energy of 23960 cal/ mol, as indicated by the following equation: k = 9.2 x 10°e-23960/RT cm³mol-'s-1 a. What proportion of the collisions between C4H6 molecules have enough energy to result in reaction when the temperature is 200°C? b. Use the collision theory to predict a value of the pre-exponential factor (in SI units) at 600 K. Assume that the collision diameter is 5 x 10-°cm. c. By how many times the calculated value of the pre-exponential factor is greater than the experimental value? Suggest a reason for this discrepancy.
Give detailed Solution with explanation *no need Handwritten
The activation energy for the gas phase decomposition of t-butyl bromide is 170 kJ.(CH3)3CBr(CH3)2C=CH2 + HBrThe rate constant at 523 K is 0.000209 /s. The rate constant will be ?????? /s at 565 K.
Give handwritten answer
Give detailed Solution with explanation needed..please give correct answer
In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °CNH4NCO(aq)(NH2)2CO(aq)the following data were obtained: [NH4NCO], M 0.780 0.390 0.195 9.75×10-2 minutes 0 131 393 918 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 0.780 M is______ min and when the starting concentration is 0.390 M is ______min.(2)The average (1/[NH4NCO]) / t from t = 0 min to t = 131 min is______ M-1 min-1.The average (1/[NH4NCO]) / t from t = 131 min to t = 393 min is_____ M-1 min-1.(3)Based on these data, the rate constant for this _______ (zerofirstsecond) order reaction is M-1 min-1. fill in the blanks