Serine (C3H703N) can be oxidized to carbon dioxide and ammonia in the presence of oxygen. The balancedoverall reaction is provided below. <2C3H703N+502 = 6C02 + 4H₂O + 2NH3<Assuming that the theoretical C-BOD is equal to the BODU (BODL or Lo) and given a first-order rate constant of0.16 what is the BOD5 of the water sample?<day'A 76 mg/LB 52 mg/LOC 100 mg/L

Answered: Serine (C3H703N) can be oxidized to…

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...

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Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.
At a certain temperature this reaction follows second-order kinetics with a rate constant of ·0.12M−1:s−1 →2Cl2O5g+2Cl2g5O2g Suppose a vessel contains Cl2O5 at a concentration of 1.29M . Calculate the concentration of Cl2O5 in the vessel 77.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
For the rearrangement of cyclopropane to propene at 500 °C (CH2)3 → CH3 CH=CH2 the following data have been obtained: [(CH₂)3], M 0.0297 0.0154 0.00793 0.00410 time, min 0 16.4 32.8 49.2 The average rate of disappearance of (CH₂) 3 over the time period from t = 0 min to t = 16.4 min is M/min.
[4] The reaction: 21 (aq) + S2O;²-(aq) → I½(aq) + 2SO,²-(aq) is first order with respect to I and first order with respect to S20g. The rate constant k was determined at different temperatures and a plot of In(k) versus 1/T was constructed resulting in the straight line: y = -5781.8x + 14.1. Assume k has units of M's. (a) Determine the activation energy for this reaction. (b) Calculate the value of k at 20 °C.
Cosmetics have often antimicrobial agents, such as methyl paraben, to prevent growth of mold and bacteria. Suppose the antimicrobial agent in a tube of sunscreen degrades with first-order kinetics, with a rate constant of 2.31 x 10-4 hr¬ at 25°C. A) Calculate the half-life of the antimicrobial agent at 25°C. Be sure to include the units. B) The activation energy for the degradation reaction is 9.2 kJ mol-1. Sup- pose you store your sunscreen in the locker room at the gym, which has an average temperature of 35°C. What is the half-life of the an- timicrobial agent in the conditions at the gym?
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Under certain conditions, the reaction 3 A+ 4B 5C is observed to proceed at a rate of 0.0275 M s ¹. What is the corresponding rate of change in product C?
The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
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The following initial rate data are for the oxidation of arsenate ion by cerium(IV) ion in aqueous solution: Experiment 1 2 3 4 3+ AsO3³ + 2Ce¹+ + H₂O → AsO4³ + 2Ce³+ + 2H+ Rate = k = [ASO3³] [Ce¹+] M M 0.0311 0.0622 0.0311 0.0622 M-2.s I Complete the rate law for this reaction in the box below. Use the form k[A] [B]", 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. -1 0.145 0.145 0.290 0.290 Initial Rate, M.s-1 S 0.000345 0.000690 0.00138 0.00276
The kinetics of the following second-order reaction were studied as a function of temperature: C₂H,Br(aq) + OH (aq) → C₂H5OH() + Br (aq) Temperature (°C) k (L/mol s) 25 35 45 55 65 8.81 x 10 0.000285 0.000854 0.00239 0.00633 . -5 Part B Determine the frequency factor for the reaction. A = VE] ΑΣΦ W ?

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