Be sure to answer all parts.The growth of Pseudomonas bacteria is modeled as a first-order process with k = 0.035 min at 37°C.The initial Pseudomonas population density is 1.0 x 103 cells/L. Enter your answers in scientificnotation.(a) What is the population density after 4.0 h?x 10 (select)cells/L(b) What is the time required for the population to go from 1.0 x 103 to 3.0 x 103 cells/ L?x 10(select)min

Answered: Image /qna-images/answer/0e5f00fc-556d-46e6-9235-e4fc8490c52f.jpg

The growth of Pseudomonas bacteria is modeled as a first-order process with k = 0.035 min at 37°C. The initial Pseudomonas population density is 1.0 x 10³ cells/L. Enter your answers in scientific notation. (a) What is the population density after 4.0 h? x 10 (select) cells/L (b) What is the time required for the population to go from 1.0 x 10 to 3.0 x 10° cells/ L? x 10 (select) min

The growth of Pseudomonas bacteria is modeled as a first-order process with k = 0.035 min at 37°C. The initial Pseudomonas population density is 1.0 x 10³ cells/L. Enter your answers in scientific notation. (a) What is the population density after 4.0 h? x 10 (select) cells/L (b) What is the time required for the population to go from 1.0 x 10 to 3.0 x 10° cells/ L? x 10 (select) min

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

Methyl acetate (CH3COOH3) reacts with water in the presence of an acid to produce methanol and acetate as described in the following equation: CH3COOH3(g) + H2O(g) → CH3OH(g) + CH3COOH(g). The reaction is first order with a rate constant of 1.26 x 10-4/s at 25oC. How long will it take for the reaction to produce 65.0% product?
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?
In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/s. Fe3+(aq) + SCN-(aq) → Fe(SCN)2+(aq). How many seconds would be required for the initial concentration of Fe3+ to decrease to 12.5% of its initial value? Express your answer to two decijal positions.
The decomposition of N2Os is first order and the rate constant k 6.82 X 103 s1. 2 N20s (g)> 4 NO2 (g) + 02 (g) at 70 °C. If the initial amount of N20s in a 2.0 L vessel is 0.0250 mol, determine the time in minutes it takes for the quantity of N20s to drop to 0.010 mol a. b. What is the half-life of N20s at 70 °C?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of ·0.0081Ms−1 2HI(g)→H2(g)+I2(g) Suppose a 4.0L flask is charged under these conditions with 400.mmol of hydrogen iodide. After how much time is there only 200.mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NHẠNCO(aq)–→(NH2)½CO(aq) is second order in NH NCO with a rate constant of 1.10x10² M' min! If the initial concentration of NH,NCO is 0.945 M, the concentration of NH NCO will be 0.160 M after minutes have passed.
The rate constant for a first-order reaction is 1.6  10–2s–1at 668 K and 5.1  10–2 s–1at 916 K. What is the activation energy? (R = 8.31 J/(mol · K))
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0096 M •s *: 2 HI (g) – H, (g) + I,(3) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of hydrogen iodide. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
For the first-order reaction N2O5( g) • 2 NO:(8) +0x8) t1/2 = 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1013 s-1, determine the value of k at 50°C. 3.
A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.47 x 10-8 s-1 at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days)
What is the effective rate constant [in units that combine M and min] for the reaction with rate law v = k[A][B]2 where k = 0.54 M -2 min-1 if the initial concentration of B is 3.7 molar and that of A is 0.032 molar?
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,O2(aq)H,0() + ½ O2(g) is first order in H20, with a rate constant of 1.10x10-3 min!. If the initial concentration of H,O, is 6.48×10-2 M, the concentration of H,O, will be 1.17x10-2 M after min have passed.