SavedA city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. For the water to be safe for drinking, the concentration of this toxin must be below 15x 10 mgL Fortunately this toxin decomposesto a safe mixture of products by first-order kinetics with a rate constant of 0.27 day. How long will it take for the water to be safe to drink?HelpSave &Exit51Multiple Choice20. days2.2 days27 days22 days26 daysNestNext7 of 35( Prev

Given-> Initial concentration of toxin = 0.63 mg/L Final concentration of toxin=1.5 ×…

Saved A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. For the water to be safe for drinking, the concentration of this toxin must be below 15x 10 mgL Fortunately this towin deco to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day. How long will it take for the water to be safe to drink? Help Multiple Choice 20. days 2.2 days 27 days 22 days 26 days Negt 7 of 35 ( Prev

Saved A city's water supply is contaminated with a toxin at a concentration of 0.63 mg/L. For the water to be safe for drinking, the concentration of this toxin must be below 15x 10 mgL Fortunately this towin deco to a safe mixture of products by first-order kinetics with a rate constant of 0.27 day. How long will it take for the water to be safe to drink? Help Multiple Choice 20. days 2.2 days 27 days 22 days 26 days Negt 7 of 35 ( Prev

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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The following data show the rate constnat of a first order reaction measured at several different temperatures. Construct and Arrhenius plot (ln k vs 1/T) to determine the activation energy (Ea). You should use a graphing program like excel to construct your graph. A sketch of the graph including the equation of the line should be included in your notebook. temperature (K) rate constant (s-1) 375 1.68 x 10-5 400 3.50 x 10-5 500 4.20 x 10-4 600 2.11 x 10-3
MISSED THIS? Watch KCV 14.6; Read Section 14.6. You can click on the Review link to access the section in your e Text. The tabulated data were collected for the following second-order reaction: A(g) + B₂ (g) → AB(g) + B(g) Temperature (K) Rate constant (L/(mol.s)) 90 100 110 120 0.00112 0.0276 0.381 3.392 Part B Use an Arrhenius plot to determine the frequency factor for the reaction. Express your answer in reciprocal moles per liter per second to three significa 15| ΑΣΦ A = 0.001156 2 Submit Previous Answers Request Answer ? M-1.s-1
Based on the data below. Graphically determine the rate law for the reaction, and extract the rate constant and initial concentrations. 2 A -----> B Time [A] 5 11.4730407 10 7.6906092 15 5.15516951 20 3.45561346 25 2.31636698 30 1.55270722 35 1.04081077
A particular second order reaction has a rate constant of 0.0345 M-1 min-1 and an initial concentration of 0.300 M. What is the half-life of this reaction? 4.35 min 12.0 min 20.1 min 96.6 min
#26 please. I got 3 A + 4 B and 6 C. I would like to see your steps This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl
-1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 1.40 s : CICH₂CH₂CI (g) → CH₂CHC1 (g) + HCI (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.47 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 0.500 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 x Ś
Using a zero order integrated rate law to find concentration change -1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0068 M.s¹: 2 NH3 (g) → N₂ (g) +3 H₂ H2(g) Suppose a 300. mL flask is charged under these conditions with 450. mmol of ammonia. How much is left 60. 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. M ☐ x10 ك ? 000 18 Ar New Chrome available :
16. The reaction between A and B is as follows: * A 2B 2C The rate of reaction with variation of concentration of A and B at the same temperature is shown in Table 2. Table 2 Rate of reaction /mol dms! 1.20 x 102 9.00 x 103 1.35 x 102 Experiment [AJAmol dm³ [B]/mol dm³ 1.00 2.00 1.00 1.50 II III 1.50 1.00 IV 2.00 0.50 What is the value of x ? A. 3.00 x 103 B. 6.00 x 103 C. 1.20 x 10 D. 2.40 x 10
. At body temperature, the first-order rate constant is 1.87 x 103 min¹ for the elimination of the cancer chemotherapy agent, cisplatin, from the human body. How many hours will it take for 2.5 x 10-3 M of cisplatin to decrease its concentration to 1.0 x 10-³ M? ray mamuntive 20 mucaraman uantment પર ભરોસ www male de contest menaces yetamanas
mechanism 1 overall reaction is 2NO + Cl2 --> 2NOCl NO + Cl2 = NOCl2 fast equilibriumNOCl2 + NO---> 2NOCl slow rate law for mechanism 1 is rate=k[no2]^2[cl2] mechanism 2 Cl2 --> 2Cl slowCl + NO --> NOCl fast rate law for this mechansim 2 is rate=k[cl2] i noticed that when the mechanism has a fast reaction at equilibrium, the rate law includes reactants form both fast and slow, whereas when the reaction has fast reactions not at equilibrium, the rate law is only the reactants from the slow step (rate determining step) why is the rate law different when the fast reaction is at equilibrium vs when the mechansim has a fast reaction not at equilibrium?