Item 99 of 18 (>I Review Constants | Periodic TableThe half-life of a reaction, t2, is the time it takes for the reactant concentration [A] to decrease by half. Forexample, after one half-life the concentration falls from the initial concentration [A]o to [A]o/2, after a secondhalf-life to [Alo/4, after a third half-life to [A]o/8, and so on. on.For a first-order reaction, the half-life is constant. It depends only on the rate constant k and nof on the reactant concentration. It is expressed ast1/2For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed ast1/2EA.Part AA certain first-order reaction (A→products) has a rate constant of 5.70x10-s at 45 °C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration?Express your answer with the appropriate units.• View Available Hint(s)8.11 minSubmitPrevlous Anawerev CorrectPart BA certain second-order reaction (Bproducts) has a rate constant of 1.00x10-3 M1.s'at 27 °C and an initial half-life of 218 s. What is the concentration of the reactant B after one half-life?Express your answer with the appropriate units.• View Available Hint(s)Tempjetes Symbols undo redo Teset keyboard shortcuts helpValueUnitsSubmit

- PartA A certain firstorder reaction (A-producta) has a rate constant of 5.70x10sa 45"C. How many minutes does ittake for the concentration of the reactant JA). to drop to 628% of the original concentration? Express your answer with the appropriate units. View Available Hints) 811 min Prevtoun Ane v Correct - Part B Acerain second-order reacton (B-producta) has a rae constant of 1.00x10 ars'x27"C and an intal hatite of 213s. Waris the concentaton of the reacart Bater one hate Express your answer with the appropriate units. View Available Hints) ge feset keyboard shotouts Help Value Units Submit

- PartA A certain firstorder reaction (A-producta) has a rate constant of 5.70x10sa 45"C. How many minutes does ittake for the concentration of the reactant JA). to drop to 628% of the original concentration? Express your answer with the appropriate units. View Available Hints) 811 min Prevtoun Ane v Correct - Part B Acerain second-order reacton (B-producta) has a rae constant of 1.00x10 ars'x27"C and an intal hatite of 213s. Waris the concentaton of the reacart Bater one hate Express your answer with the appropriate units. View Available Hints) ge feset keyboard shotouts Help Value Units Submit

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

For the rearrangement of cyclopropane to propene at 500 °C(CH2)3CH3CH=CH2the following data have been obtained: [(CH2)3], M 0.192 9.20×10-2 4.41×10-2 2.11×10-2 time, min 0 18.3 36.6 54.9 The average rate of disappearance of (CH2)3 over the time period from t = 36.6 min to t = 54.9 min is M min-1.
The rxn I- + OCl- ® IO- + Cl- is first order with respect to I- and first order with respect to OCl-. The rate constant is 8.0 x 10-2 L/mol×s. What is the rate of rxn when [I-] = 0.10 M and [OCl-] = 0.20 M? a) 4.4 x 10-4 M/s b) 1.6 x 10-3 M/s c) 3.2 x 10-3 M/s d) 2.2 x 10-4 M/s e) 2.4 x 10-5 M/s
- 1 - 1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 32.5M •S : NH,ОH (аq) -- Nн; (ад) +н,о (аq) Suppose a vessel contains NH,OH at a concentration of 0.910M. Calculate the concentration of NH,OH in the vessel 0.120 seconds later. You may assume '4 no other reaction is important. Round your answer to 2 significant digits. OM x10
The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 7.99 x 10-³ M-s¹, when [NO] = S = 0.192 M and [H₂] = 0.129 M. From this experiment, the rate M².s¹. constant is
Calculate the concentration [A] for a reaction A Product after 7.00 min, knowing that the initial concentration [A]o is 2.4 M, and the rate constant is 3.2x10-3 M-1sec-1. Edit Format Table 12pt v Paragraph v BIU T?v : hp 732006020610 f3 米 fo f9 @
I Review | Constants | Period MISSED THIS? Read Section 15.4 (Pages 642 - 649); Watch KCV 15.4, IWVE 15.4.The decomposition of SO2 Cl2 is first order in SO2 Cl2 and has a rate constant of 1.40x104s-1 at a certain temperature. -kt + In(SO2C2]o - (1.40 x 10-s)(220 s) + In 0.175 M In[SO2 Cl2]t %3D -1.774 Take the inverse natural logarithm of both sides of the equation. [SO2 Cl2]: e-1.774 M 0.170 M Part E If the initial concentration of SO2 Cl2 is 0.175 M, what is the concentration of SO2 Cl2 after 510 s ? Express your answer using three significant figures. ΑΣφ (SO2 Cl2]e = M