The rate law for the reaction A - P is rate = k[A]³. The first half-life of the reaction is 20 seconds,what is the time for the second half-life? (to guarantee some marks you can submit yourcalculations)Select one:O a. 40 secondsO b. 160 secondsO . 80 secondsO d. 10 secondsO e. 20 seconds

Half life is the time taken for the reactant to reduce to half of its initial concentration. It is a…

Answered: The rate law for the reaction A - P is…

Chemistry

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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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If the half-life of a 1st order reaction is 67 minutes, k= a. 1.0x10-2s-1 b. 97 s-1 c. 5800 s-1 d. 1.7x10-4s-1
What is the half life of the following reaction, given the following set of conditions (Hint: observe the units for the rate constant to determine the order of the reaction!): 2 HI (g) → H2 (g) + I2 (g) Initial concentration of HI = 1.00 M k = 1.2 x 10-3 M-1 s-1 Select one: a. 420 s b. 240 s c. 580 s d. 830 s
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2HIg) --> H2g) +l2ls) The above reaction is zero order with respect to HI. The rate constant was found to be 1.2 X 10-4 mol/L.s. If the intial concentration of HI was 0.250 mol/L. Cal culate the comcentration of HI at 13.6 minutes after the start of the reaction (You answer should be to 2 d.p. eg., 0.45 Answer:
The decomposition of a chemical follows the Zero order with a rate constant, k = 0.00543 M/s. If the initial concentration of the reactant is 2.32. what is the concentration after 900 seconds?. The decomposition of a chemical is in the second order with a rate constant, k = .0123 M-1min-1. If the initial concentration of the reactant is 0.765 M. What is the concentration after 15 minutes.
2. A certain second order reaction has a half-life of 58.0 s. Determine the time (in seconds) needed for the reaction to be 88.0 % complete if the starting concentration is 14.20 M. (Hint: you're given the half-life, what can you determine? Once you have that, are you able to solve for the time?)
The reaction B→ products is of order "x", i.e. rate = k[B]*. When [B]o 1.20 M, the half-life of the reaction is 20. s. When [B]o = 0.40 M, = the half-life of the reaction is 60 s. What is the order of the reaction? 02 01 0-1 3.
You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 1.3 mol of A is mixed with 2.3 mol of B to make a 1.000 L solution and the rate of the reaction is 1.6 M/s, what is the rate constant (k)?
I need the answer as soon as possible
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The rate law for the reaction A - P is rate = k[A]³. The first half-life of the reaction is 20 seconds, what is the time for the second half-life? (to guarantee some marks you can submit your calculations) Select one: O a. 40 seconds O b. 160 seconds O . 80 seconds O d. 10 seconds O e. 20 seconds