Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:A first-order reaction is 75% complete in 349 s.
(a) What are the first and second half-lives for this reaction?
1st
2nd
S
S
(b) How long does it take for 90.9% completion?
S
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- 17. If one defines the rate of the reaction 30 CH3OH +B10H14 0 10 B(OCH3)3 + 22 H2 as -A[B10 H14] At Rate = then the rate is also correctly expressed by 1 A[CH3 OH] At 1 ΔΒ(0CH> )s] At 1 A[H;] (a) Rate = 30 (b) Rate = 10 (c) Rate = 22 At (d) none of these. (e) all of these.arrow_forwardCurrent Attempt in Progress The reaction 2A + 2B M+Nhas the rate law: Rate = k[A]?. At 25°C, k = 0.0376 L mol1s1. If the initial concentrations of A and B are 0.387 M and O.459 M, respectively Your answer is correct. (a) What is the half-life of the reaction? 68.7 seconds Hint Your answer is incorrect. (b) What will be the concentrations of A and B after 30.0 minutes? [A] = i ! M [B] = i M Hintarrow_forward1. (a) Show that decomposition of the organic compound 1,3-pentadiene is a second-order reaction and determine the rate constant. The concentration of 1,3-pentadiene was measured as a function of time. The data are as follows: (b) What is the value of the rate constant for the decomposition of 1,3-pentadiene.(c) What is the initial concentration for the reaction? Report to 3 significant figures.(d) What is the concentration of 1,3-pentadiene after 3.750 x10^3 s? Time(s) [1,3-pentadiene] (M) 0 .480 1000 .179 2000 .110 3000 .0795 4000 .0622 5000 .0510arrow_forward
- The following data were obtained on the initial rates of a reaction of a d-metal complex in aqueous solution. What is (a) the order of reaction with respect to the complex and the reactant Y. (b) the rate constant? For the experiments (a) [Y] = 2. 7 mmol dm-3 and for experiments (b) ]Y] = 6.1 mmol dm-3[complex]/(mmol dm-3) 8.01 9.22 12.11v/(mol dm-3 s-1) (a) 125 144 190 (b) 640 730 960arrow_forwardThe following data were obtained for the reaction 2C102 (ag) + 20H (ag) → Cl0; (ag) + C102 (ag) + H,0(1) A[CIO2] where Rate = - At [C102]o (mol L) [OH ], (mol L) Initial Rate (molL·s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 x 10-1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH] b Determine the value of the rate constant. Rate constant = 2.30x1 / L²/mol? - s c What would be the initial rate for an experiment with [CIO2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·sarrow_forwardThe half-life (t¼) of a/an order reaction is independent of the initial concentration: (A) (B) First Zeroarrow_forward
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