[References)CHEMWORKA certain substance, initially present at 0.950 M, decomposes by first-order kinetics with a rate constant of 1.25 × 102 mol L-'s"! Calculate the time (in seconds) required for the system toreach a concentration of 0.555M.secondsSubmitHide HintsHint 1 Hint 2ptThe integrated rate law for this reaction is1 pt• (A] - -kt + [A]o1 ptO lax([A][A],) = -ktO MA] = kt + 1/[A]oO 1ptO In[A] - kt + In[AloO ptO MA) = -kt + 1/[AloO 1 ptCheck int1st Attempt1 ptO 1 ptFeedback151 ptn 161 ptSubmit AnswerTry Another Version10 item attempts remainingressItemsPreviousish AsnigmentSave and Exit416 PM2/26/2021%232+ backERs/DFGxcv BTCpauset shiftaltctrl

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A certain substance, initially present at 0.950 M, decomposes by first-order kinetics with a rate constant of 1.25 × 102 mol L 's'!. Calculate the time (in seconds) required for the system to reach a concentration of 0.555M. seconds Submit Hide Hints Hint 1 Hint 2 The integrated rate law for this reaction is (A)- kt + (Alo OMA) - k+ MA O la[A] -kt + In[A]o OMA)- kt+ MA

A certain substance, initially present at 0.950 M, decomposes by first-order kinetics with a rate constant of 1.25 × 102 mol L 's'!. Calculate the time (in seconds) required for the system to reach a concentration of 0.555M. seconds Submit Hide Hints Hint 1 Hint 2 The integrated rate law for this reaction is (A)- kt + (Alo OMA) - k+ MA O la[A] -kt + In[A]o OMA)- kt+ MA

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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