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The experimental rate constant for the reaction, when L P(C,Hs)3, is 9.3 x 103 s1 at 20 °C. If the initial concentration of Ni(CO), is 0.018 M, what is the concentration of the product after 6.7 minutes? Concentration =

The experimental rate constant for the reaction, when L P(C,Hs)3, is 9.3 x 103 s1 at 20 °C. If the initial concentration of Ni(CO), is 0.018 M, what is the concentration of the product after 6.7 minutes? Concentration =

Chemistry
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 substitution of CO in Ni(CO)4 by another molecule L [where L is an electron-pair donor such as P(CH3)3] was studied some years ago and led to an understanding of some of the general principles that govern the chemistry of compounds having metal-CO bonds. A detailed study of the kinetics of the reaction led to the following mechanism: Slow Ni(CO) + Ni(CO), + CO Fast Ni(CO); +L Ni(CO),L The experimental rate constant for the reaction, when L P(C,Hs)3, is 9.3 x 10 s1 at 20 °C. If the initial concentration of Ni(CO), is 0.018 M, what is the concentration of the product after 6.7 minutes? Concentration = M
Transcribed Image Text:The substitution of CO in Ni(CO)4 by another molecule L [where L is an electron-pair donor such as P(CH3)3] was studied some years ago and led to an understanding of some of the general principles that govern the chemistry of compounds having metal-CO bonds. A detailed study of the kinetics of the reaction led to the following mechanism: Slow Ni(CO) + Ni(CO), + CO Fast Ni(CO); +L Ni(CO),L The experimental rate constant for the reaction, when L P(C,Hs)3, is 9.3 x 10 s1 at 20 °C. If the initial concentration of Ni(CO), is 0.018 M, what is the concentration of the product after 6.7 minutes? Concentration = M
Expert Solution
Step 1
  • First order kinetics:- The reactions which has order equal to one, follows first order kinetics. 
  • Example- All the nuclear reactions follow first order kinetics.
  • First order kinetics rate equation is as follows:-

        Kt=lnaoat

       where,

       K=rate constant of the reaction

       t= time

     ao= initial concentration at time zero

     at= concentration left after time 't=6.7min'

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