CH,COOC,H,–CH,COOH + C,H,the rate constant at 675.0 K is 0.00106 /s and the rate constant at 719.0 Kis 0.00939 /s.The activation energy for the gas phase decomposition of ethyl acetateiskJ/mol.Arrhenius EquationThe variation of the rate constant with temperature can be expressed bythe Arrhenius Equation. The two-point form of this equation can be writtenas:"(수)- (뉴EaInT1where k and kj are the values of the rate constant at the Kelvintemperatures T2 and T1, respectively, E is the activation energy, and R isthe ideal gas constant.You may see slightly different, but equivalent, forms of this equation. It'seasy to confuse the different forms. They will all give the same result, butnot if you mix parts of one form with parts of another!Here are two more forms that you are likely to see. Can you spot thedifferences between these and the form above?Eak1Inkaln () --Gk2EaRT2In the first one, the k2 and ki terms are interchanged. To balance this, the1andT2terms are as well.In the second one, a minus sign precedesEaThis is balanced by11interchangingandT

Given: Rate constant at 675.0 K = 0.00106 s-1 Rate constant at 719.0 K = 0.00939 s-1

CH,COOC,H, the rate constant at 675.0 K is 0.00106/s and the rate constant at 719.0 K is 0.00939 /s. +CH;COOH + C,H, The activation energy for the gas phase decomposition of ethyl acetate is | kJ/mol.

CH,COOC,H, the rate constant at 675.0 K is 0.00106/s and the rate constant at 719.0 K is 0.00939 /s. +CH;COOH + C,H, The activation energy for the gas phase decomposition of ethyl acetate is | kJ/mol.

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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