If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows:forward rate= |A|B|reverse rate = k₁ [CD]where ky and k, are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal:k[A][B]=k [CD]Thus, the rate constants are related to the equilibrium constant in the following manner:Part Athe forward reaction.For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k. given that the reverse reaction is of the same molecularity asinclude- (multiplication dot) between eachExpress your answer with the appropriate units. Include explicit multiplication within units, for example to enter Mmeasurement.View Available Hint(s)ValueSubmitPart BShow Transcribed Textk₂ = ValueSubmitUnitsPÅY Part CFor a different reaction, K, -95.6, k = 7.42 x 10's, and k, = 77.6s¹ Adding a catalyst increases the forward rate constant to 1.09x10 s What is the new value of thereverse reaction constant, k,, after adding catalyst?Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter Ms include (multiplication dot) between eachmeasurement.View Available Hint(s)2The equilibrium constant wilCE ?UnitsK. ==CDABGincreasedecreaseYet another reaction has an equilibrium constant K 4.32 x 10 at 25°C. It is an exothermic reaction, giving off quite a bit of heat while the reaction proceeds if the temperature israised to 200 C, what will happen to the equilibrium constant?View Avaliable Hint(s)not change

This question belong to Chemical Kinetics. Kc = Kf/Kb,

If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows: forward ratek AB reverse rate = k₁ [CD] where ky and ke are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal: k[A][B]=k, [CD] Thus, the rate constants are related to the equilibrium constant in the following manner: Part A For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k,, given that the reverse reaction is of the same molecularity as the forward reaction. k. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M include (multiplication dot) between each measurement. View Available Hint(s) Value Submit → C K₁ = 2- Units CD AB ?

If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows: forward ratek AB reverse rate = k₁ [CD] where ky and ke are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal: k[A][B]=k, [CD] Thus, the rate constants are related to the equilibrium constant in the following manner: Part A For a certain reaction, K, 8.01x102 and k1.64x102 Ms Calculate the value of the reverse rate constant, k,, given that the reverse reaction is of the same molecularity as the forward reaction. k. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M include (multiplication dot) between each measurement. View Available Hint(s) Value Submit → C K₁ = 2- Units CD AB ?

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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