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Choose the correct molecularity and rate law for each of the elementary reactions shown below. (a) I(g) + Br(g) Æ IBr(g)   Molecularity:   unimolecular                         bimolecular                            termolecular Rate Law: Rate = k [I] [Br] Rate = k [I]2 [Br]2     Rate = k [IBr]2Rate = k [IBr]   (b) IBr(g) Æ I(g) + Br(g)   Molecularity:   unimolecular                          bimolecular                            termolecular                         Rate Law: Rate = k [IBr]2 Rate = k [I]2 [Br]2     Rate = k [I] [Br]Rate = k [IBr]   (c) NO(g) + N2O(g) Æ N2(g) + NO2(g)   Molecularity:     unimolecular                          bimolecular                          trimolecular Rate Law: Rate = k [N2] [NO2] Rate = k [N2]2 [NO2]2     Rate = k [NO] [N2O] Rate = k [NO]2 [N2O]2   (d) 2 I(g) Æ I2(g)   Molecularity:      Rate Law: Rate = k [I2]2Rate = k [I]2    Rate = k [I2]Rate = k [I]   (e) I2(g) Æ 2 I(g)   Molecularity:      Rate Law: Rate = k [I] Rate = k [I2]     Rate = k [I2]2 Rate = k [I]2

Choose the correct molecularity and rate law for each of the elementary reactions shown below. (a) I(g) + Br(g) Æ IBr(g)   Molecularity:   unimolecular                         bimolecular                            termolecular Rate Law: Rate = k [I] [Br] Rate = k [I]2 [Br]2     Rate = k [IBr]2Rate = k [IBr]   (b) IBr(g) Æ I(g) + Br(g)   Molecularity:   unimolecular                          bimolecular                            termolecular                         Rate Law: Rate = k [IBr]2 Rate = k [I]2 [Br]2     Rate = k [I] [Br]Rate = k [IBr]   (c) NO(g) + N2O(g) Æ N2(g) + NO2(g)   Molecularity:     unimolecular                          bimolecular                          trimolecular Rate Law: Rate = k [N2] [NO2] Rate = k [N2]2 [NO2]2     Rate = k [NO] [N2O] Rate = k [NO]2 [N2O]2   (d) 2 I(g) Æ I2(g)   Molecularity:      Rate Law: Rate = k [I2]2Rate = k [I]2    Rate = k [I2]Rate = k [I]   (e) I2(g) Æ 2 I(g)   Molecularity:      Rate Law: Rate = k [I] Rate = k [I2]     Rate = k [I2]2 Rate = k [I]2

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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Choose the correct molecularity and rate law for each of the elementary reactions shown below.


(a) I(g) + Br(g) Æ IBr(g)  

Molecularity:   unimolecular

                        bimolecular  

                         termolecular

 Rate Law:
Rate = k [I] [Br]
Rate = k [I]2 [Br]2    
Rate = k [IBr]2Rate = k [IBr]


 
(b) IBr(g) Æ I(g) + Br(g)  

Molecularity:   unimolecular

                         bimolecular  

                         termolecular

                       

 Rate Law:
Rate = k [IBr]2
Rate = k [I]2 [Br]2    
Rate = k [I] [Br]Rate = k [IBr]


 
(c) NO(g) + N2O(g) Æ N2(g) + NO2(g)  

Molecularity:     unimolecular

                         bimolecular

                         trimolecular

 Rate Law:
Rate = k [N2] [NO2]
Rate = k [N2]2 [NO2]2    
Rate = k [NO] [N2O]
Rate = k [NO]2 [N2O]2


 
(d) 2 I(g) Æ I2(g)  
Molecularity:      Rate Law:
Rate = k [I2]2Rate = k [I]2    Rate = k [I2]Rate = k [I]


 
(e) I2(g) Æ 2 I(g)  
Molecularity:      Rate Law:
Rate = k [I]
Rate = k [I2]    
Rate = k [I2]2
Rate = k [I]2
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