Consider the following reaction: 4 HBr(g) + O2(g)  2 H2O(g) + 2 Br2(g) (a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)]     Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) If the rate constant for this reaction at a certain temperature is 8860, what is the reaction rate when [HBr(g)] = 0.00558 M and [O2(g)] = 0.00825 M? Rate =  _______M/s. (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0112 M while the concentration of O2(g) is 0.00825 M? Rate =  _______M/s

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Consider the following reaction:

4 HBr(g) + O2(g)  2 H2O(g) + 2 Br2(g)





(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?

Rate = k [HBr(g)] [O2(g)]
Rate = k [HBr(g)]2 [O2(g)]    
Rate = k [HBr(g)] [O2(g)]2Rate = k [HBr(g)]2 [O2(g)]2
Rate = k [HBr(g)] [O2(g)]3
Rate = k [HBr(g)]4 [O2(g)]






(b) If the rate constant for this reaction at a certain temperature is 8860, what is the reaction rate when [HBr(g)] = 0.00558 M and [O2(g)] = 0.00825 M?

Rate =  _______M/s.



(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.0112 M while the concentration of O2(g) is 0.00825 M?

Rate =  _______M/s

Expert Solution
Step 1

 

Recall the given reaction,                      4 HBr g  +  O2 g    2 H2O g  +  2 Br2 gThe reaction is first order in HBr g and first order in O2 g .We have to calculate - a The rate law for this reaction .b The reaction rate when HBr g = 0.00558 M and O2 g = 0.00825 M .c The reaction rate when HBr g = 0.0112 M and O2 g = 0.00825 M .

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