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posted by  b-ren on 9/9/2008 10:40:51 PM  |  status: Live  

Average Rate

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Question Details:
Consider the following reaction:
2{\rm{ N}}_2 {\rm{O(}}g)\; \rightarrow \;2{\rm{ N}}_2 (g)\; + \;{\rm{O}}_2 (g)
 
 
In the first 11.0 s of the reaction, 1.7×10−2 mol of { is produced in a reaction vessel with a volume of 0.250 L. What is the average rate of the reaction over this time interval?
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Sage
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posted by Jesley on 9/9/2008 11:09:46 PM  |  status: Live
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b-ren's comment:
"Thanks alot"
Response Details:
average rate = Δ[O2]/Δt
                    =([O2]final -[O2]initial )/(tfinal -tinitial)
at time t=0 , [O2]initial =0
at, tfinal =11.0s ,
[O2]final=1.7x10-2mol/0.250L
               =0.068M
average rate = ( 0.068M-0)/(11.0s -0)
                         =6.182x10-3 M s-1                           
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