The rate of the reaction NO 2 (g)+ CO(g) --> NO(g) + CO(g) depends only on the c
ID: 677016 • Letter: T
Question
The rate of the reaction NO2(g)+ CO(g) --> NO(g) + CO(g) depends only on the concentration of the nitrogen dioxidebelow 225 degrees C. At a temperature below 225 degrees C, the following data werecollected. Time (s) [NO2](mol/L) 0 .500 1.2 x103 .444 3.0 x103 .381 4.5 x103 .340 9.0 x103 .250 1.8 x104 .174 Determine the rate law, the integrated law, and the value ofthe rate constant. Calculate [NO2] at 2.70 x 104 seconds after the start of thereaction. The rate of the reaction NO2(g)+ CO(g) --> NO(g) + CO(g) depends only on the concentration of the nitrogen dioxidebelow 225 degrees C. At a temperature below 225 degrees C, the following data werecollected. Time (s) [NO2](mol/L) 0 .500 1.2 x103 .444 3.0 x103 .381 4.5 x103 .340 9.0 x103 .250 1.8 x104 .174 Determine the rate law, the integrated law, and the value ofthe rate constant. Calculate [NO2] at 2.70 x 104 seconds after the start of thereaction.Explanation / Answer
We Know that : Thegiven equation is : NO2(g)+ CO(g) --> NO(g) + CO2(g) By plotting the graph for ln [ NO2 ] &Time and 1/ [ NO2 ] vstimte we get straight line Which indicates that : Rate = - [ NO2 ] / t = K [ NO2 ]2 Rate constant of theReaction = 1 / NO2 fromthe final time to the initial time K = 5.7471 - 2 / 1800 - 0 = 0.00208173L / mol-s IntegratedRate law for the second order reaction is : 1/ [ NO2 ] = Kt + 1 / [NO2 ]0 Rate of theReaction for IInd Order is : 1 / [ NO2] = 2.08 x 10-4 L/ mol-s x 27000 s + 1 / 0.500 M = 7.616 [ NO2 ] = 0.13130 M Rate of theReaction for IInd Order is : 1 / [ NO2] = 2.08 x 10-4 L/ mol-s x 27000 s + 1 / 0.500 M = 7.616 [ NO2 ] = 0.13130 MRelated Questions
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