Dinitrogen pentoxide, (N₂O3), decomposes to NO₂ and O₂ at relatively low temperatures in the following reaction 2N₂O54NO

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Dinitrogen Pentoxide N O3 Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 1 (36.64 KiB) Viewed 80 times

Dinitrogen Pentoxide N O3 Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 2 (24.77 KiB) Viewed 80 times

Dinitrogen Pentoxide N O3 Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 3 (31.73 KiB) Viewed 80 times

Dinitrogen Pentoxide N O3 Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 4 (9.29 KiB) Viewed 80 times

Dinitrogen pentoxide, (N₂O3), decomposes to NO₂ and O₂ at relatively low temperatures in the following reaction 2N₂O54NO₂ +0₂. The rate law should be of the form rate = k[N₂0₂² To determine the rate law, we need to find the order, x, and the rate constant k. To do this the concentration of N₂O5 was monitored as a function of time, this data was used to construct the following table. In[N₂O₁] 1/[N₂Osl No answer text provided. 0 01 t (s) 2 0 600 1200 1800 2400 3000 3600 [N₂Os] 0.0365 0.0274 0.0206 -3.882 0.0117 -3.310 27.4 0.0156 -4.160 0.0086 -3.597 0.0064 -4,448 -4.755 -5.051 36.5 48.5 64.1 Using data in the Excel file 'Excel Spreadsheet Kinetics Day 2: plot graphs to determine the order x What is the order x? 85.5 116 156 4 pt
ts rning bring The rate law should be of the form =k[N₂O₁]* To determine the rate law, we need to find the order, x, and the rate constant k. To do this the concentration of N₂Os was monitored as a function of time, this data was used to construct the following table. t(s) [N₂Osl In[N₂O₁] 1/[N₂Osl rate= 0 0.0365 -3.310 600 0.0274 -3.597 1200 0.0206 -3.882 1800 0.0156 -4.160 2400 0.0117 -4.448 3000 0.0086 -4.755 3600 0.0064 -5.051 27.4 36.5 48.5 64.1 85.5 116 156 Using data in the Excel file 'Excel Spreadsheet Kinetics Day 2, determine the rate law and answer the following What is the value for the rate constant k? (here just enter the number)
Dinitrogen pentoxide, (N₂Os). decomposes to NO₂ and O₂ at relatively low temperatures in the following reaction 2N₂O54NO₂ + O₂ The rate law should be of the form rate. k N₂O₁] To determine the rate law, we need to find the order, x, and the rate constant k. To do this the concentration of N₂Os was monitored as a function of time, this data was used to construct the following table. t(s) [N₂O5] In[N₂0s] 0 0.0365 -3.310 600 0.0274 1200 0.0206- -3.882 1800 0.0156 -4.160 2400 0.0117 -4.448 -3.597 3000 0.0086 -4.755 3600 0.0064 OMI 1/ M/s -5.051 1/[N₂Os] No answer text provided 274 36.5 48.5 64,1 Using data in the Excel file 'Excel Spreadsheet Kinetics Day 2: answer the following. What are the correct units for k? 85.5 116 156
If we started with 1.0M of N₂Os how many seconds, (to 2 sig figs), would it take for the [N₂Os] to decay to half this value? (enter just the value not the units)