Dinitrogen Pentoxide N Os Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 1 (38.63 KiB) Viewed 53 times
Dinitrogen Pentoxide N Os Decomposes To No And O At Relatively Low Temperatures In The Following Reaction 2n O54no 2 (19.37 KiB) Viewed 53 times
Dinitrogen pentoxide, (N₂Os), 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[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) [N₂Os] In[N₂Os] 0 600 0.0365 -3.310 0.0274 1200 0.0206 -3.882 -3.597 1800 0.0156 -4.160 2400 0.0117 -4.448 3000 0.0086 -4.755 3600 0.0064 -5.051 M²1 01/s 1/[N₂Osl M/s No answer text provided. 27.4 36.5 48.5 64.1 85.5 Using data in the Excel file 'Excel Spreadsheet Kinetics Day 2, answer the following. What are the correct units for k? 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) 144 Question 27 4 pts Assuming with start with 1.0 M of N₂O5, what is the instantaneous rate for the reaction at t-2000s? Again give the answer in mols/L and to 2 sig figs (just give the number not the units)
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