Below is the answer and then a chemistry problem from an old test my professor g

Question

Below is the answer and then a chemistry problem from an old test my professor gave us from a previous year's final. I solved part A but can't seem to figure out how you would get B. Any help?

Also final is in a few hours so the sooner the better!

Thanks!!

2.11 times lO4 M-1 s-1, Mechanism #2 The following reaction between NO, and 03 was studied at T= 296 K, and was shown to be first order in NO2 and first order in 03. 2NO,(g) + 03(g) rightarrow N205(g) + 02(g) In one experiment, initial concentrations of [NO2]i = 0.01 M and [03]j = 0.02 M produced an initial rate of 4.22 M s-1. Find the value of the rate constant. (Be sure to report your answer with appropriate units.) The following mechanisms have been proposed for the reaction. Which one of these mechanisms is more likely to be correct, and why? (To receive credit here you must give a reasonable explanation of how you chose the more plausible mechanism. Please be brief, but be sure that you make your point clearly.) Mechanism # 1: Mechanism#2: NO2 + NO2 rightarrow N204(slow) N02 + 03 rightarrow NO3 + O2(slow) N204 + 03 rightarrow N205 + O2(fast) NO3 + NO2 rightarrow N205(fast)

Explanation / Answer

Both Mechanisms are two step, with the starting reaction slow, and the final reaction fast. Mechanism 2 would be the better choice here because you are yielding only one final product, N2O5. Mechanism 1 would produce the O2 byproduct which would end up reacting with the N2O5 and muddling the results.

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