The reaction, 2 NO2(g) + O3(g) N2O5(g) + O2(g), was studied at a certain tempera

ID: 733932 • Letter: T

Question

The reaction, 2 NO2(g) + O3(g) N2O5(g) + O2(g), was studied at a certain temperature with the following results:
Experiment [NO2(g)] (M) [O3(g)] (M) Rate (M/s)
1 0.904 0.904 5.31e+04
2 0.904 1.81 1.06e+05
3 1.81 0.904 1.06e+05
4 1.81 1.81 2.13e+05

If the rate law for this reaction is, Rate = k [NO2(g)] [O3(g)], what is the value of the rate constant?

a) The value of rate constant is k = 6.50e+04 M-1 s-1.
b) The value of rate constant is k = 5.56e+05 M-1 s-1.
c) The value of rate constant is k = 1.92e+06 M-1 s-1.
d) The value of rate constant is k = 1.49e+05 M-1 s-1.
e) The value of rate constant is k = 7.75e+03 M-1 s-1.

Explanation / Answer

a) The value of rate constant is k = 6.50e+04 M-1 s-1.

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The reaction, 2 NO2(g) + O3(g) N2O5(g) + O2(g), was studied at a certain tempera

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