the reaction, 2 NO2(g) + O3(g)----->N2O5(g) + O2(g), was studied at a certain te
ID: 733943 • 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) [H2(g)] (M) RATE
1 .0782 .0782 4.24e+01
2 .0782 .156 8.46e+01
3 .156 .0782 1.69e+02
4 .156 .156 3.37e+02
If the rate law for this reaction is, Rate = k [NO(g)]2 [H2(g)], what is the value of the rate constant?
a) The value of rate constant is k = 8.87e+04 M-2 s-1.
b) The value of rate constant is k = 2.62e+06 M-2 s-1.
c) The value of rate constant is k = 3.61e+04 M-2 s-1.
d) The value of rate constant is k = 1.37e+04 M-2 s-1.
e) The value of rate constant is k = 6.59e+05 M-2 s-1.?
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Explanation / Answer
second order reaction 42.4= k[NO2]2 [h2] k = 42.4/0.782^3 = 8.87 * 10^4 M^-1 s^-1
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