Answer: Rate Laws (Section)The following data were
Chapter , Problem 36E(choose chapter or problem)
The following data were collected for the rate of disappearance of \(\mathrm{NO}\) in the reaction \(2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}_{2}(g)\)
Experiment |
\({[\mathrm{NO}](\mathrm{M})}\) |
\({\left[\mathrm{O}_{2}\right](\mathrm{M})}\) |
Initial Rate \((\mathrm{M} / \mathrm{s})\) |
1 |
0.0126 |
0.0125 |
\(1.14 \times 10^{-2}\) |
2 |
0.0252 |
0.0125 |
\(5.64 \times 10^{-2}\) |
3 |
0.0252 |
0.0250 |
\(1.13 \times 10^{-1}\) |
(a) What is the rate law for the reaction?
(b) What are the units of the rate constant?
(c) What is the average value of the rate constant calculated from the three data sets?
(d) What is the rate of disappearance of \(\mathrm{NO}\) when
\({[\mathrm{NO}]=0.0750 \mathrm{M} \text { and }\left[\mathrm{O}_{2}\right]=0.0100 \mathrm{M}}\)?
is the rate of disappearance of \(\mathrm{O}_{2}\) at the concentrations given in part ?
Equation Transcription:
Text Transcription:
NO
2NO(g)+O2(g) \rightarrow 2NO2(g)
[NO](M)
[O2](M)
(M/s)
1.14 x 10-2
5.64 x 10-2
1.13 x 10-1
NO
[NO]=0.0750M and [O2]=0.0100M
O2
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