Nitric oxide reacts rapidly with unstable nitrogen trioxide (NO3) to form NO2: $$NO(g)+NO3(g)2NO2(g) Calculate the numeric value of the rate constant for the above reaction from the data in the table below. Initial Reaction Rates for the Formation of NO2 by the Reaction of NO with NO3 at 298 K. Experiment [NO]0 (M) [NO3]0 (M) Initial Reaction Rate (M/s) 1 1.80×10-3 1.80×10-3 3.60×104 2 3.60×10-3 1.80×10-3 7.20×104 3 3.60×10-3 3.60×10-3 144000 The rate constant, k, is M-1s-1
Nitric oxide reacts rapidly with unstable nitrogen trioxide (NO3) to form NO2: $$NO(g)+NO3(g)2NO2(g) Calculate the numeric value of the rate constant for the above reaction from the data in the table below. Initial Reaction Rates for the Formation of NO2 by the Reaction of NO with NO3 at 298 K. Experiment [NO]0 (M) [NO3]0 (M) Initial Reaction Rate (M/s) 1 1.80×10-3 1.80×10-3 3.60×104 2 3.60×10-3 1.80×10-3 7.20×104 3 3.60×10-3 3.60×10-3 144000 The rate constant, k, is M-1s-1
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Nitric oxide reacts rapidly with unstable nitrogen trioxide (NO3) to form NO2:
$$NO(g)+NO3(g)2NO2(g)
Calculate the numeric value of the rate constant for the above reaction from the data in the table below.
Initial Reaction Rates for the Formation of NO2 by the Reaction of NO with NO3 at 298 K.
| Experiment | [NO]0 (M) | [NO3]0 (M) | Initial Reaction Rate (M/s) |
| 1 | 1.80×10-3 | 1.80×10-3 | 3.60×104 |
| 2 | 3.60×10-3 | 1.80×10-3 | 7.20×104 |
| 3 | 3.60×10-3 | 3.60×10-3 | 144000 |
The rate constant, k, is
M-1s-1
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