The following data were obtained for the reaction of NO with O2. Concentrations are in molecules/cm3 and rates are in molecules/cm3⋅s.[NO]0[O2]0Initial Rate1 × 10181 × 10182.0 × 10162 × 10181 × 10188.0 × 10163 × 10181 × 101818.0 × 10161 × 10182 × 10184.0 × 10161 × 10183 × 10186.0 × 1016What is the rate law? a.Rate = k[NO][O2]2 b.Rate = k[NO]2[O2] c.Rate = k[NO]2[O2]2 d.Rate = k[NO]2 e.Rate = k[NO][O2]

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Chemistry

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The following data were obtained for the reaction of NO with O₂. Concentrations are in molecules/cm³ and rates are in molecules/cm³⋅s.

[NO]₀	[O₂]₀	Initial Rate
1 × 10¹⁸	1 × 10¹⁸	2.0 × 10¹⁶
2 × 10¹⁸	1 × 10¹⁸	8.0 × 10¹⁶
3 × 10¹⁸	1 × 10¹⁸	18.0 × 10¹⁶
1 × 10¹⁸	2 × 10¹⁸	4.0 × 10¹⁶
1 × 10¹⁸	3 × 10¹⁸	6.0 × 10¹⁶

What is the rate law?

	a.	Rate = k[NO][O₂]²
	b.	Rate = k[NO]²[O₂]
	c.	Rate = k[NO]²[O₂]²
	d.	Rate = k[NO]²
	e.	Rate = k[NO][O₂]

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