**Reaction Rate Data for Nitrogen Dioxide and Fluorine**The following initial rate data are provided for the reaction of nitrogen dioxide (NO₂) with fluorine (F₂):\[ 2 \text{NO}_2 + \text{F}_2 \rightarrow 2 \text{NO}_2\text{F} \]| Experiment | \([\text{NO}_2]_0\), M | \([\text{F}_2]_0\), M | Initial Rate, M·s⁻¹ ||------------|------------------|------------------|--------------------|| 1 | 4.38 | 3.40 | 1.88 × 10⁻³ || 2 | 4.38 | 6.80 | 3.75 × 10⁻³ || 3 | 8.76 | 3.40 | 3.75 × 10⁻³ || 4 | 8.76 | 6.80 | 7.51 × 10⁻³ |**Task:** Complete the rate law for this reaction using the form:\[ k[\text{A}]^m[\text{B}]^n \]- Note: '1' is understood for \(m\) or \(n\) when concentrations taken to the zero power do not appear. Do not enter '1' for \(m\) or \(n\).**Rate Law Completion:**- Rate = \(__\)- Rate constant, \(k =\) \(__\) M⁻¹·s⁻¹

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Use the References to access important values if needed for this question. The following initial rate data are for the reaction of nitrogen dioxide with fluorine: Experiment [NO₂]0, M 4.38 4.38 8.76 8.76 1 2 3 4 2 NO2+ F2 → 2 NO₂ F Rate = [F20, M Initial Rate, M s 1 . 3.40 1.88 × 10-3 6.80 3.75 x 10-3 3.40 3.75 x 10 6.80 -3 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for k= M-¹ 1 .S -3 7.51 × 10- m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.

Use the References to access important values if needed for this question. The following initial rate data are for the reaction of nitrogen dioxide with fluorine: Experiment [NO₂]0, M 4.38 4.38 8.76 8.76 1 2 3 4 2 NO2+ F2 → 2 NO₂ F Rate = [F20, M Initial Rate, M s 1 . 3.40 1.88 × 10-3 6.80 3.75 x 10-3 3.40 3.75 x 10 6.80 -3 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for k= M-¹ 1 .S -3 7.51 × 10- m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n.

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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Question

**Reaction Rate Data for Nitrogen Dioxide and Fluorine**

The following initial rate data are provided for the reaction of nitrogen dioxide (NO₂) with fluorine (F₂):

\[ 2 \text{NO}_2 + \text{F}_2 \rightarrow 2 \text{NO}_2\text{F} \]

| Experiment | \([\text{NO}_2]_0\), M | \([\text{F}_2]_0\), M | Initial Rate, M·s⁻¹ |
|------------|------------------|------------------|--------------------|
| 1 | 4.38 | 3.40 | 1.88 × 10⁻³ |
| 2 | 4.38 | 6.80 | 3.75 × 10⁻³ |
| 3 | 8.76 | 3.40 | 3.75 × 10⁻³ |
| 4 | 8.76 | 6.80 | 7.51 × 10⁻³ |

**Task:** Complete the rate law for this reaction using the form:

\[ k[\text{A}]^m[\text{B}]^n \]

- Note: '1' is understood for \(m\) or \(n\) when concentrations taken to the zero power do not appear. Do not enter '1' for \(m\) or \(n\).

**Rate Law Completion:**

- Rate = \(__\)

- Rate constant, \(k =\) \(__\) M⁻¹·s⁻¹

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