The decomposition of nitrous oxide at 565°C is described by the following chemical equation:\[ \text{N}_2\text{O}(g) \rightarrow \text{N}_2(g) + \frac{1}{2} \text{O}_2(g) \]This reaction is second order in \(\text{N}_2\text{O}\) with a rate constant of \(1.10 \times 10^{-3} \, \text{M}^{-1}\text{s}^{-1}\).If the initial concentration of \(\text{N}_2\text{O}\) is 2.16 M, the concentration of \(\text{N}_2\text{O}\) will be \(\_\_\_\_\) M after 1480 seconds have passed.

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The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+ ½ O₂(g) is second order in N₂O with a rate constant of 1.10 × 10-³ If the initial concentration of N₂O is 2.16 M, the concentration of 1 M. S

The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+ ½ O₂(g) is second order in N₂O with a rate constant of 1.10 × 10-³ If the initial concentration of N₂O is 2.16 M, the concentration of 1 M. S

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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