**The Decomposition of Nitrous Oxide at 565 °C**The chemical reaction for the decomposition of nitrous oxide is:\[ \text{N}_2\text{O} (g) \rightarrow \text{N}_2 (g) + \dfrac{1}{2} \text{O}_2 (g) \]This reaction is second order with respect to N₂O, and the rate constant is \(1.10 \times 10^{-3} \, \text{M}^{-1}\text{s}^{-1}\).**Problem:**Given that the initial concentration of N₂O is 2.16 M, what will the concentration of N₂O be after 1480 seconds?**Answer:**\[ \boxed{\text{M}} \]

Let a is initial concentration. and a-x is concentration after time t

The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(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 N₂O will be M after 1480 seconds have passed. 1 M.S

The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(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 N₂O will be M after 1480 seconds have passed. 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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