**The decomposition of ammonia on a tungsten surface at 1100 °C:**\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]is **zero order** in \(\text{NH}_3\).In one experiment, when the initial concentration of \(\text{NH}_3\) was \(3.00 \times 10^{-3}\) M, the concentration of \(\text{NH}_3\) dropped to \(5.91 \times 10^{-4}\) M after 506 seconds had passed.Based on these data, the rate constant for the reaction is \(\_\_\_\_\_\) M s\(^{-1}\).

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The decomposition of ammonia on a tungsten surface at 1100 °C NH31/2 N,+ 3/2 H, is zero order in NH3. In one experiment, when the initial concentration of NH3 was 3.00×10³ M, the concentration of NH3 dropped to 5.91×10* M after 506 seconds had passed. Based on these data, the rate constant for the reaction is Ms!.

The decomposition of ammonia on a tungsten surface at 1100 °C NH31/2 N,+ 3/2 H, is zero order in NH3. In one experiment, when the initial concentration of NH3 was 3.00×10³ M, the concentration of NH3 dropped to 5.91×10* M after 506 seconds had passed. Based on these data, the rate constant for the reaction is Ms!.

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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