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
![**The Decomposition of Ammonia on a Platinum Surface at 856 °C**
The chemical reaction:
\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]
is **zero order** in NH₃.
In one experiment, when the initial concentration of NH₃ was \( 8.13 \times 10^{-3} \) M, the concentration of NH₃ dropped to \( 1.98 \times 10^{-3} \) M after \( 2.75 \times 10^{3} \) seconds had passed.
Based on these data, the rate constant for the reaction is [________] M s⁻¹.
**Explanation:**
This example demonstrates a zero-order reaction, where the rate of reaction is independent of the concentration of reactants. Given the decrease in ammonia concentration over time, one can calculate the rate constant using the zero-order rate law equation:
\[ \text{Rate} = k \]
where:
- \( k \) is the rate constant.
In zero-order reactions, the rate of decomposition of NH₃ directly provides information to calculate \( k \) using the formula:
\[ k = \frac{{[\text{NH}_3]_0 - [\text{NH}_3]}}{t} \]
where:
- \([\text{NH}_3]_0\) is the initial concentration,
- \([\text{NH}_3]\) is the concentration after time \( t \),
- \( t \) is the elapsed time.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc4eca0ea-f525-4d8f-9259-04e892974916%2F34789409-4951-4483-82a8-49f55046c4dc%2F2jc7ahn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**The Decomposition of Ammonia on a Platinum Surface at 856 °C**
The chemical reaction:
\[ \text{NH}_3 \rightarrow \frac{1}{2} \text{N}_2 + \frac{3}{2} \text{H}_2 \]
is **zero order** in NH₃.
In one experiment, when the initial concentration of NH₃ was \( 8.13 \times 10^{-3} \) M, the concentration of NH₃ dropped to \( 1.98 \times 10^{-3} \) M after \( 2.75 \times 10^{3} \) seconds had passed.
Based on these data, the rate constant for the reaction is [________] M s⁻¹.
**Explanation:**
This example demonstrates a zero-order reaction, where the rate of reaction is independent of the concentration of reactants. Given the decrease in ammonia concentration over time, one can calculate the rate constant using the zero-order rate law equation:
\[ \text{Rate} = k \]
where:
- \( k \) is the rate constant.
In zero-order reactions, the rate of decomposition of NH₃ directly provides information to calculate \( k \) using the formula:
\[ k = \frac{{[\text{NH}_3]_0 - [\text{NH}_3]}}{t} \]
where:
- \([\text{NH}_3]_0\) is the initial concentration,
- \([\text{NH}_3]\) is the concentration after time \( t \),
- \( t \) is the elapsed time.
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