N2O5 is used as a source of NO2 in chemical reactions. The compound decomposes in a first order reaction. If the initial concentration of N2O5 = 0.400 M, and the concentration is 0.025 M after 120 seconds, what is the rate constant k of the reaction? a. 7.50 s-1 b. 333 s-1 c. 2.77 s-1 d. 2.31 x 102s1 e. 5.21 x 104s

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**Chemical Reaction Kinetics Example Problem**

*Nitrogen Pentoxide Decomposition Rate Constant Calculation*

**Problem:**

N₂O₅ is used as a source of NO₂ in chemical reactions. The compound decomposes in a first-order reaction. If the initial concentration of N₂O₅ is 0.400 M, and the concentration is 0.025 M after 120 seconds, what is the rate constant \( k \) of the reaction?

**Options:**
a. 7.50 s\(^{-1}\)
b. 333 s\(^{-1}\)
c. 2.77 s\(^{-1}\)
d. 2.31 × 10\(^{-2}\) s\(^{-1}\)
e. 5.21 × 10\(^{-4}\) s\(^{-1}\)

**Solution Strategy:**
To find the reaction rate constant \( k \) for a first-order reaction, use the first-order kinetics formula:
\[ \ln([A]_t) = \ln([A]_0) - kt \]
Where:
- \([A]_t\) is the concentration of N₂O₅ at time \( t \)
- \([A]_0\) is the initial concentration of N₂O₅
- \( t \) is the time elapsed
- \( k \) is the rate constant to be determined

Given:
- \([A]_0 = 0.400 \, M\)
- \([A]_t = 0.025 \, M\)
- \( t = 120 \, \text{s}\)

Follow these steps to solve for \( k \):

1. Substitute the given concentrations and time into the first-order kinetics formula.
2. Rearrange and solve for \( k \).

This example helps illustrate the application of first-order kinetics principles in determining the rate constant of a decomposition reaction.
Transcribed Image Text:**Chemical Reaction Kinetics Example Problem** *Nitrogen Pentoxide Decomposition Rate Constant Calculation* **Problem:** N₂O₅ is used as a source of NO₂ in chemical reactions. The compound decomposes in a first-order reaction. If the initial concentration of N₂O₅ is 0.400 M, and the concentration is 0.025 M after 120 seconds, what is the rate constant \( k \) of the reaction? **Options:** a. 7.50 s\(^{-1}\) b. 333 s\(^{-1}\) c. 2.77 s\(^{-1}\) d. 2.31 × 10\(^{-2}\) s\(^{-1}\) e. 5.21 × 10\(^{-4}\) s\(^{-1}\) **Solution Strategy:** To find the reaction rate constant \( k \) for a first-order reaction, use the first-order kinetics formula: \[ \ln([A]_t) = \ln([A]_0) - kt \] Where: - \([A]_t\) is the concentration of N₂O₅ at time \( t \) - \([A]_0\) is the initial concentration of N₂O₅ - \( t \) is the time elapsed - \( k \) is the rate constant to be determined Given: - \([A]_0 = 0.400 \, M\) - \([A]_t = 0.025 \, M\) - \( t = 120 \, \text{s}\) Follow these steps to solve for \( k \): 1. Substitute the given concentrations and time into the first-order kinetics formula. 2. Rearrange and solve for \( k \). This example helps illustrate the application of first-order kinetics principles in determining the rate constant of a decomposition reaction.
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