**Transcription for Educational Website:**---**Enter your answer in the provided box.**The rate constant for the following second-order reaction is 0.80 /(M · s) at 10°C.\[ 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \]Calculate the half-life when \([\text{NOBr}]_0 = 0.134 \, M.\)\[ \boxed{ \; \; \; \; } \, s \]---**Explanation:**This task involves calculating the half-life of a second-order reaction. The given reaction is the decomposition of nitrosyl bromide (NOBr) into nitrogen monoxide (NO) and bromine (Br₂). A specific rate constant is provided, and the initial concentration of NOBr is given. To calculate the half-life of a second-order reaction, the formula:\[ t_{1/2} = \frac{1}{k [A]_0} \]is used, where:- \( k \) is the rate constant,- \([A]_0\) is the initial concentration of the reactant.No graphs or diagrams are provided in the image.

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Enter your answer in the provided box. The rate constant for the following second-order reaction is 0.80/(M - s) at 10°C. 2NOBR(g) → 2NO(g) + Br2(g) Calculate the half-life when [NOB1]o = 0.134 M.

Chemistry

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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

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Question

**Transcription for Educational Website:**

---

**Enter your answer in the provided box.**

The rate constant for the following second-order reaction is 0.80 /(M · s) at 10°C.

\[ 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \]

Calculate the half-life when \([\text{NOBr}]_0 = 0.134 \, M.\)

\[ \boxed{ \; \; \; \; } \, s \]

---

**Explanation:**

This task involves calculating the half-life of a second-order reaction. The given reaction is the decomposition of nitrosyl bromide (NOBr) into nitrogen monoxide (NO) and bromine (Br₂). A specific rate constant is provided, and the initial concentration of NOBr is given.

To calculate the half-life of a second-order reaction, the formula:

\[ t_{1/2} = \frac{1}{k [A]_0} \]

is used, where:
- \( k \) is the rate constant,
- \([A]_0\) is the initial concentration of the reactant.

No graphs or diagrams are provided in the image.

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