Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Problem Statement:**
Given that \( K_p = 7.3 \times 10^{-6} \) for the reaction below at 400.0 K, determine the value of \( K_c \).
The gas constant \( R = 0.0821 \, \text{L} \cdot \text{atm/mol} \cdot \text{K} \).
**Chemical Reaction:**
\[ 2 \text{NBr}_3 \, (g) \rightleftharpoons \text{N}_2 \, (g) + 3 \text{Br}_2 \, (g) \]
**Concepts Used:**
The relationship between \( K_p \) and \( K_c \) is given by the equation:
\[ K_p = K_c (RT)^{\Delta n} \]
where:
- \( R \) is the gas constant,
- \( T \) is the temperature in Kelvin,
- \( \Delta n \) is the change in moles of gas (moles of products - moles of reactants).](https://content.bartleby.com/qna-images/question/055086f6-4d26-404b-b10d-4e78791428d4/f2f6bb5c-307e-46ef-bfb1-f445f0550742/mhneg0aa_processed.jpeg)
Transcribed Image Text:**Problem Statement:**
Given that \( K_p = 7.3 \times 10^{-6} \) for the reaction below at 400.0 K, determine the value of \( K_c \).
The gas constant \( R = 0.0821 \, \text{L} \cdot \text{atm/mol} \cdot \text{K} \).
**Chemical Reaction:**
\[ 2 \text{NBr}_3 \, (g) \rightleftharpoons \text{N}_2 \, (g) + 3 \text{Br}_2 \, (g) \]
**Concepts Used:**
The relationship between \( K_p \) and \( K_c \) is given by the equation:
\[ K_p = K_c (RT)^{\Delta n} \]
where:
- \( R \) is the gas constant,
- \( T \) is the temperature in Kelvin,
- \( \Delta n \) is the change in moles of gas (moles of products - moles of reactants).
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