Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Consider the reaction:
\[ \text{P (s)} + \frac{3}{2}\text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_3 \text{(g)} \]
Write the equilibrium constant for this reaction in terms of the equilibrium constants, \( K_1 \) and \( K_2 \), for the reactions below:
\[ \text{P (s)} + \frac{5}{2}\text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_5 \text{(g)} \quad K_1 \]
\[ \text{PCl}_3 \text{(g)} + \text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_5 \text{(g)} \quad K_2 \]
*For answers with both a subscript and a superscript, enter the subscript first. For example, enter \( K_1^2 \) if the first equilibrium constant should be squared.*
\[ K = \boxed{} \]](https://content.bartleby.com/qna-images/question/f0a8a901-2497-4ce7-b3d7-44550ff0e1ad/b349d9b1-e004-4950-b9b5-8a7564a96b86/dydtgpy_processed.png)
Transcribed Image Text:Consider the reaction:
\[ \text{P (s)} + \frac{3}{2}\text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_3 \text{(g)} \]
Write the equilibrium constant for this reaction in terms of the equilibrium constants, \( K_1 \) and \( K_2 \), for the reactions below:
\[ \text{P (s)} + \frac{5}{2}\text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_5 \text{(g)} \quad K_1 \]
\[ \text{PCl}_3 \text{(g)} + \text{Cl}_2 \text{(g)} \rightleftharpoons \text{PCl}_5 \text{(g)} \quad K_2 \]
*For answers with both a subscript and a superscript, enter the subscript first. For example, enter \( K_1^2 \) if the first equilibrium constant should be squared.*
\[ K = \boxed{} \]
![A student ran the following reaction in the laboratory at 477 K:
\[ \text{PCl}_5(\text{g}) \rightleftharpoons \text{PCl}_3(\text{g}) + \text{Cl}_2(\text{g}) \]
When he introduced \(\text{PCl}_5(\text{g})\) at a pressure of 1.12 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of \(\text{PCl}_5(\text{g})\) to be 0.755 atm.
Calculate the equilibrium constant, \( K_p \), he obtained for this reaction.
\[ K_p = \] (space for answer)
The problem involves a gaseous equilibrium where phosphorus pentachloride (\(\text{PCl}_5\)) dissociates into phosphorus trichloride (\(\text{PCl}_3\)) and chlorine gas (\(\text{Cl}_2\)). The reaction was studied at a temperature of 477 K, where the initial pressure and equilibrium pressures are given. The objective is to calculate the equilibrium constant \( K_p \) based on the pressures at equilibrium.](https://content.bartleby.com/qna-images/question/f0a8a901-2497-4ce7-b3d7-44550ff0e1ad/b349d9b1-e004-4950-b9b5-8a7564a96b86/ky3cxn2_processed.png)
Transcribed Image Text:A student ran the following reaction in the laboratory at 477 K:
\[ \text{PCl}_5(\text{g}) \rightleftharpoons \text{PCl}_3(\text{g}) + \text{Cl}_2(\text{g}) \]
When he introduced \(\text{PCl}_5(\text{g})\) at a pressure of 1.12 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of \(\text{PCl}_5(\text{g})\) to be 0.755 atm.
Calculate the equilibrium constant, \( K_p \), he obtained for this reaction.
\[ K_p = \] (space for answer)
The problem involves a gaseous equilibrium where phosphorus pentachloride (\(\text{PCl}_5\)) dissociates into phosphorus trichloride (\(\text{PCl}_3\)) and chlorine gas (\(\text{Cl}_2\)). The reaction was studied at a temperature of 477 K, where the initial pressure and equilibrium pressures are given. The objective is to calculate the equilibrium constant \( K_p \) based on the pressures at equilibrium.
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