An equilibrium mixture of PC1, (g), PC13(g), and Cl₂ (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl₂ (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PC1₂(g) + Cl₂(g) =PC1, (g) Calculate the new partial pressures, P, after equilibrium is reestablished. PPCL, = T
An equilibrium mixture of PC1, (g), PC13(g), and Cl₂ (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl₂ (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PC1₂(g) + Cl₂(g) =PC1, (g) Calculate the new partial pressures, P, after equilibrium is reestablished. PPCL, = T
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![### Equilibrium Mixture and Partial Pressures
An equilibrium mixture of \( \text{PCl}_5 (g) \), \( \text{PCl}_3 (g) \), and \( \text{Cl}_2 (g) \) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of \( \text{Cl}_2 (g) \) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates.
The chemical equation for this reaction is:
\[ \text{PCl}_3 (g) + \text{Cl}_2 (g) \rightleftharpoons \text{PCl}_5 (g) \]
Calculate the new partial pressures, \( P \), after equilibrium is reestablished.
#### Partial Pressure Calculation:
\[
P_{\text{PCl}_3} = \_\_\_\_\_\_\_ \text{ Torr}
\]
\[
P_{\text{Cl}_2} = \_\_\_\_\_\_\_ \text{ Torr}
\]
\[
P_{\text{PCl}_5} = \_\_\_\_\_\_\_ \text{ Torr}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe24fc82a-b7ed-4d5f-9001-130a2252ab39%2Fd6aaee35-cece-4a6a-8991-9d60084e236c%2Fpntdnt_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium Mixture and Partial Pressures
An equilibrium mixture of \( \text{PCl}_5 (g) \), \( \text{PCl}_3 (g) \), and \( \text{Cl}_2 (g) \) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of \( \text{Cl}_2 (g) \) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates.
The chemical equation for this reaction is:
\[ \text{PCl}_3 (g) + \text{Cl}_2 (g) \rightleftharpoons \text{PCl}_5 (g) \]
Calculate the new partial pressures, \( P \), after equilibrium is reestablished.
#### Partial Pressure Calculation:
\[
P_{\text{PCl}_3} = \_\_\_\_\_\_\_ \text{ Torr}
\]
\[
P_{\text{Cl}_2} = \_\_\_\_\_\_\_ \text{ Torr}
\]
\[
P_{\text{PCl}_5} = \_\_\_\_\_\_\_ \text{ Torr}
\]
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