A mixture of isobutylene ((CHs):CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH.);CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:):CCH:(g) + HCI(g)
A mixture of isobutylene ((CHs):CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH.);CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:):CCH:(g) + HCI(g)
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![A mixture of isobutylene \((\text{(CH}_3\text{)}_2\text{CCH}_2, 0.400 \text{ bar partial pressure})\) and HCl \((0.600 \text{ bar partial pressure})\) is heated at 500.0 K. The equilibrium constant \(K\) for the gas-phase thermal decomposition of tert-butyl chloride \((\text{(CH}_3\text{)}_3\text{CCl})\) is 3.45 at 500.0 K.
\[\text{(CH}_3\text{)}_3\text{CCl(g)} \rightleftharpoons \text{(CH}_3\text{)}_2\text{CCH}_2\text{(g)} + \text{HCl(g)}\]
Calculate the value of \(K_c\).
---
In the provided scenario, the equilibrium constant \(K\) is calculated for a reaction at 500.0 K. Partial pressures of the reactants and products are given, and \(K\) for the gas-phase decomposition reaction is known.
To proceed with the calculation:
- Use the given equilibrium constant \(K\) to determine the concentration-based equilibrium constant \(K_c\).
- Ensure you understand the relationship between \(K_p\) (calculated using partial pressures) and \(K_c\) (calculated using concentrations) for gas-phase reactions, which involves the equation \(K_p = K_c(RT)^{\Delta n}\), where \(\Delta n\) is the change in moles of gas, \(R\) is the universal gas constant, and \(T\) is the temperature in Kelvin.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1243504b-5612-4510-ba6c-7b5ec7c70d6e%2F2cac7052-0cf5-480b-b878-1bec62cc9c26%2Fxi9911m_processed.png&w=3840&q=75)
Transcribed Image Text:A mixture of isobutylene \((\text{(CH}_3\text{)}_2\text{CCH}_2, 0.400 \text{ bar partial pressure})\) and HCl \((0.600 \text{ bar partial pressure})\) is heated at 500.0 K. The equilibrium constant \(K\) for the gas-phase thermal decomposition of tert-butyl chloride \((\text{(CH}_3\text{)}_3\text{CCl})\) is 3.45 at 500.0 K.
\[\text{(CH}_3\text{)}_3\text{CCl(g)} \rightleftharpoons \text{(CH}_3\text{)}_2\text{CCH}_2\text{(g)} + \text{HCl(g)}\]
Calculate the value of \(K_c\).
---
In the provided scenario, the equilibrium constant \(K\) is calculated for a reaction at 500.0 K. Partial pressures of the reactants and products are given, and \(K\) for the gas-phase decomposition reaction is known.
To proceed with the calculation:
- Use the given equilibrium constant \(K\) to determine the concentration-based equilibrium constant \(K_c\).
- Ensure you understand the relationship between \(K_p\) (calculated using partial pressures) and \(K_c\) (calculated using concentrations) for gas-phase reactions, which involves the equation \(K_p = K_c(RT)^{\Delta n}\), where \(\Delta n\) is the change in moles of gas, \(R\) is the universal gas constant, and \(T\) is the temperature in Kelvin.
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